Name_________________________________________Date_________________________ Period_________________Chemistry-Exam 2 Review

Unit 1- Experimentation and Measurement <10 %a. Identifying testable questions and writing hypothesesb. Identifying independent variable/dependent variable/control groupc. Safetyd. Lab Equipment-names and usee. Metric units and measurement- know prefixes and know correct units for measurements (e.g. gram for

mass, liter for volume, etc)f. Accuracy vs Precision difference and when % error appliesg. Graphing Data correctly- correctly labelled axes and correctly chosen chart typeh. Scientific Notationi. Significant Figures- in calculations and on measurement devices

1. Use the diagram to answer the question. The diagram above shows two targets that have been struck by 4 darts each. Select the statement below which is correct.

A. Target A has been hit with a high degree of precision, yet a low degree of accuracy. B. Target B has been hit with a high degree of precision, yet a low

degree of accuracy. C. Target A has been hit with a high degree of accuracy, yet a low

degree of precision. D. Target B has been hit with a high degree of accuracy, and a high degree of precision.

2. Four lab groups measured the pH of juice from a watermelon. Their results are shown in the table. The actual pH of the watermelon juice is 5.27. Which group had the greatest precision in their measurements?

a. Group 1b. Group 2c. Group 3d. Group 4

3. A student converted the speed of light from meters per second to kilometers per hour and obtained a value of 1,079,252,850 kilometers per hour (km/h). What is this speed written in scientific notation?

a. 1.07925285 × 108 km/hb. 1,079.25285 × 106 km/h

c. 10.7925285 × 108 km/hd. 1.07925285 × 109 km/h

4. Some students observed that the mass of an ice cube in a freezer decreased by half over thirty days. Which statement made by these students is a testable hypothesis?

a. The ice cube shrank in size because it was kept in the freezer for a long time.b. The ice cube lost mass because some ice molecules escaped into the gas phase.c. The ice cube shriveled up because something happened to the water molecules.d. The ice cube became smaller because that is what usually happens in cold temperatures.

Target BTarget A

Name_________________________________________Date_________________________ Period_________________Chemistry-Exam 2 Review

5. A student used a dilute hydrochloric acid (HCl) solution during a titration. The initial and final volume of the HCl are shown in the diagram. How many significant figures should be reported for the volume of HCl used during the titration?

a. 2b. 3c. 4d. 5

6. Use the data table to answer the question.

Time(minutes)

Temperature(°C)

0 -20

5 -1 10 0

15 0 20 38

Students heated a beaker of ice until the ice completely melted. They recorded the temperature of the ice every five minutes. Which graph best represents the data from the table?

a.

b.

c.

d.

Unit 2- Matter <5 %a. Intensive vs Extensive propertiesb. Physical vs Chemical propertiesc. Calculating Density (density= m/v)d. Separating Mixturese. Classifying Matter (element, compound, homogeneous mixture, heterogeneous mixture) based on

microscopic or macroscopic viewsf. Physical vs Chemical Change- know evidence, be able to identify a reactant vs productg. Conservation of matter (mass)

Name_________________________________________Date_________________________ Period_________________Chemistry-Exam 2 Review

7. Mr. Noto wants to confirm the metal used in a ring. The volume of the ring is 1.35 cubic centimeters (cm3). What is the metal composition of the ring?

a. Sterling silverb. 18 ct white goldc. Pure goldd. Platinum

8. What physical property is used in distillation to separate the components?

a. melting pointb. boiling point

c. chemical energyd. Ignition temperature

9. Which of the following substances is less dense than air?

a. Waterb. Helium

c. Iced. Gold

10. Use the table to answer the question. The table shows the procedures for and the results of two experiments using copper (II) chloride, CuCl2. Which of the following conclusions can be made based on the results of the experiments?

A. Physical changes occurred in both experiments. B. A chemical change occurred in experiment 1, and a physical change

occurred in experiment C. A physical change occurred in experiment 1, and a chemical change occurred in experiment 2 D. Chemical changes occurred in both experiments.

Unit 3- Atom and its Nucleus <5 %a. History of the atom- how has the model changed over time and why?b. Structure of the atom- what are the parts, where are they, describe them.c. Isotopes- definition and notationd. Atomic Mass calculations (weighted average)e. Types of radiation-how to block them, what causes them, what is released, writing nuclear equations, etcf. Half-Life- definition, calculations, reading graphs, how this affects real world useg. Fission vs Fusion- definition, when/where are they used, how much energy is released…

11. Evan is comparing Carbon-12 and Carbon-14 atoms. Which statement correctly compares the subatomic particles in the carbon atoms?a. The carbon-14 atom has the same number of electrons, protons, and neutrons as the carbon-12 but more mass.b. The carbon-14 atom has two more electrons than the carbon-12 atom, but they have the same number of

protons and neutrons.

Name_________________________________________Date_________________________ Period_________________Chemistry-Exam 2 Review

c. The carbon-14 atom has two more electrons and two more protons than the carbon-12 atom, but they have the same number of neutrons.

d. The carbon-14 atom has two more neutrons than the carbon-12 atom, but they have the same number of electrons and protons.

12. The half-life of a radioisotope is the amount of time it takes for

a. half the sample to decayb. all the sample to decayc. the age of an artifact to be calculatedd. detectable radiation to be absorbed

13. A 2 cm-thick piece of cardboard placed over a radiation source would be most effective in protecting against which type of radiation?

A. alpha B. beta

C. gamma D. x-ray

Unit 4- Atom and its Electrons <5 %a. Orbital diagramsb. Electron configuration-long hand and short handc. Bohr diagrams- the real onesd. Waves- parts and relationship between wavelength/frequency/energye. Electromagnetic spectrum- order, calculationsf. Flame test- what is happening?

14. Use the diagram to answer the question. The diagram shows a partial periodic table. The electron configuration of oxygen is 1s22s22p4. On the periodic table, fluorine is one space to the right of oxygen. Which of the following electron configurations represents fluorine?

A. 1s22s22p3 B. 1s22s22p5 C. 1s22s22p63s23p3 D. 1s22s22p63s23p5

Name________________________________Date_______________________ Period_______________

Unit 5- Periodic Trends ~22 %a. Lewis dot diagrams and valence electrons for elementsb. Periodic Table organization-columns, rows, historyc. Periodic Trends-atomic radius, electronegativity, ionization energyd. Cation vs Anion formatione. Properties of elements based on position in the periodic table

15. Which of these elements has the highest electronegativity?

a. Potassium (K)b. Calcium (Ca)

c. Bromine (Br)d. Krypton (Kr)

16. Use the table to answer the question.

The table above provides some information about an unidentified element. Based on this information, the unidentified element is best classified as which of the following?

A. a metal in group 1 (1A) B. a metal in group 14 (4A) C. a nonmetal in period 4 D. a metalloid in period 5

17. Alkali metals, alkaline earth metals, and aluminum all form ions with positive charges equal to

a. atomic numberb. group number

c. periodd. atomic mass

18. Which of the following atoms has the largest atomic radius?

a. Barium (Ba)b. Chlorine (Cl)

c. Iodine (I)d. Magnesium (Mg)

19. Which of the following atoms has six valence electrons?

a. Magnesium (Mg)b. Silicon (Si)

c. Sulfur (S)d. Argon (Ar)

20. What group in the periodic table has a tendency to form ions with a +2 charge?

A. Group 1 – alkali metals B. Group 2 – alkaline earth metals

C. Group 17 - halogens D. Group 18 – noble gases

21. Use the Lewis dot structures to answer the question.

What charge will the gallium atoms have if they react with the oxygen atoms to form ionic bonds? A. -3

Name________________________________Date_______________________ Period_______________B. +1 C. +2

D. +3

22. Chlorine forms a 1- ion, but sulfur forms a 2- ion. What is the main reason for this difference in these two atoms? A. Chlorine and sulfur are part of two different periods of the periodic table, and these periods will form ions with different charges.

B. Chlorine and sulfur are part of two different groups of the periodic table, and these groups will form ions with different charges.

C. Chlorine is part of the oxygen group that only needs one more electron to reach a stable electron

configuration. D. Sulfur is part of the halogen group that only needs two more electrons to reach a stable electron configuration.

23. Which of the following atoms has the largest ionization energy?

a. Barium (Ba)b. Chlorine (Cl)

c. Iodine (I)d. Magnesium (Mg)

24. Which of the following elements would form a cation?

a. Bromine (Br)b. Helium (He)

c. Lithium (Li)d. Sulfur (S)

25. Sulfur would have chemical properties most like

a. Manganeseb. Tellurium

c. Chlorined. Xenon

26. Which of the following elements is a metal?

a. Bromine (Br)b. Helium (He)

c. Lithium (Li)d. Sulfur (S)

27. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a. In, 49 protons, 49 electronsb. Zn, 30 protons, 60 electrons

c. Cs, 55 protons, 132.9 electronsd. F, 19 protons, 19 electrons

Name________________________________Date_______________________ Period_______________Unit 6- Lewis Structures ~14 %

a. Lewis dot diagrams for ionic and covalent compoundsb. Crisscross method for ionic formula writingc. Breaking the Octet Ruled. Single vs Double vs Triple bondse. Determine electron geometry (steric number) for covalent compoundsf. Determine VSEPR shapes for covalent compounds

28. Which pair of elements will form ionic bonds in a ratio of 2:1?

A. calcium (Ca) and sulfur (S) B. sulfur (S) and chlorine (Cl)

C. potassium (K) and sulfur (S) D. potassium (K) and chlorine (Cl)

29. What is the Lewis dot structure for nitrogen trifluoride (NF3) ?

A.

B.

C.

D.

30. Which Lewis dot structure accurately represents a formula unit of magnesium chloride (MgCl2)?

B.

C.

D.

E.

31. The formation of an ionic bond involves the

a. transfer of electronsb. transfer of neutrons

c. transfer of protonsd. sharing of electrons

32. Some students are modeling covalent bonds with brief descriptions and Lewis dot diagrams, using arrows to show electron movement. Which model best demonstrates covalent bonding in bromine chloride (BrCl)?

a.

b.

c.

d.

Name________________________________Date_______________________ Period_______________

33. Lacey uses R, T, X, and Z to represent four different unknown elements in the periodic table. The dots represent valence electrons. Which unknown element will most likely form an ionic bond with Fluorine?

a.

b.

c.

d.

34. Which numbered bond in the diagram represents an ionic bond? a. Bond 1b. Bond 2c. Bond 3 d. Bond 4

35. Which of the following correctly shows how carbon and hydrogen bond to form a compound? A

.

B.

C.

D.

Unit 7- Polarity and IMF ~12 %a. Determine polarity of a compound from structureb. Determine the intermolecular force (IMF) present between compoundsc. Determine polarity of a bond from electronegativityd. Predict compound properties based on IMF

36. Use the table to answer the question.

The table shows the electronegativities of four elements. Which of the following bonds is the most polar?

A. carbon-hydrogen B. hydrogen-oxygen C. fluorine-fluorine D. carbon-fluorine

37. Which statement explains why a molecule of CH4 is nonpolar?

A. The bonds between the atoms in a CH4 molecule are polar. B. The bonds between the atoms in a CH4 molecule are ionic. C. The geometric shape of a CH4 molecule distributes the charges symmetrically. D. The geometric shape of a CH4 molecule distributes the charges asymmetrically.

Name________________________________Date_______________________ Period_______________38. Which of the following has the strongest intermolecular force?

A. hexane with London Dispersion ForceB. ethanol with one H-bond

C. methane with London Dispersion ForceD. ammonia with Dipole-Dipole

39. Which compound is made up of nonpolar molecules?

a. HBrb. H2Sc. NH3

d. CH4

40. Which of these is a property of an ionic compound?

a. Low melting pointb. Poor conductor of electricity

c. Crystal shaped. Shared electrons

41. Which of these is a property of a covalent compound?

a. high melting pointb. good conductor of electricity

c. high solubilityd. Shared electrons

42. The table below lists the melting points of various substances. Based on this table, what type of substance has the highest melting point?

a. Dipole Moleculeb. Covalent Moleculec. Ionicd. Metallic

43. Based on bond type, which compound has the highest melting point?a. CH3OHb. C6H14

c. CaCl2

d. CCl4

Name________________________________Date_______________________ Period_______________Unit 8- Naming ~18 %

a. Name/write formulas for binary and ternary ionic compounds including those containing transition metalsb. Name/write formulas for covalent compoundsc. Name /write formulas for binary and ternary acids

44. What is the formula for Iron (III) Oxide?a. Fe3O2

b. I3O2

c. Fe2O3

d. FeO3

45. In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains

a. two carbon atomsb. two oxygen atoms

c. a polyatomic iond. an ionic bond

46. Zinc carbonate is an odorless, white, sand-like solid. It is used in cosmetics, lotions, porcelains, pottery, and rubber. What is the chemical formula for zinc carbonate?

A. ZnCO3 B. Zn (CO3)2

C. Zn2CO3 D. Zn3CO2

47. What is the correct name for the acid whose chemical formula is H2SO4?

A. hydrosulfuric acid B. hydrosulfurous acid

C. sulfurous acid D. sulfuric acid

48. Uranium Hexafluoride is used to extract uranium-235 (U-235) from uranium to make the fuel for nuclear reactors and to make nuclear bombs. What is the chemical formula of uranium hexafluoride?

A. UFB. UHF

C. UF6

D. U2H6

49. Carbon tetrachloride was once commonly used as a solvent for dry cleaning and in fire extinguishers before more environmentally friendly compounds were developed. What is the chemical formula for carbon tetrachloride?

A. CClB. CTeCl

C. C4ClD. CCl4

50. The name iron (II) indicates that a compound contains

a. iron ions with an 11+ chargeb. iron ions with a 2+ charge

c. iron ions with a negative charged. two types of iron ions

51. What is the formula for the hydronitric acid?A. HNO3

B. HNO2

C. H3ND. HN3

52. What is the name of the compound with the chemical formula CrCl3?

A. chromium tetrachloride B. chromium trichloride

C. chromium (II) chloride D. chromium (III) chloride

53. N2S3 is properly named:A. Nitrogen sulfideB. Nitrogen (III) sulfide

C. Nitrogen (II) sulfideD. None of these

Name________________________________Date_______________________ Period_______________

54. What is the correct formula for Calcium Carbonate?A. Ca2(CO3)2

B. CaCO3

C. Ca2CO3

D. Ca2CO5

55. What is the formula for carbonic acid?A. CO3

2-

B. H4CC. H2CO3

D. HCO3

Unit 9- Chemical Quantities ~11 %a. Use dimensional analysis to convert mass, particles, or liters to and from molesb. Calculate the percent composition of given compounds from formulas and from mass datac. Determine the empirical formula for a compound from percent composition datad. Determine the molecular formula for a compound from percent composition data and molar mass

56. What is the empirical formula for a compound that contains 17.34% hydrogen and 82.66% carbon?a. C5Hb. C2H5

c. CH3

d. CH2

57. A student found that the empirical formula of an unknown compound is CH2O and that its molar mass is 210 grams per mole. What is the molecular formula of the compound?

A. C5H10O5

B. C6H12O6

C. C7H14O7

D. C8H16O8

58. A compound is 40.0% carbon, 53.3% oxygen, and 6.66% hydrogen. What is its empirical formula?A. C4H5H7

B. CO2H3

C. COH2

D. None of these is the correct empirical formula

59. The percent composition of the compound CH2 isA. 14% hydrogen and 86% carbonB. 86% hydrogen and 14% carbonC. 17% hydrogen and 83% carbonD. 83% hydrogen and 17% carbon

60. What is the total number of atoms contained in 2.00 moles of nickel?A. 58.9B. 118

C. 6.02 x 1023

D. 1.2 x 1024

61. What is the mass in grams of 2.50 moles K2CO3?A. 345 gB. 265 g

C. 247.5 gD. 167.5 g

62. What is the molar mass of (NH4)3PO4?A. 113 gB. 121 g

C. 149 gD. 404 g

Name________________________________Date_______________________ Period_______________