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Life: The Science of Biology, Tenth EditionSadava • Hillis • Heller • Berenbaum

Chapter 2: Small Molecules and the Chemistry of Life

TEST FILE QUESTIONS(By Xenia Morin)

Multiple Choice

1. The calcium phosphate enamel on teeth from an animal skeleton is found to have a high ratio of 18O to 16O. From this information it can be assumed that the animala. experienced prolonged malnutrition.b. experienced prolonged exposure to radioactivity.c. lived in a region where it rained “heavy” water.d. lived in a region where it rained “light” water.e. had a diet that was high in cholesterol-rich meat.Answer: cTextbook Reference: 2.0 Chapter IntroductionBloom’s Category: 3. Applying

2. The best reference source for the atomic number and mass number of elements isa. a good chemistry text.b. a dictionary.c. the periodic table.d. a general physics book.e. a good biology text.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

3. Which component of an atom does not significantly add to its mass?a. Protonb. Neutronc. Electrond. Both a and be. All of the aboveAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

4. What is the difference between an atom and an element?

© 2014 Sinauer Associates, Inc.

a. An atom is made of protons, electrons, and (most of the time) neutrons; an element is composed of only one kind of atom.b. An element is made of protons, electrons, and (most of the time) neutrons; an atom is composed of only one kind of element.c. An atom does not contain electrons, whereas an element does.d. An atom contains protons and electrons, whereas an element contains protons, electrons, and neutrons.e. None of the aboveAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

5. The number of protons in a neutral atom equals the number ofa. electrons.b. neutrons.c. electrons plus neutrons.d. neutrons minus electrons.e. isotopes.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

6. Which of the following statements about the atom is true?a. There are usually more protons than electrons in an atom because the negative charge of an electron is larger than the positive charge of a proton.b. The negative charge of an electron adds mass to an atom without influencing other properties.c. In an atom with a neutral charge, the number of electrons is equal to the number of protons.d. The number of electrons determines whether an atom of an element is radioactive.e. The energy level of electrons is higher in shells close to the nucleus of the atom.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

7. An atom that is neutrally charged containsa. only neutrons.b. the same number of neutrons and electrons.c. the same number of neutrons and protons.d. the same number of protons and electrons.e. no charged particles.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

8. The atomic number of an element is the same as the number of _______ in each atom.


a. neutronsb. neutrons plus electronsc. neutrons plus protonsd. protonse. protons plus electronsAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

9. The six elements most common in organisms area. calcium, iron, hydrogen, phosphorus, potassium, and oxygen.b. water, carbon, hydrogen, nitrogen, sodium, and oxygen.c. carbon, oxygen, hydrogen, phosphorus, sulfur, and nitrogen.d. nitrogen, carbon, iron, sulfur, calcium, and hydrogen.e. phosphorus, helium, carbon, potassium, hydrogen, and oxygen.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

10. Because atoms can have the same number of protons but a different number of neutrons, elements havea. isotopes.b. multiple atomic masses listed on the periodic table.c. multiple atomic numbers.d. isomerse. Both a and bAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

11. The mass number of an atom is determined primarily by the _______ it contains.a. number of electronsb. number of protonsc. sum of the number of protons and electronsd. sum of the number of protons and neutronse. number of chargesAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

12. An atom with _______ has an atomic mass of 14.a. 14 neutronsb. 14 electronsc. 7 neutrons and 7 electronsd. 7 protons and 7 electronse. 6 protons and 8 neutrons


Answer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

13. Which of the following elements has a higher atomic mass than phosphorus?a. Hydrogenb. Oxygenc. Sodiumd. Magnesiume. CalciumAnswer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

14. 3115P and 32

15P have virtually identical chemical and biological properties because they have the samea. half-life.b. number of neutrons.c. atomic weight.d. mass number.e. number of electrons.Answer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 4. Analyzing

15. Hydrogen, deuterium, and tritium all have the samea. mass number.b. atomic number.c. mass.d. radioactive decay.e. nuclear composition.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

16. The number of different natural elements found in the universe is closest toa. 18.b. 54.c. 86.d. 94.e. 146.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

17. All of the following elements occur naturally in living organisms except for


a. lithium.b. selenium.c. sodium.d. manganese.e. molybdenum.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

18. According to the periodic table, which of the following elements has the same number of outer-shell (valence) electrons as oxygen?a. Calciumb. Nitrogenc. Fluorined. Sodiume. SulfurAnswer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

19. According to the periodic table, the compound that sulfur forms with hydrogen is most like which of the following compounds?a. NH4

+

b. NH3

c. H2Od. HFe. HClAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?; 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing

20. Compared to carbon, silicon has the same number ofa. protons.b. valence (outer-shell) electrons.c. neutrons.d. electrons.e. Both a and cAnswer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

21. Which of the following elements is found in all living things?a. Nitrogenb. Phosphorusc. Sulfur


d. Carbone. All of the aboveAnswer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

22. Which of the following pairs has similar chemical properties?a. 12C and 14Cb. 12C and 40Cac. 16O and 16Nd. 1H and 22Nae. 18O and 45CaAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

23. A stable isotope of phosphorus has an atomic number of 15 and an atomic mass of 31. How many neutrons does this isotope of phosphorus have?a. 14b. 16c. 30d. 31e. 46Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

24. Hydrogen’s atomic weight is 1.00794. The reason the number is not a whole number is thata. the weight of an electron is included in the calculation.b. the average of the mass numbers, which takes into account the abundance of all the element’s isotopes, is included in the calculation.c. the mass of the neutron is not included in the calculation.d. the weight of a neutron is not a whole number.e. the calculation is dimensionless.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

25. The atomic weight of carbon is 12.011. Its mass number is 12.000. Why are these two values slightly different?a. Atomic weight does not take into account the weight of rare isotopes of the element.b. The atomic weight does not include the weight of the protons.c. The atomic weight includes the weight of the electrons.d. Atomic weight is the average of the mass numbers of a representative sample of the element, including all its isotopes.


e. The mass number of an element is always lower than its atomic weight.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

26. Calcium has an atomic number of 20 and an atomic weight of 40.08. From this information it can be determined that this elementa. forms ions.b. forms isomers.c. has at least two isotopes.d. has a pH of 7.e. None of the aboveAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 4. Analyzing

27. Carbon-12 is the most abundant isotope of carbon on Earth. Carbon-13 makes up about 1 percent of Earth’s carbon atoms, and is useful for radioimaging. Which of the following is true?a. Carbon-13 has more protons than carbon-12.b. Carbon-13 has more neutrons than carbon-12.c. Carbon-13 has more electrons than carbon-12.d. Carbon-13 has an electronic configuration that is different from that of carbon-12.e. Carbon-13 has an equal number of protons and neutrons.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

28. Nitrogen-14 and Nitrogen-15 are isotopes. Nitrogen-15 is used to determine protein structure. Which of the following is true?a. Nitrogen-15 has more neutrons than nitrogen-14.b. Nitrogen-15 has more protons than nitrogen-14.c. Nitrogen-15 has more electrons than nitrogen-14.d. Nitrogen-15 has an electronic configuration that is different from that of nitrogen-14.e. Nitrogen-15 has an equal number of protons and neutrons.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

29. What part of the atom determines how the atom reacts chemically?a. Protonb. Neutronc. Electrond. Innermost shelle. NucleusAnswer: c


Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

30. The ability of an atom to combine with other atoms is determined by the atom’sa. atomic weight.b. ability to form isomers.c. number and distribution of electrons.d. nuclear configuration.e. mass number.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

31. Which of the following elements is the most chemically reactive?a. Carbonb. Heliumc. Neond. Argone. All of the above have the same chemical reactivity.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

32. All of the elements listed below follow the octet rule except fora. hydrogen.b. chlorine.c. carbon.d. sodium.e. nitrogen.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

33. Which of the elements listed below requires two additional electrons to fill the outermost electron shell?a. Lithiumb. Carbonc. Nitrogend. Oxygene. FluorineAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

34. An atom is most stable whena. it can have one unpaired valence electron, allowing it to fulfill the octet rule.


b. it can share electrons with other atoms to form an uneven number of pairs of electrons.c. it has eight electrons.d. it can fill its outermost shell by either sharing electrons or by gaining or losing one or more electrons until is filled.e. its outermost electron shell fulfills the quartet rule.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

35. Which of the following is the correct order (in decreasing order) for the relative strengths of chemical bonds?a. Covalent, ionic, hydrogen, van der Waals forcesb. Ionic, covalent, hydrogen, van der Waals forcesc. van der Waals forces, covalent, ionic, hydrogend. Hydrogen, covalent, van der Waals forces, ionice. Ionic, covalent, van der Waals forces, hydrogenAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

36. Which of the following atoms usually has the greatest number of covalent bonds with other atoms?a. Carbonb. Oxygenc. Sulfurd. Hydrogene. NitrogenAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

37. In a hydrogen molecule, the two atoms are held together bya. hydrogen bonds.b. a shared pair of electrons.c. van der Waals forces.d. ionic attractions.e. differences in electronegativity.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

38. Which of the following statements about ionic and covalent bonds is true?a. An ionic bond is stronger than a covalent bond.b. Compared to an ionic bond, a nonpolar covalent bond has more equal electron sharing.c. An ionic bond is almost identical to a nonpolar covalent bond.d. Ionic bonds vary in length but covalent bonds are all the same length.


e. An ionic bond can have multiple bonds but a covalent bond cannot.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

39. Which of the following statements is true?a. Carbon makes the same number of covalent bonds as phosphorus does.b. Oxygen makes more covalent bonds than sulfur does.c. Sulfur makes more covalent bonds than carbon does.d. Hydrogen makes more covalent bonds than carbon does.e. Oxygen makes fewer covalent bonds than nitrogen does.Answer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

40. Oxygen forms _______ covalent bond(s), carbon forms _______, and hydrogen forms _______.a. one; four; oneb. four; four; fourc. two; four; noned. two; four; one.e. two; two; twoAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

41. The ball-and-stick structure of methane (CH4) shows that alla. bonds are hydrogen bonds.b. bond angles are the same.c. bond lengths are the same.d. Both a and be. Both b and cAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing

42. Which of the following statements about the Bohr structure of methane (CH4) is true?a. All bonds contain paired electrons shared between carbon and hydrogen.b. All bonds contain paired electrons from carbon.c. All bonds contain paired electrons from hydrogen.d. All bonds are hydrogen bonds.e. All bonds are ionic bonds.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing


43. The shapes of large biological molecules can change because the three-dimensional orientationa. of atoms depends upon bond angles, and bond angles often vary in a stable biological molecule.b. of atoms depends upon rotations around single covalent bonds.c. is dependent upon some atoms with very flexible bonds.d. is not dependent upon hydrogen bonds.e. of bonds can stretch according to electronegativity of the atoms.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 3. Applying

44. Chemical bonds formed by differences in the electronegativity of the atoms area. covalent bonds.b. ionic bonds.c. hydrogen bonds.d. van der Waals forces.e. Both b and cAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

45. A double covalent chemical bond represents the sharing of _______ electron(s).a. oneb. twoc. threed. foure. sixAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

46. Two carbon atoms held together in a double covalent bond share _______ electron(s).a. oneb. twoc. fourd. sixe. eightAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

47. All of the following are nonpolar except fora. O2.b. N2.c. CH4.


d. NaCl.e. H2.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 3. Applying

48. When magnesium (Mg) bonds with another element, ita. gains two electrons from the other element.b. shares four electrons with the other element.c. loses two electrons to the other element.d. forms a hydrogen bond.e. gains six electrons from the other element.Answer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 3. Applying

49. The two covalent bonds in a water molecule are polar becausea. oxygen is more electronegative than hydrogen.b. oxygen and hydrogen have similar electronegativities.c. oxygen is less electronegative than hydrogen.d. water a small molecule.e. water is hydrophilic.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

50. A covalent bond is formed by the sharing of _______ between atoms, whereas an ionic bond is formed by the _______.a. neutrons; sharing of electronsb. electrons; electric attraction between two neutral atomsc. protons; electric attraction between two neutral atomsd. protons; sharing of electronse. electrons; transfer of electrons from one atom to anotherAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

51. Particles that have a net negative charge are calleda. electronegative.b. cations.c. anions.d. acids.e. bases.Answer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering


52. Which of the following molecules is held together primarily by ionic bonds?a. Waterb. Sugarc. Sodium chlorided. Methanee. AmmoniaAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

53. Hydrogen bondsa. form between two hydrogen atoms.b. form only between hydrogen and oxygen atoms within a molecule.c. form between a weak electronegative atom and hydrogen.d. involve a transfer of electrons.e. form weak interactions but can provide structural stability when many are found in a single molecule.Answer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

54. Cholesterol is a lipid and most often found in cell membranes. It is composed primarily of carbon and hydrogen atoms and has the following chemical formula: C27H46O. Based on this information, one would expect cholesterol to bea. insoluble in water.b. a highly polar molecule.c. a cation.d. an anion.e. insoluble in hexane.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 5. Evaluating

55. Hydrogen bonds are attractionsa. between oppositely charged ions.b. between atoms resulting in electron sharing.c. between cations.d. between atoms each with partial electrical charges.e. that rely upon hydrophobic interactions.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

56. A van der Waals interaction is an attraction betweena. two nonpolar molecules, due to the exclusion of water.


b. the electrons of one molecule and the nucleus of the same molecule.c. the electrons of one molecule and the protons of a nearby molecule.d. two adjacent nonpolar molecules, due to variations in their electron distribution.e. two polar molecules, because they are surrounded by water molecules.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

57. In addition to covalent and ionic bonds, _______ are important in biological systems.a. van der Waals interactionsb. hydrogen bondsc. hydrophobic interactionsd. Both a and be. All of the aboveAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

58. Which of the following statements about biochemical reactions is false?a. They obey the rules of chemistry and physics.b. They must always balance the number of atoms in the reactants and the products.c. They can create new energy during the reaction.d. They can store energy in the form of a covalent bond.e. They can change the form of energy found in the cell.Answer: cTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 2. Understanding

59. Which statement about the following reaction is true?C3H8 + 5 O2 3 CO2 + 4 H2O + energya. O2 is a product.b. The reaction is reversible.c. The reaction is balanced.d. Energy is needed for this reaction to occur.e. All of the aboveAnswer: cTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 3. Applying

60. Two characteristics of water make it different from most other compounds: Its solid state is _______ its liquid state, and it takes up _______ heat as it changes to its gaseous state.a. less dense than; large amounts ofb. more dense than; small amounts ofc. less dense than; small amounts ofd. more dense than; large amounts of


e. just as dense as; noAnswer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

61. Which characteristic of water contributes most to the relatively constant temperatures of the oceans?a. Water has the ability to ionize slightly.b. Water has a high specific heat.c. Salt water has low surface tension.d. Salt water is denser than fresh water.e. Water requires a small amount of heat energy to raise its temperature.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

62. Ice floats because the ice crystalsa. take up more space than the liquid water.b. are more dense than liquid water.c. form heat, which makes water expand.d. can move quickly and therefore can float.e. have a high surface tension.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

63. In the summer, ice is used to cool beverages primarily because ita. is composed only of water.b. floats.c. dilutes the taste.d. is inexpensive.e. absorbs a lot of heat when it melts.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

64. The amount of energy required to heat 20 g of water by 3°C isa. greater than the amount of heat required to heat 10 g of water by 6°C.b. less than the amount of heat required to heat 10 g of water by 6°C.c. the same as the amount of heat required to heat 5 g of water by 12°C.d. less than the amount of heat required to heat 30 g of water by 1°C.e. less than the amount of energy given off when 20 g of water cools by 3°C.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying


65. Which of the following correctly states an unusual property of water?a. Water will not react with other atoms.b. Solid water (ice) is denser than liquid water.c. The conversion of water from its solid to its liquid state does not require energy.d. Little heat energy is needed to raise the temperature of water.e. The hydrogen bonds between water molecules continually form and break.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

66. When exposed to extreme heat, the human body relies on _______ to absorb excess calories of heat and maintain normal body temperature.a. evaporationb. condensationc. respirationd. transpiratione. All of the aboveAnswer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

67. Surface tension and cohesion occur in pure water because watera. forms nonpolar bonds.b. forms ionic bonds.c. resists the breaking of hydrogen bonds.d. forms weak bonds.e. resists the breaking of ionic bonds.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

68. H2SO4 can ionize completely to yield two H+ ions and one SO42– ion. H2SO4 is

therefore aa. weak base.b. strong base.c. buffer.d. weak acid.e. strong acid.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

69. To determine the number of molecules in a teaspoon of sugar you have to knowa. the weight of the sugar.b. the weight and density of the sugar.c. the molecular weight of the sugar.


d. Avogadro’s number.e. the weight and molecular weight of the sugar, and Avogadro’s number.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

70. When 0.1 mole of sodium hydroxide (NaOH) is added to 1 liter of water, it ionizes, releasing OH– and Na+ ions. The resulting solution isa. acidic.b. basic.c. neutral.d. molar.e. a buffer.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

71. A mole of hydrogen and a mole of carbon havea. different numbers of molecules.b. fewer numbers of hydrogen atoms than carbon atoms.c. the same number of molecules.d. the capacity to form one mole of carbohydrate.e. a different number of molecules that a mole of oxygen.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

72. Which of the following compounds containing 1H, 12C, and/or 16O has the greatest number of molecules in a sample with a mass of 2 grams?a. Water (H2O)b. Carbon dioxide (CO2)c. Acetic acid (CH3OOH)d. Carbonic acid (H2CO3)e. Table sugar (C12H22O11)Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

73. The difference between an acid and a base is that an acid _______, whereas a base _______.a. undergoes a reversible reaction; does notb. releases OH– ions in solution; accepts OH– ionsc. releases H+ ions in solution; accepts H– ionsd. releases OH– ions in solution; releases H+ ionse. releases H+ ions in solution; accepts H+ ionsAnswer: e


Textbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

74. How would you make 100 ml of an aqueous solution with a 0.25 M concentration of a compound that has a molecular weight of 200 daltons?a. Add 25 grams of the compound to 100 ml of water.b. Add 20 grams of the compound to 100 ml of water.c. Measure 2.5 grams of the compound and add water until the volume equals 100 ml.d. Measure 2 grams of the compound and add water until the volume equals 100 ml.e. Measure 5 grams of the compound and add water until the volume equals 100 ml.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

75. Which of the following has the greatest concentration of hydrogen ions?a. Household ammonia at pH 11b. Baking soda at pH 9c. Human blood at pH 7d. Black coffee at pH 5e. Cola at pH 3Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

76. The optimum soil pH for growing strawberries is 6.5, whereas the optimum soil pH for growing blueberries is 4.5. Therefore, the number of hydrogen ions needed to grow strawberries is _______ times the number needed for blueberries.a. 2b. 10c. 100d. 1,000e. 1,000,000Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 4. Analyzing

77. Which of the following statements comparing a solution of lemon juice (pH ~2) to a solution of tomato juice (pH ~4) is true?a. The lemon juice has more hydroxyl ions per liter.b. The lemon juice has more hydrogen acceptors per liter.c. The lemon juice has more H+ ions per liter.d. The lemon juice has a higher pH.e. None of the aboveAnswer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying


78. Carbonic acid and sodium bicarbonate act as buffers in the blood. When a small amount of acid is added to this buffer, the H+ ions are used up as they combine with the bicarbonate ions. When this happens, the pH of the blooda. becomes basic.b. becomes acidic.c. does not change.d. is reversible.e. ionizes.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 4. Analyzing

79. Solutions that contain buffers tend to resist pH changes because buffersa. are bases.b. change from ionic to nonionic in solution.c. change from nonionic to ionic in response to changes in pH and release or absorb H+.d. are weak acids or bases.e. are ionic polar molecules that add or absorb H+ in solutions.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

80. A solution with pH 9 containsa. more H+ ions than OH– ions.b. more OH– ions than H+ ions.c. the same number of OH– ions and H+ ions.d. no OH– ions.e. only H– ions.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

81. A 1.0 M solution of HCl has a pH ofa. 1.0.b. 3.5.c. 7.0.d. 11.2.e. 14.0.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

82. A substance with a pH of 6.0 containsa. more OH– than H+.b. 610 hydrogen ions.


c. 610 moles of hydrogen ions.d. 10–6 moles of hydrogen ions.e. 106 moles of hydrogen ions.Answer: dTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

83. Acid rain is a serious environmental problem. A sample of rainwater collected in the Adirondack Mountains had an H+ concentration of 1.0 ×10–4 mol/L. The pH of this sample wasa. 0.0001.b. –4.c. 4.d. 1.e. 10,000.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

Fill in the Blank

1. The mass of a _______ serves as the standard unit of measure for one dalton (Da). A _______ also has a mass of about 1 Da.Answer: proton; neutronTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

2. Oxygen and carbon are defined as different elements because they have atoms with a different number of _______ in the nucleus.Answer: protonsTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

3. Every atom except for _______ has one or more neutrons in its nucleus.Answer: hydrogenTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

4. Based on the periodic table, the molecular weight of glucose (C6H12O6), to the nearest round number, is _______.Answer: 180Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?;2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 3. Applying


5. An element’s _______ takes into account the abundances of the naturally occurring isotopes.Answer: atomic weight (or relative atomic mass)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

6. _______ occurs when a radioisotopic atom is transformed into another atom, with an accompanying emission of energy in the form of alpha, beta, or gamma radiation.Answer: Radioactive decayTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

7. The chemical properties of an element are determined by the number of _______ in the atom’s _______.Answer: electrons; valence shell (or outermost shell)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

8. The tendency of atoms in stable molecules to have eight electrons in their outermost shells is known as the _______.Answer: octet ruleTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

9. A _______ links two or more atoms through attractive forces to create a molecule.Answer: chemical bondTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

10. Of the different types of chemical bonds, the strongest bond in biological systems is the _______ bond.Answer: covalentTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

11. An atom’s electronegativity depends on how many _______ charges it has, and on the distance between the _______ and the valence electrons.Answer: positive; nucleusTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

12. Oxygen, which has an electronegativity of 3.5, will have a stronger attraction for _______ compared to carbon, which has an electronegativity of 2.5.Answer: electrons (or valence electrons)Textbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding


13. The electric charge in_______ covalent bonds is unequally distributed because one nucleus has a stronger attraction for the electrons than the other has.Answer: polarTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

14. When two nonpolar molecules are in close proximity, their interactions are enhanced by _______.Answer: van der Waals forcesTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

15. A _______ bond forms when there is an attraction between a partial positive charge on a hydrogen atom involved in a polar covalent bond and a partial negative charge on a nearby electronegative atom.Answer: hydrogenTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

16. In the equation C6H12O6 6 CO2 + 6 H2O, C6H12O6 functions as the _______.Answer: reactantTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 2. Understanding

17. The amount of heat needed to raise one gram of a substance by 1°C is known as _______ heat.Answer: specificTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 1. Remembering

18. One mole of a substance contains 6.02 × 1023 molecules. This number is known as _______.Answer: Avogadro’s numberTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 1. Remembering

19. The water strider skates along the surface of water due to a property of liquids called _______.Answer: surface tensionTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

20. A chemical reaction that can proceed in either direction is called a(n) _______ reaction.Answer: reversible


Textbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 1. Remembering

21. Prolactin is a peptide hormone produced by the pituitary gland that stimulates breast and milk development in pregnant women. The normal prolactin concentration in a pregnant woman’s blood is 10‒209 ng/mL. Because prolactin’s molecular weight is 22,000 g/mol, a concentration of 110 ng/mL is equivalent to a concentration of 5 nM (nanomolar). Compared to the concentration of most molecules in the blood, the concentration of prolactin is significantly _______.Answer: lowerTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 4. Analyzing

22. If the pH of an acid rain sample is 2.5 pH units more acidic than water, the acid rain sample has a pH of _______.Answer: 4.5Textbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

23. Blood contains bicarbonate ions and carbonic acid and prevents significant changes in pH in the body because it acts as a(n) _______.Answer: bufferTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

24. The law of _______ is an important chemical principle of reversible reactions.Answer: mass actionTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 1. Remembering

25. A urine sample taken from a patient suffering from a kidney stone is found to have a pH of 5.5. Acidic urine is associated uric acid or cystine stones. Alkaline urine is associated with calcium- and phosphate-containing stones. The patient’s kidney stone most likely contains _______ crystals.Answer: uric acid or cystineTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

Diagram

1.‒3. Refer to the figure below showing part of the periodic table.


1. Which element has an atomic number of 15?Answer: Phosphorus (P)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

2. Which element has the same number of valence electrons as silicon (Si)?Answer: Carbon (C)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

3. Which elements shown in the figure have complete outer shells?Answer: Helium (He), neon (Ne), and argon (Ar)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

4.‒7. Refer to the figure below showing Bohr models of five elements.


4. Which of the diagrams represents magnesium (Mg; atomic number 12)?Answer: BTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

5. Which of the diagrams represents a stable atom, and which element is it?Answer: E; argon (Ar)Textbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

6. Which of the diagrams shows an atom that will lose electrons to form a stable ion?Answer: Both A and BTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

7. Which of the following represents the correct ordering of the atoms shown in the figure, from lowest electronegativity to highest electronegativity?


a. A < B < C < D < Eb. B < C < E < D < Ac. C < B < D < A < Ed. D < E < A < B < Ce. E < D < B < A < CAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 4. Analyzing

8.‒10. Refer to the figure below showing the electron shells and orbitals.

8. Which orbital(s) is/are an s orbital?Answer: Orbitals A and BTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

9. Which orbital(s) is/are a py orbital?Answer: Orbital DTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

10. A nitrogen atom (atomic number 7) will contain which orbitals found in the figure?Answer: Orbitals A, B, C, and DTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

11.‒12. Refer to the figure below showing various chemical bonds and interactions.


11. Which of the following represents the correct order of relative strengths, from weakest to strongest, of the bonds and interactions shown in the figure?a. E < D < A < B < Cb. E < A < C = B < Dc. D < B < C < A < Ed. B = C < A < E < De. E < C = B < A < DAnswer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing

12. Nonpolar molecules would likely exhibit which type of bonds or interactions?Answer: A or ETextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

13.‒15. Refer to the figure below showing the chemical structure of several molecules.

13. Which molecule is a hydrocarbon?Answer: OctaneTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing

14. Which of the molecules are most likely to be miscible (soluble in each other)?a. Octane and waterb. Water and methanolc. Amino acid and octaned. Methanol and octanee. Amino acid and methanol


Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 4. Analyzing

15. Which molecule is an ion?a. Octaneb. Waterc. Methanold. Amino acide. None of the aboveAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

16.‒17. Refer to the figure below.

16. The product(s) of the reaction shown in the figure is/area. CO2.b. H2O.c. heat and light.d. Both a and be. All of the aboveAnswer: eTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 2. Understanding


17. Why is the reaction shown in the figure a balanced equation?Answer: It is a balanced equation because an equal number of atoms are found in the reactants and products. Matter is neither created nor destroyed. For example, the total number of carbon atoms (black), oxygen atoms (red), and hydrogen atoms (white/grey) on the left side of the equation are equal to the total number of C, N, and H atoms on the right side.Textbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 2. Understanding

18.‒19. Refer to the figure below.

18. Which part of the diagram refers to the buffering range?a. The red zoneb. The blue zonec. The area above the top dotted lined. The area between the dotted linese. The area below the bottom dotted lineAnswer: dTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding

19. Which part of the diagram has the largest H+ change per unit of base added?a. The area between the dotted linesb. The area between pH 2 and pH 4c. The area between pH 4 and pH 6d. The area between pH 6 and pH 8


e. Both the area between pH 2 and pH 4 and the area between pH 6 and pH 8Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 4. Analyzing

DIAGNOSTIC QUIZ QUESTIONS (from BioPortal)(By Xenia Morin)

1. Which of the following statements about isotopes is false?a. Isotopes vary in the number of neutrons but not protons.b. Carbon-13 and heavy oxygen are common elements used in isotope analysis.c. Isotopes have the same atomic number but not the same atomic weight.d. Deuterium is an isotope of hydrogen containing 1 proton and 2 neutrons.e. Isotopes have virtually the same chemical reactivity.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

2. Isotopic analysis of biological samples can be a useful tool in the study ofa. the diets of humans.b. the diets of ancient animals.c. migration patterns of ancient people.d. migration patterns of dinosaurs.e. All of the aboveAnswer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 3. Applying

3. Which of the following best describes the difference between an element and a molecule?a. An element is composed of atoms; a molecule is not.b. An element is unstable; molecules are stable.c. An element is composed of only one kind of atom; molecules can be composed of more than one kind of atom.d. Elements always have lower atomic weights than molecules.e. Elements exist in nature only as parts of molecules.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

4. The reactivity of an atom arises from thea. energy difference between the s and p orbitals.b. presence of unpaired electrons in the outermost electron shell or valence shell.c. s-orbital rather than the p-orbital electron shell configuration.d. sum of the potential energies of all electron shells.


e. potential energy of the outermost electron shell or valence shell.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

5. An element that contains 10 protons and 10 electrons is likely toa. form covalent bonds with another element.b. form ionic bonds with another element.c. be chemically inert (stable).d. be radioactive.e. be toxic.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?; 2.2 How Do Atoms Bond to Form Molecules?; 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 4. Analyzing

6. Covalent bond formation depends on the ability of atoms to _______ other atoms.a. share one or more pairs of electrons withb. donate electrons toc. receive electrons fromd. share neutrons withe. donate protons toAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

7. Which of the following interactions between atoms is the strongest?a. Hydrophobic interactionsb. Ionic attractionc. Covalent bondsd. van der Waals forcese. Hydrogen bondsAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

8. Rank the elements carbon (C), hydrogen (H), oxygen (O), and phosphorus (P) in decreasing order of the number of covalent bonds they usually form.a. C > P > N > O > Hb. P > O > C > N > Hc. P > C > N > O > Hd. P > C > O > N > He. P > C > O > H > NAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?


Bloom’s Category: 1. Remembering

9. For a covalent bond to be polar, the two atoms that form the bond must havea. differing atomic weights.b. differing numbers of neutrons.c. differing melting points.d. differing electronegativities.e. similar electronegativities.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

10. Polar moleculesa. have bonds with an unequal distribution of electric charge.b. must form ions in water solution.c. have bonds with an equal distribution of electrical charge.d. have bonds with an overall negative charge.e. have bonds with an overall positive charge.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

11. Solid salt, NaCl, is neutral. When dissolved in water, NaCla. remains as NaCl (does not dissociate).b. dissociates to form Na– and Cl+.c. dissociates to form Na+ and Cl– ions that do not interact with water molecules.d. dissociates to form Na+ and Cl– ions that do interact with water molecules.e. does not dissociate, but interacts with water molecules.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

12. Hydrocarbons are _______ and _______, whereas salts are _______ and _______.a. nonpolar; hydrophobic; polar; hydrophilicb. nonpolar; hydrophilic; polar; hydrophobicc. polar; hydrophilic; nonpolar; hydrophobicd. polar; hydrophobic; nonpolar; hydrophilice. None of the aboveAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

13. Propane (CH3—CH2—CH3), is considered a nonpolar molecule because ita. has more attraction to water than to other propane molecules.b. has more attraction to other propane molecules than water.c. is a gas.


d. can undergo a chemical reaction with oxygen.e. forms hydrogen bonds.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

14. Which of the following structures is depicted incorrectly?

a.

b.

c.

d.

e. Answer: aTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 4. Analyzing

15. Which of the following statements about chemical reactions is false?a. They occur when atoms combine or change their bonding partners.b. They may lead to the destruction or creation of energy.c. They may go to completion.d. They may lead to changes in forms of energy.e. They convert reactants into products.Answer: bTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Bloom’s Category: 2. Understanding

16. Sweating is a useful cooling device for humans because watera. absorbs a great deal of heat in changing from its liquid state to its gaseous state.b. absorbs a great deal of heat in changing from its solid state to its liquid state.c. can exist in three states at temperatures common on Earth.d. is an outstanding solvent.e. ionizes readily.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 2. Understanding


17. Which of the following properties of water contributes most to the ability of fish in lakes to survive very cold winters?a. Water is cohesive.b. Water has a high heat capacity.c. Frozen water is more dense than liquid water.d. Frozen water is less dense than liquid water.e. Water forms hydrogen bonds.Answer: dTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

18. The molecular weight of acetic acid is 60. How much acetic acid would you need to prepare 10 ml of a 0.001 M (1.0 mM) solution?a. 6.0 gb. 0.6 mgc. 0.0006 gd. 0.06 mge. 0.006 gAnswer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

19. Given that Avogadro’s number is 6.02 × 1023, how many molecules of KCl are there in 10–13 liter of a 1 M KCl solution?a. 6.02 × 1036

b. 6.02 × 1010

c. 6.02 × 10–10

d. 6.02 × 103

e. 6.02 × 1013

Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 3. Applying

20. Why is the pH of a 0.1 M solution of acetic acid in water higher than that of a 0.1 M solution of HCl in water?a. HCl is a weaker acid than acetic acid.b. The acetic acid does not fully ionize in water, whereas HCl does.c. HCl does not fully ionize in water, whereas acetic acid does.d. Acetic acid is a better buffer than HCl.e. Acetate (ionized acetic acid) is a strong base.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Bloom’s Category: 4. Analyzing


LEARNINGCURVE QUESTIONS (from BioPortal)(By Xenia Morin)

1. Living organisms obey the same laws of _______ and _______ as everything else on our planet.a. chemistry; physicsb. biology; chemistryc. biology; physicsd. mathematics; physicse. mathematics; chemistryAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 2. Understanding

2. Biological organisms are made ofa. atoms, elements, water, other molecules, and ions.b. atoms, water, and other molecules.c. water, other molecules, and cations.d. only the elements C, N, P, K, and S.e. only the elements C, N, O, P, K, and S.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering

3. A helium atom containsa. a very large nucleus by volume.b. electrons that have a mass similar to that of protons.c. two hydrogen molecules.d. two positively charged neutrons.e. two negatively charged electrons.Answer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering

4. Which particles determine how an atom interacts with other atoms?a. Protonsb. Neutronsc. Electronsd. Nucleie. BosonsAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: Easy



5. The Bohr model of an atom does not emphasizea. the electron shells.b. the pairing of electrons in different electron shells.c. the number of reactive electrons.d. the relationship between s orbitals and p orbitals.e. the number of electrons in the valence shell.Answer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 2. Understanding

6. Which six elements provide most of the mass of biological organisms?a. C, O, N, H, P, Sb. K, O, N, H, P, Cc. C, O, Na, H, P, Sd. C, O, N, H, F, Mge. C, O, N, H, P, MgAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering

7. _______ is the heaviest isotope of the element whose atomic number is 1.a. Hydrogenb. Deuteriumc. Tritiumd. Heliume. TitaniumAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 1. Remembering

8. Atoms are generally charged and have mass. This statement isa. true, because all atoms have mass and have protons.b. true, because all atoms have mass and have electrons.c. false, because atoms have mass and have neutrons, which cancel out the charge.d. false, because atoms have mass but also have equal numbers of protons and electrons, which results in no (net) charge.e. Both a and bAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 1. Remembering


9. Which molecule or molecules has an atomic weight of approximately 16?a. Methane (CH4)b. Water (H2O)c. Oxygen gas (O2)d. Both a and be. Both a and cAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 3. Applying

10. In which column/group in the periodic table would you expect to find elements with five valence electrons?a. The group that starts with Beb. The group that starts with Bc. The group that starts with Nd. The group that starts with Fe. None of the aboveAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 3. Applying

11. In the periodic table, when elements are in the same vertical column, they share a similara. atomic mass.b. number of neutrons.c. number of valence electrons.d. number of unstable isotopes.e. number of protons.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering

12. Another term for atomic weight isa. relative atomic mass.b. atomic mass.c. atomic number.d. isotopic mass.e. Both a and dAnswer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering


13. Oxygen (O) has an atomic number of 8. What is the approximate atomic mass of an oxygen atom in daltons?a. 8b. 12c. 16d. 20e. 24Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 2. Understanding

14. Which describes the most significant relationship between radioactive decay and a radioactive isotope?a. Radioactive decay changes the form of the radioactive isotope.b. Radioactive decay sometimes releases mass, which changes the form of the radioactive isotope.c. Radioactive decay sometimes releases protons, which changes the radioisotope to a new element.d. Radioactive decay changes the form of the stable isotope.e. Radioactive decay sometimes releases protons, which changes the stable atom to a new element.Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 2. Understanding

15. Which of the following sets of elements, when their symbols are read in the order provided, spells a word?a. Carbon, oxygen, fluorine, iron, nitrogen, sulfurb. Barium, cobalt, nitrogenc. Germanium, nickel, iodine, uranium, sulfurd. Calcium, fluorine, phosphorus, iodine, neone. Potassium, argon, sulfurAnswer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 3. Applying

16. In the periodic table, phosphorus has an atomic weight, or relative atomic mass, of 30.947. The three main isotopes of phosphorus are P-31, P-32, and P-33. If the atomic number for phosphorus is 15, why is the relative atomic mass not 30?a. Phosphorus has one stable and abundant isotope, P-31, which has one additional neutron that adds approximately one unit in mass.b. Phosphorus has many electrons that add mass.


c. Phosphorus’s radioisotopes decay, producing less mass than P-30.d. Phosphorus isotope P-32 is stable and contributes two neutrons that add mass.e. Phosphorus has one additional proton that adds mass.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 4. Analyzing

17. Stable isotope analysis can be a useful tool to studya. the movement of ancient people.b. the movement of ancient animals.c. the location where plants were grown.d. the sources of food in marine systems.e. All of the aboveAnswer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 4. Analyzing

18. Which orbitals would you expect to be occupied in a fluorine atom?a. 1s, 2s, 2px

b. 1s, 2s, 2px, 2py

c. 1s, 2s, 2px, 2py, 2pz

d. 1s, 2s, 2px, 2py, 2pz, 3se. 1s, 2s, 3s, 2px, 2py

Answer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 3. Applying

19. What is the maximum number of electrons contained in a single p orbital?a. 1b. 2c. 4d. 6e. 8Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 1. Remembering

20. An orbital determines the _______ and _______ of its corresponding electron shell.a. size; atomic massb. energy level; orientationc. energy level; orientation and geometryd. s orbital; p orbital


e. size; valence shellAnswer: cTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: HardBloom’s Category: 1. Remembering

21. P orbitals are nota. found in all atoms with atomic number 2 and higher.b. found in three different orientations: x, y, and z.c. dumbbell shaped.d. the location in an atom where a p electron may reside at least 90 percent of the time.e. parts of the electron shells of an atom.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 2. Understanding

22. In the periodic table, why are hydrogen, lithium, and sodium in the same column?a. They have different numbers of protons.b. They have the same number of unpaired electrons.c. They have the same number of electrons.d. The periodic table is in alphabetical order.e. They have fully filled electron shells.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: MediumBloom’s Category: 2. Understanding

23. How many electrons occupy the 2s orbital in an oxygen atom?a. 1b. 2c. 4d. 6e. 8Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Difficulty: EasyBloom’s Category: 2. Understanding

24. What is the molecular formula and approximate atomic weight of the following biological molecule?

CH3-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-COOH

a. C14H26O; 114 Dab. C12H28O4; 196 Da


c. C14H28O2; 200 Dad. C14H28O2; 228 Dae. C14H26O2; 260 DaAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 4. Analyzing

25. Which defines a compound?a. A pure substance with a fixed ratio of elements that cannot form a saltb. A pure substance with a fixed ratio of two or more elements that are combined through bondsc. A pure substance with a fixed ratio of three or more elements that are combined through bondsd. A mixturee. A molecule, such as hydrogen gasAnswer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 1. Remembering

26. Covalent bondsa. are polar but not nonpolar bonds.b. may be single, double, or triple bonds and can vary in orientation.c. share one or more electron pairs.d. Both a and be. Both b and cAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 2. Understanding

27. What is the molecular weight of C6H12O6?a. 24 Dab. 48 Dac. 120 Dad. 180 Dae. 280 DaAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 3. Applying

28. A(n) _______ is an atom that has gained or lost one or more electrons. A(n) _______ bond is created by a(n) _______ attraction between two _______ atoms.a. ion; ionic; electrical; charged


b. cation; ionic; charged; positivec. anion; ionic; electrical; negatived. ionic; van der Waals; electrostatic; chargede. anion; cation; charged; negativeAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 2. Understanding

29. What type of chemical bond connects the two carbon atoms in the molecule shown?

a. Nonpolar covalent bondb. Asymmetric bondc. Polar covalent bondd. Hydrogen bonde. Double covalent bondAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 3. Applying

30. What type of chemical bond connects the carbon and oxygen atoms in the molecule shown?

a. Nonpolar covalent bondb. Asymmetric bondc. Polar covalent bondd. Hydrogen bonde. Hydrophobic interactionAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 3. Applying

31. Which of the following is not an example of a chemical bond or interaction?a. Ionic attractionb. van der Waals interactionc. Electronegativityd. Covalent bonde. Hydrogen bondAnswer: c


Textbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 2. Understanding

32. Which of the following is false?a. Bond angles are fixed and determined by the atoms.b. In a single carbon–hydrogen bond, the bond length varies between molecules.c. A nitrogen–hydrogen triple bond and a nitrogen–hydrogen single bond share electrons in a similar way.d. The presence of multiple covalent bonds depends on the number of electrons shared between atoms.e. Covalent bonds are considered polar when there is uneven sharing of electrons.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 4. Analyzing

33. Which of the following correctly ranks the relative strengths of bonds and interactions?a. Covalent bond > ionic attraction > hydrogen bond > hydrophobic interaction > van der Waals.b. Covalent bond > ionic attraction = hydrogen bond > hydrophobic interaction > van der Waals.c. Covalent bond < ionic attraction < hydrogen bond < hydrophobic interaction < van der Waals.d. Covalent bond < ionic attraction = hydrogen bond < hydrophobic interaction < van der Waals.e. Covalent bond < ionic attraction = van der Waals < hydrophobic interaction < hydrogen bondAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 4. Analyzing

34. Hydrogen bonds are most similar toa. weak nonpolar interactions.b. covalent bonds.c. hydrophobic interactions.d. anion interactions.e. polar interactions.Answer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 4. Analyzing

35. Which of the following statements is false?


a. Covalent bonds can be polar or nonpolar.b. Hydrogen bonds form between or within molecules.c. Hydrophilic interactions are essentially the same as hydrogen bonds.d. van der Waals forces are so weak that they have no significant importance in molecular interactions.e. Hydrophobic molecules tend to aggregate together.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 4. Analyzing

36. Carbon atoms can bond _______ hydrogen atoms, and the outer shell of each hydrogen atom then contains _______ electrons.a. 2; 2b. 2; 4c. 4; 4d. 4; 2e. 8; 2Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 3. Applying

37. Which of the following is not a way to represent the structure and/or shape of a molecule?a. A polar model.b. A ball-and-stick model.c. A space-filling model.d. A Bohr model.e. A structural formula.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 1. Remembering

38. Refer to the figure below.


This is a(n) _______ illustrated using a _______ model.a. methane molecule; ball-and-stick modelb. methane molecule; space-filling modelc. methane molecule; Bohr modeld. ethane molecule; structural modele. ethane molecule; ball-and-stick modelAnswer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 3. Applying

39. A molecule’s three-dimensional shape varies by _______ without changing the bond angles or its stability.a. bending a hydrogen bondb. converting a space-filling model to a ball-and-stick modelc. converting a space-filling model to a Bohr modeld. rotating atoms around a covalent bonde. rotating atoms around an ionic bondAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 2. Understanding

40. The electronegativity of an atom is a relative measure of thea. number of electrons in an atom.b. number of electrons in the atom’s outermost electron shell.c. difference between the number of atoms and the number of protons.d. affinity an atom has for electrons and its ability to capture additional electrons.e. affinity an atom has for protons and its ability to capture additional protons.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 1. Remembering


41. Which of the following statements is true?a. A double covalent bond involves 8 electrons.b. A double covalent bond involves 4 electrons.c. A triple covalent bond is formed among 3 atoms.d. A triple covalent bond involves 12 electrons.e. None of the aboveAnswer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 2. Understanding

42. Which of the following covalent bonds would be the most polar?a. Nitrogen–oxygenb. Carbon–oxygenc. Hydrogen–oxygend. Nitrogen–hydrogene. Carbon–hydrogenAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 3. Applying

43. Which atom, sodium or chloride, is more electronegative? Which will “steal” an electron from the other?a. sodium; sodiumb. sodium; chloridec. chloride; sodiumd. chloride; chloridee. neither; neitherAnswer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: MediumBloom’s Category: 2. Understanding

44. A cation has the opposite charge from a(n)a. hydrophilic.b. anion.c. nonpolar.d. ionic interaction.e. complex ion.Answer: bTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 1. Remembering

45. Why does sodium chloride (NaCl) dissolve in water?


a. Sodium and chloride form a polar covalent bond.b. Sodium and chloride can form cations.c. Water is a polar solvent.d. Both a and be. Both b and cAnswer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 2. Understanding

46. Which of the following statements about the ionic bonds in magnesium chloride (MgCl2) is false?a. Each chlorine atoms steals one electron from the same magnesium atom.b. The charge on the magnesium atom when bonded with 2 Cl atoms is +2.c. There are two ionic bonds in magnesium chloride.d. Two magnesium atoms are involved.e. All of the above statements are true.Answer: dTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: HardBloom’s Category: 2. Understanding

47. The term hydrophobic is the opposite ofa. hydrophilic.b. hygroscopic.c. hydrochloric.d. anisotropic.e. acidophilic.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 1. Remembering

48. Van der Waals interactions are most similar toa. weak nonpolar interactions.b. product interactions.c. hydrophilic interactions.d. anion interactions.e. reactant interactions.Answer: aTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Difficulty: EasyBloom’s Category: 2. Understanding

49. Which general chemical principles can be applied to all chemical reactions?a. The number of atoms in the reactants must match the number of atoms in the products.


b. Matter can neither be created nor destroyed.c. Energy can change its form but cannot be destroyed or created.d. Both a and be. a, b, and cAnswer: eTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: EasyBloom’s Category: 1. Remembering

50. The equation C4H10 + 7 O2 4 CO2 + 6 H2O + energy is incorrect becausea. two carbon atoms are missing from the products.b. two hydrogen atoms are missing from the products.c. two carbons atoms are missing from the reactants.d. two hydrogen atoms are missing from the reactants.e. Two oxygen atoms are missing in the products.Answer: dTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: EasyBloom’s Category: 1. Remembering

51. Consider the following statement: In a chemical reaction, the properties of the products are usually similar to the reactants.a. This is true, because chemical properties don’t change much when chemical partners change.b. This is true, because redox reactions don’t change the properties.c. This is false, because the chemical properties can be significantly altered when chemical partners change.d. This is false, because a chemical reaction usually changes the mass of the reactants but not their energy.e. This is false, because energy can’t be created or destroyed.Answer: cTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: MediumBloom’s Category: 1. Remembering

52. When a chemical reaction occurs, changes in the form of _______ occur, which represents the capacity of the reaction to do _______.a. work; energyb. reactant; energyc. products; workd. reactants; productse. energy; workAnswer: eTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: MediumBloom’s Category: 2. Understanding


53. Which statement best explains how atoms change partners when propane combusts?a. Carbon breaks a bond with hydrogen and forms a bond with oxygen.b. Carbon breaks a bond with oxygen and forms a bond with hydrogen and oxygen.c. Oxygen breaks a bond with oxygen and forms a bond with hydrogen.d. Oxygen breaks a bond with oxygen and forms a bond with carbon.e. Oxygen breaks a bond with oxygen and forms a bond with carbon or hydrogen.Answer: eTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: HardBloom’s Category: 2. Understanding

54. Which will correctly balance the following combustion equation for hexane?2 CXHY + 19 O2 Z CO2 + 14 H2O + energya. X = 6, Y = 14, Z = 10b. X = 6, Y = 12, Z = 10c. X = 6, Y = 14, Z = 12d. X = 6, Y = 16, Z = 12e. X = 6, Y = 14, Z = 14Answer: cTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions?Difficulty: HardBloom’s Category: 3. Applying

55. Water has _______ nonbonding electrons pair(s) and _______ bonding electron pair(s).a. 0; 1b. 1; 1c. 1; 2d. 2; 2e. 4; 2Answer: dTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 1. Remembering

56. What is the molecular formula for a water molecule?a. H2Ob. HO2

c. H–O–Hd. H3O+ + OH–

e. None of the aboveAnswer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 1. Remembering


57. Which of the following statements is false? Water hasa. low specific heat capacity.b. the ability to form ice that floats and can insulate the water below.c. the capacity to form hydrogen bonds.d. a rigid crystalline structure below 0°C.e. the ability to dissolve polar solutes.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding

58. Why does a water molecule have a tetrahedral shape?a. Because oxygen bonds to two hydrogen atomsb. Because oxygen contains two sets of unpaired electronsc. Because oxygen contains two sets of paired electronsd. Both a and be. Both a and cAnswer: dTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding

59. If 1 calorie of energy is needed to raise 1 g of water by 1°C, what is the amount of energy needed to raise 15 g of water by 3°C?a. 3 caloriesb. 9 caloriesc. 15 caloriesd. 30 caloriese. 45 caloriesAnswer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

60. If carbon dioxide has a molecular weight of approximately 44, then 0.25 moles of carbon dioxide hasa. Avogadro’s number of molecules.b. a molecular weight of 22.c. a molecular weight of 11.d. approximately 1.5 1024 molecules.e. a molecular weight of 88.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying


61. Changes in the physical form of water lead to the release or absorption of heat energy. Which of the following statements is true?a. Water absorbs heat from the environment when changing from liquid to gas.b. Water absorbs heat from the environment when changing from liquid to solid.c. Water releases heat to the environment when changing from liquid to gas.d. Water releases heat to the environment when changing from gas to vapor.e. None of the aboveAnswer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding

62. Which of the following is false?a. Water is acidic.b. Water is a good solvent.c. Water has a high specific heat capacity.d. Water is ubiquitous in living organisms.e. Water is an important habitat for living organisms.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 1. Remembering

63. Consider the following statement: Most biochemical reactions take place in aqueous solutions.a. True, because water is the solvent in an aqueous solution and cells are full of water.b. True, because water is the reactant in the aqueous solution.c. False, because water is the reactant and cannot also be the aqueous solution.d. False, because most biochemical reactions love water.e. False because most biochemical reactions involve enzymes and not water.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding

64. The _______ in an aqueous solution is water.a. nonpolar solventb. solutec. solventd. ione. reactantAnswer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 1. Remembering


65. What is the significance of Avogadro’s number?a. It is the total number of molecules found in the world.b. It is the number of molecules in a mole.c. It is the total number of moles of any molecule found in the world.d. It is the number of molecules in 1 kg of a compound.e. None of the aboveAnswer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 2. Understanding

66. What is the molarity of 14.5 g of NaCl in 0.5 L of water?a. 0.125 Mb. 0.25 Mc. 0.5 Md. 0.75 Me. 1 MAnswer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

67. What differentiates a strong acid from a weak acid?a. A weak acid accepts H+ ions.b. Ionization of a weak acid is irreversible, whereas ionization of a strong acid is reversible.c. Ionization of a weak acid in water is incomplete, whereas ionization of a strong acid in water is complete.d. A strong acid is more basic than a weak acid.e. None of the above is correct. Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

68. Which of the following molecules can be characterized as a weak acid?a. HClb. HCO3

–

c. CH3COOHd. NH3

e. None of the aboveAnswer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding


69. The pH scale is a log scale. This means thata. a solution with pH of 7 is twice as acidic as a solution with pH of 9.b. a solution with pH of 7 is twice as acidic as a solution with pH of 5.c. a solution with pH of 7 is 10 times more acidic than a solution with pH of 9.d. a solution with pH of 7 is 10 times more acidic than a solution with pH of 5.e. a solution with pH of 7 is 100 times more acidic than a solution with pH of 9.Answer: eTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

70. If a tomato puree mixture has a hydrogen concentration of 1 10–4 M, it has a pH ofa. 3.5.b. 4.0.c. 4.5.d. 5.0.e. 5.5.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

71. The pH of pure rainwater is 5.5. Samples of rainwater were collected from two areas. The average in area A was pH 5.3, and the average in area B was pH 5.0. Which of the following statements is false?a. Pure rainwater is more acidic than pure water.b. Rainwater from area B is more basic than that from area A.c. Rainwater from area A is more acidic than pure rainwater.d. Rainwater from area B has a hydrogen ion concentration of 1 10–5 M.e. Rainwater from area A has a hydrogen ion concentration of 5 10–6 M.Answer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: HardBloom’s Category: 3. Applying

72. _______ capacity is a term used to describe the ability of a solution to prevent large changes in pH with the addition of a base or acid.a. Heatb. Bufferingc. Cohesived. Vaporizatione. FreezingAnswer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: Easy



73. An aqueous solution with a mixture of a _______ acid and its corresponding _______ is called a(n) _______.a. strong; base; molar solutionb. weak; base; bufferc. strong; acid; ionic solutiond. strong; acid; buffere. buffer; base; acidAnswer: bTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 1. Remembering

74. Buffers demonstrate which important chemical principle?a. The law of mass actionb. The law of thermodynamicsc. The law of motiond. The law of reversibilitye. The law of compoundsAnswer: aTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: EasyBloom’s Category: 1. Remembering

75. Refer to the figure below.


For the solution containing a buffer, the pH range with greatest buffering capacity isa. 2–4.b. 3–5.c. 4–6.d. 5–7.e. 6–8.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life?Difficulty: MediumBloom’s Category: 2. Understanding

STUDY GUIDE QUESTIONS(By Edward Awad)

1. Atomic number is determined by the number of _______ in an atom.a. protons and neutronsb. electronsc. neutronsd. protonse. protons, neutrons, and electronsAnswer: dTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

2. Which of the following statements concerning electrons is false?a. Electrons orbit the nucleus of an atom in defined orbitals.b. The outer shell of all atoms must contain eight electrons.c. An atom may have more than one valence shell.d. Electrons are negatively charged particles.e. All of the above are true; none is false.Answer: bTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

3. The element with which of the following atomic numbers would be most stable?a. 1b. 3c. 12d. 15e. 18Answer: eTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 4. Analyzing


4. What is the difference between an element and a molecule?a. Molecules may be composed of different types of atoms, whereas elements are always composed of only one type of atom.b. Molecules are composed of only one type of atom, whereas elements are composed of different types of atoms.c. Molecules are elements.d. Molecules always have larger atomic weights than elements have.e. Molecules do not have electrons, whereas elements do.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 1. Remembering

5. The strongest chemical bonds occur whena. two atoms share electrons in a covalent bond.b. two atoms share electrons in an ionic bond.c. hydrogen bonds are formed.d. van der Waals forces are in effect.e. there are hydrophobic interactions.Answer: aTextbook Reference: 2.1 How Does Atomic Structure Explain the Properties of Matter?Bloom’s Category: 2. Understanding

6. Any molecule that is hydrophilica. cannot form hydrogen bonds.b. is a polar molecule.c. is a nonpolar molecule.d. has a partial positive region and a partial negative region.e. Both b and dAnswer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

7. The stability of the three-dimensional shape of many large molecules is dependent ona. covalent bonds.b. ionic bonds.c. hydrogen bonds.d. van der Waals attractions.e. hydrophobic interactions.Answer: cTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 1. Remembering

8. The molecular weight of glucose is 180. If you added 180 grams of glucose to a 0.5 liter of water, what would be the molarity of the resulting solution?a. 18b. 1


c. 9d. 2e. 0.5Answer: dTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 3. Applying

9. Ice floats in water becausea. ice is less dense than water.b. there are no hydrogen bonds in ice.c. ice is denser than water.d. water has a higher heat capacity than ice.e. ice has more covalent bonds than water.Answer: aTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 1. Remembering

10. Cola has a pH of 3; blood plasma has a pH of 7. The hydrogen ion concentration of cola is therefore _______ than the hydrogen ion concentration of blood plasma.a. 4 times greaterb. 4 times smallerc. 400 times greaterd. 10,000 times greatere. 30,000 times greaterAnswer: dTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 3. Applying

11. Solution A has a pH of 2. Solution B has a pH of 8. Which of the following statements about these solutions is true?a. A is basic and B is acidic.b. A is acidic and B is basic.c. A is a base and B is an acid.d. A has a greater [OH–] than B.e. None of the aboveAnswer: bTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 4. Analyzing

12. What is the weight of one mole of glucose (C6H12O6)?a. 180 gramsb. 42 atomic mass unitsc. 96 gramsd. 342 gramse. 6.02 gramsAnswer: a


Textbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 3. Applying

13. Which of the following statements about buffers is true?a. They allow the pH of a solution to vary widely.b. They make solutions basic.c. They maintain pH homeostasis.d. They disrupt pH homeostasis.e. They make solutions more acidic.Answer: cTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 1. Remembering

14. Which of the following statements about water is true?a. Water has a low heat of vaporization.b. Water has a high specific heat.c. When water freezes, it gains energy from the environment.d. All of the abovee. None of the aboveAnswer: bTextbook Reference: 2.4 What Makes Water So Important for Life? Bloom’s Category: 1. Remembering

15. Which of the following statements about chemical reactions is true?a. The bonding partners of atoms remain constant.b. All reactions release energy as they proceed.c. The bonding partners of atoms change.d. All reactions consume energy as they proceed.e. None of the aboveAnswer: cTextbook Reference: 2.3 How Do Atoms Change Partners in Chemical Reactions? Bloom’s Category: 1. Remembering

16. Covalent bonds form whena. atoms of opposite charge are attracted to each other.b. hydrogen and oxygen interact.c. hydrophilic molecules bind hydrophobic molecules.d. electrons of nonpolar substances interact.e. atoms share electrons.Answer: eTextbook Reference: 2.2 How Do Atoms Bond to Form Molecules?Bloom’s Category: 2. Understanding

CHAPTER REVIEW QUESTIONS (from Textbook)


1. The atomic number of an elementa. equals the number of neutrons in an atom.b. equals the number of protons in an atom.c. equals the number of protons minus the number of neutrons.d. equals the number of neutrons plus the number of protons.e. depends on the isotope.Answer: bBloom’s Category: 1. Remembering

2. The mass number of an elementa. equals the number of neutrons in an atom.b. equals the number of protons in an atom.c. equals the number of electrons in an atom.d. equals the number of neutrons plus the number of protons.e. depends on the relative abundances of its electrons and neutrons.Answer: dBloom’s Category: 1. Remembering

3. Which of the following statements about the isotopes of an element is not true?a. They all have the same atomic number.b. They all have the same number of protons.c. They all have the same number of neutrons.d. They all have the same number of electrons.e. They all have identical chemical properties.Answer: cBloom’s Category: 1. Remembering

4. Which of the following statements about covalent bonds is not true?a. A covalent bond is stronger than a hydrogen bond.b. A covalent bond can form between atoms of the same element.c. Only a single covalent bond can form between two atoms.d. A covalent bond results from the sharing of electrons by two atoms.e. A covalent bond can form between atoms of different elements.Answer: cBloom’s Category: 1. Remembering

5. Which of the following statements about water is not true?a. It releases a large amount of heat when changing from liquid into vapor.b. Its solid form is less dense than its liquid form.c. It is the most effective solvent for polar molecules.d. It is typically the most abundant substance in a living organism.e. It takes part in some important chemical reactions.Answer: aBloom’s Category: 1. Remembering

6. The reaction HCl H+ + Cl– in the human stomach is an example of the


a. cleavage of a hydrophobic bond.b. formation of a hydrogen bond.c. elevation of the pH of the stomach.d. formation of ions by dissociation of an acid.e. formation of polar covalent bonds.Answer: dBloom’s Category: 1. Remembering

7. Using the information in the periodic table (Figure 2.2), draw a Bohr model (see Figures 2.5 and 2.7) of silicon dioxide, showing electrons shared in covalent bonds.Answer:

Bloom’s Category: 3. Applying

8. Compare a covalent bond between two hydrogen atoms with a hydrogen bond between a hydrogen and an oxygen atom, with regard to the electrons involved, the role of polarity, and the strength of the bond.Answer: An easy way to answer this question is to make a simple table:

Covalent H—H Hydrogen H….O

Electrons Shared Remain with H and O

Polarity Nonpolar Polar; + at H end

Strength Stronger Weaker

Bloom’s Category: 2. Understanding

9. Use Tables 2.2 and 2.3 to determine for each of the pairs of bonded atoms below:a. whether the bond is polar or nonpolar;b. if polar, which end is d–; andc. whether the bond is hydrophilic or hydrophobic.

C–H C=O O–P C–C

Answer: C–H: nonpolar; hydrophobicC=O: polar; – at O; hydrophilicO–P: polar; – at O; hydrophilic


C–C: nonpolar; hydrophobicBloom’s Category: 2. Understanding

10. Geckos are lizards that are amazing climbers. A gecko can climb up a glass surface and stick to it with a single toe. Professor Kellar Autumn at Lewis and Clark College and his students and collaborators have shown that each toe of a gecko has millions of micrometer-sized hairs, and that each hair splits into hundreds of 200-nanometer tips that provide intimate contact with a surface. Careful measurements show that a million of these tips could easily support the animal, but it has far more. The toes stick well on hydrophilic and hydrophobic surfaces. Bending the hairs allows the gecko to detach. What kind of noncovalent force is involved in gecko sticking?Answer: This is an example of Van der Waals forces, which act over a short distance and do not involve polarity.Bloom’s Category: 4. Analyzing

11. Would you expect the elemental composition of Earth’s crust to be the same as that of the human body?Answer: The human body has the same elements as Earth’s crust but in very different proportions.Bloom’s Category: 5. Evaluating


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