CP Final Review 2013- 2014 Multiple-Choice Questions

MOLES____1. How many grams are there in 2.50 moles of chromium?

a. 41.6 g c. 130.0 gb. 20.8 g d. 60.0 g

_____2.The molar mass of aluminum sulfate is _____.a. 123 g/molb. 214 g/molc. 278 g/mold. 342 g/mol

____3. Which one of the following compounds has the lowest molar mass?a. Carbon monoxide. c. Carbon dioxide.b. Nitrogen dioxide. d. Nitrogen monoxide.

____4. How many oxygen atoms are there in 0.25 mole of oxygen gas?a. 3.011 x 1023 c. 1.556 x 1023

b. 6.022 x 1023 d. 1.204 x 1024

____5. A chemical formula includes the symbols of the elements in the compound and subscripts that indicatea. the number of moles in each element.b. how many atoms or ions of each type are combined in the simplest unit.c. the formula mass.d. the charges on the elements or ions.

____6. How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?a. 1 c. 4b. 2 d. 5

____7. Changing a subscript in a correctly written chemical formulaa. changes the number of moles represented by the formula.b. changes the charges on the other ions in the compound.c. changes the formula so that it no longer represents that compound.d. has no effect on the formula.

____8. How many grams are there in 1.5 moles of chlorine gas?a. 35.5 g b. 71.0 g c. 106.5 g d. 184.6 g

____9. The molar mass of MgI2 is _____.a. the sum of the masses of 1 mol of Mg and 2 mol of I.b. the sum of the masses of 1 mol of Mg and 1 mol of I.c. the sum of the masses of 2 mol of Mg and 2 mol of I.

d. impossible to calculate.

____10.The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?a. 0.4003 mol c. 2.498 molb. 1.000 mol d. 114.95 mol

____11.The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?a. 5 g c. 769.0 gb. 30.76 g d. 796.05 g

____12.The molar mass of H2O is 18.015 g/mol. How many grams of H2O are present in 0.20 mole?a. 0.2 g c. 35.9 gb. 3.6 g d. 89.9 g

____13.The empirical formula is always the accepted formula for a(n)a. atom. c. molecular compound.b. molecule. d. ionic compound.

____ 14. The empirical formula for a compound shows the symbols of the elements with subscripts indicating thea. actual numbers of atoms in a molecule.b. number of moles of the compound in 100 g.c. smallest whole-number ratio of the atoms.d. atomic masses of each element.

____ 15. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?a. CHO c. C3H4O3

b. CH2O d. C2H4O2

____ 16. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?a. C3H6 c. C5H8

b. C4H10 d. C5H15

____ 17. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?a. NO c. NO4

b. N2O2 d. N2O4

____ 18. The number of atoms in 1 mole of carbon is ___.a. 6.022 x 1022. c. 5.022 x 1022.b. 6.022 x 1023. d. 5.022 x 1023.

____ 19. Molar mass ____.a. is the mass in grams of one mole of a substance.b. is numerically equal to the average atomic mass of the element.c. both a and bd. neither a nor b

____ 20. A mass of 6.005 g of carbon (atomic mass 12.010 amu) containsa. 1 mol C. c. 0.5000 mol C.b. 2 atoms C. d. 1 atom O.

____ 21. What is the number of moles of chemical units represented by 9.03 x 1024 units?a. 1.50 mol c. 10.0 molb. 9.03 mol d. 15.0 mol

____ 22. A prospector finds 39.39 g of gold (atomic mass 196.9665 amu). She hasa. 1.20 x1023 atoms. c. 4.30 x 1023 atoms.b. 2.30 x 1023 atoms. d. 6.02 x 1023 atoms.

____ 23. A sample of tin (atomic mass 118.69 amu) contains 3.01 x 1023 atoms. The mass of the sample is ___.a. 3.01 g. c. 72.6 g.b. 59.3 g. d. 11 g.

____ 24. What is the percentage composition of CF4?a. 20% C, 80% F c. 16.8% C, 83.2% Fb. 13.6% C, 86.4% F d. 81% C, 19% F

____ 25. What is the percentage composition of CuCl2?a. 33% Cu, 66% Cl c. 65.50% Cu, 34.50% Clb. 50% Cu, 50% Cl d. 47.263% Cu, 52.737% Cld. always equal to the total mass of the products.

EQUATIONS____ 26. The law of conservation of mass follows from the concept that

a. atoms are indivisible in chemical reactions.b. atoms of different elements have different properties.c. matter is composed of atoms.d. atoms can be destroyed in chemical reactions.

____ 27. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is ____ the sum of the masses of the individual elements.a. equal to c. less thanb. greater than d. either greater than or less than

____ 28. Knowledge about what products are produced in a chemical reaction is obtained bya. inspecting the chemical equation. c. laboratory analysis.b. balancing the chemical equation. d. writing a word equation.

____ 29. A chemical reaction has NOT occurred if the products havea. the same mass as the reactants.b. less total bond energy than the reactants.c. more total bond energy than the reactants.d. the same chemical properties as the reactants.

____ 30. Which observation does NOT indicate that a chemical reaction has occurred?a. formation of a precipitate c. evolution of heat and lightb. production of a gas d. change in total mass of substances

____ 31. A solid produced by a chemical reaction in solution that separates from the solution is calleda. a precipitate. c. a molecule.b. a reactant. d. the mass of the product.

____ 32. After the correct formula for a reactant in an equation has been written, thea. subscripts are adjusted to balance the equation.b. formula should not be changed.c. same formula must appear as the product.d. symbols in the formula must not appear on the product side of the equation.

____ 33. In writing an equation that produces hydrogen gas, the correct representation of hydrogen gas isa. H. c. H2.b. 2H. d. OH.

____ 34. To balance a chemical equation, it may be necessary to adjust thea. coefficients. c. formulas of the products.b. subscripts. d. number of products.

____ 35. According to the law of conservation of mass, the total mass of the reacting substances isa. always more than the total mass of the products.b. always less than the total mass of the products.c. sometimes more and sometimes less than the total mass of the products.d. always equal to the total mass of the products.

____ 36. A chemical equation is balanced when thea. coefficients of the reactants equal the coefficients of the products.b. same number of each kind of atom appears in the reactants and in the products.c. products and reactants are the same chemicals.d. subscripts of the reactants equal the subscripts of the products.

____ 37.Which word equation represents the reaction that produces water from hydrogen and oxygen?a. Water is produced from hydrogen and oxygen.b. Hydrogen plus oxygen yields water.c. H2 + O2 →water.d. Water can be separated into hydrogen and oxygen.

____38. For the formula equation 2Mg + O2 → 2MgO, the word equation would begina. Manganese plus oxygen . . . c. Magnesium plus oxygen . . .b. Molybdenum plus oxygen . . . d. Heat plus oxygen . . .

____39 . In an equation, the symbol for a substance in water solution is followed by

a. (1). c. (aq).b. (g). d. (s).

____ 40. The reaction 2Mg(s) + O2(g) → 2MgO(s) is aa. synthesis reaction. c. single-replacement reaction.b. decomposition reaction. d. double-replacement reaction.

____ 41. The reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is aa. composition reaction. c. single-replacement reaction.b. decomposition reaction. d. double-replacement reaction.

____ 42. In the equation 2Al(s) + 3Fe(NO3)2(aq) → 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced bya. nitrate. c. aluminum.b. water. d. nitrogen.

____ 43. An insoluble gas that forms in a double-replacement reaction in aqueous solutiona. bubbles out of solution. c. disassociates into ions.b. forms a precipitate. d. reacts with the water.

____ 44. The formulas for the products of the reaction between sodium chloride and fluorine gas are ____.a. nothing, no reaction c. NaF + Clb. FCl + Na d. NaF + Cl2

____ 45. An element in the activity series can replace any element _____.a. in the periodic table. c. above it on the list.b. below it on the list. d. in its group.

____ 46. What can be predicted by using an activity series?a. whether a certain chemical reaction will occurb. the amount of energy released by a chemical reactionc. the electronegativity values of elementsd. the melting points of elements

____ 47. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is ____ the sum of the masses of the individual elements.a. equal to c. less thanb. greater than d. either greater than or less than

____ 48. A chemical equation is balanced when the ____.a. coefficients of the reactants equal the coefficients of the products.b. same number of each kind of atom appears in the reactants and in the products.c. products and reactants are the same chemicals.d. subscripts of the reactants equal the subscripts of the products.

____ 49. Which word equation represents the reaction that produces water from hydrogen and oxygen?a. Water is produced from hydrogen and oxygen.

b. Hydrogen plus oxygen yields water.c. H2 + O2 → water.d. Water can be separated into hydrogen and oxygen.

____50. For the formula equation 2Mg + O2 → 2MgO, the word equation would begina. Manganese plus oxygen . . . c. Magnesium plus oxygen . . .b. Molybdenum plus oxygen . . . d. Heat plus oxygen . . .

____ 51 . In an equation, the symbol for a substance in water solution is followed bya. (1). c. (aq).b. (g). d. (s).

____ 52 . When the equation Fe3O4 + Al → Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?a. 3 c. 6b. 4 d. 9

____53.Which coefficients correctly balance the formula equation NH4NO2(s) → N2(g) + H2O(l)?a. 1, 2, 2 c. 2, 1, 1b. 1, 1, 2 d. 2, 2, 2

____54.Which coefficients correctly balance the formula equation CaO + H2O → Ca(OH)2?a. 2, 1, 2 c. 1, 2, 1b. 1, 2, 3 d. 1, 1, 1

____ 55. The complete balanced equation for the reaction between zinc hydroxide and acetic acid is ___.a. ZnOH + CH3COOH → ZnCH3COO + H2O.b. Zn(OH)2 + CH3COOH → Zn + 2CO2 +3H2O.c. Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + 2H2O.d. Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + H2 + O2.

____ 56. What is the balanced equation for the combustion of sulfur?a. S(s) + O2(g) → SO(g) c. 2S(s) + 3O2(g) → SO3(s)b. S(s) + O2(g) → SO2(g) d. S(s) + 2O2(g) → SO4

2–(aq)

____57 .Which equation is NOT balanced?a. 2H2 + O2 → 2H2Ob. 4H2 + 2O2 → 4H2Oc. H2 + H2 + O2 → H2O + H2Od. 2H2 + O2 → H2O

____ 58. The equation AX → A + X is the general equation for a ____.a. synthesis reaction. c. combustion reaction.b. decomposition reaction. d. single-replacement reaction.

____ 59. The equation AX + BY → AY + BX is the general equation for a _____.a. synthesis reaction. c. single-replacement reaction.

b. decomposition reaction. d. double-replacement reaction.

____ 60. The equation A + X → AX is the general equation for a(n) ____.a. combustion reaction. c. synthesis reaction.b. ionic reaction. d. double-replacement reaction.

____ 61. In what kind of reaction does a single compound produce two or more simpler substances?a. decomposition reaction c. single-replacement reactionb. synthesis reaction d. ionic reaction

____ 62. The equation A + BX → AX + B is the general equation for aa. double-replacement reaction. c. single-replacement reaction.b. decomposition reaction. d. combustion reaction.

____ 63. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new compounds?a. synthesis reaction c. decomposition reactionb. double-replacement reaction d. combustion reaction

____ 64. The reaction 2Mg(s) + O2(g) → 2MgO(s) is aa. synthesis reaction. c. single-replacement reaction.b. decomposition reaction. d. double-replacement reaction.

____ 65. The reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is aa. composition reaction. c. single-replacement reaction.b. decomposition reaction. d. double-replacement reaction.

____ 66. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are ____.a. Na2SO4 and H2O. c. SI4 and Na2O.b. NaSO4 and H2O. d. S + O2 and Na.

BONDING AND MOLECULAR GEOMETRY ____ 67. A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the

atoms together is called a(n)a. dipole. c. chemical bond.b. Lewis structure. d. London force.

____68. Atoms are ____ when they are combined.a. more stable c. not bound togetherb. less stable d. at a high potential energy

____69.A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)a. covalent bond. c. charged bond.b. ionic bond. d. dipole bond.

____ 70.The chemical bond formed when two atoms share electrons is called a(n)a. ionic bond. c. Lewis structure.

b. orbital bond. d. covalent bond.____71. If two covalently bonded atoms are identical, the bond is ____.

a. nonpolar covalent. c. nonionic.b. polar covalent. d. coordinate covalent.

____72. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called ___.a. nonpolar. c. ionic.b. polar. d. dipolar.

____73.The B—F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is ____.a. polar covalent. c. nonpolar covalent.b. ionic. d. pure covalent.

____74. In which of these compounds is the bond between the atoms NOT a nonpolar covalent bond?a. Cl2 c. HClb. H2 d. O2

____ 75. A molecule is a ____.a. negatively charged group of atoms held together by covalent bonds.b. positively charged group of atoms held together by covalent bonds.c. neutral group of atoms held together by covalent bonds.d. neutral group of atoms held together by ionic bonds.

____ 76. What principle states that atoms tend to form compounds so that each atom can have eight electrons in its outermost energy level?a. rule of eights c. configuration ruleb. Avogadro principle d. octet rule

____ 77. Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or ____.a. chlorine. c. oxygen.b. hydrogen. d. helium.

____ 78. A shorthand representation of the composition of a substance using atomic symbols and numerical subscripts is called a(n) ___.a. Lewis structure. c. polyatomic ion.b. chemical formula. d. multiple bond.

____ 79. The ions in an ionic compound are organized into a(n) ____.a. molecule. c. polyatomic ion.b. Lewis structure. d. crystal.

____ 80. In a crystal of an ionic compound, each cation is surrounded by _____.a. molecules. c. dipoles.b. positive ions. d. anions.

____ 81. To form a molecule with a “bent” shape, the ratio of shared to unshared pairs of electrons is __.a. 1:2 c. 2:2

b. 2:1 d. 3:1

____ 82. Which molecule has a pyramidal shape?a. CBr4 c. BF3

b. CO2 d. NH3

____ 83. Identify the molecule that will have a linear shape.a. CCl4

b. H2Oc. NH3

d. CO2

____84. Which formula represents a tetrahedral molecule?a. SiBr4 c. HBrb. CaCl2 d. AlF3

____ 85 The correct electron dot notation for a molecule of iodine is

____86. VSEPR theory is a model for predicting _____.a. the strength of metallic bonds. c. lattice energy values.b. the shape of molecules. d. ionization energy.

____ 87. Which bond has the greatest degree of ionic bonding? a) Li-Br b) F-F c) H-Cl d) S-O

____ 88. If two atoms exert equal attractions for electrons, they form ____. a) a non-polar covalent bond; b) an ionic bond; c) a polar covalent bond; d) no bond

____ 89. Which of the following is not a polar molecule? a) hydrogen fluoride b) hydrogen c) water d) ammonia (NH3)

____ 90. Which of the following kinds of bonds exists in a N2 molecule? a) ionic b) polar c) single d) double e) triple

____ 91. A polar molecule is one in which there is a separation of charge caused by a) an average distribution of electrons; b) a non-uniform electron distribution; c) a complete loss of electrons; d) an uneven number of electron pairs.

____ 92. Which is an example of a non-polar molecule that contains polar covalent bonds? a) CBr4 b) N2 c) H2O d) NH3 e) none of these

_____93. Which one is an example of a diatomic molecule? a) magnesium ion b) nitrogen gas c) helium gas d) sodium chloride

_____94. Why is NH3 classified as a polar molecule? a) It is a gas at STP. b) N-H bonds are non-polar. c) Nitrogen and hydrogen are both nonmetals. d) NH3 molecules have asymmetrical charge distributions.

_____95. The substance whose electron dot formula indicates four covalent bonds is a) AlF3; b) N2; c) H2O; d) CH2F2.

_____96. The molecular shape predicted by the VSEPR theory when two shared pairs of electrons and no un-shared pair of electrons surround the central atom is a) tetrahedral; b) pyramidal; c) bent; d) linear.

_____97. Which pair of elements will not form an ionic bond? a) Ba and Cl b) Ca and S c) K and O d) C and Cl

_____98.What is the true electron dot notation for ammonia, NH3?

IONIC AND COVALENT (MOLECULAR) COMPOUNDS

_____99. What is the formula unit for ammonium phosphate? a) NH4PO4 b) (NH4)3PO4 c) (NH4)3(PO4)2 d) (NH4)3PO3

_____100. What is the total number of atoms are there in 3 units of lithium carbonate?a. 15 b.12 c. 18 d.21

_____101. How many oxygen atoms are there in 5 units of dinitrogen pendoxide? a) 35 b) 25 c) 10 d) 5 e) None of these.

_____102. What is the proper name for N2O? a) nitrogen oxygen b) nitrogen oxide c) dinitrogen oxide d) dinitrogen monoxide

_____103. What is the proper name for Ba(OH)2? a) barium hydroxide b) barium hydrogen oxygen c) barium dihydroxide d) None of these.

_____104. How many moles of oxygen atoms are there in 1 mole of calcium phosphite? a) 3 b) 4 c) 6 d) 8 e) none of these

_____105. How many significant figures are there in the measurement of 321000 s? a) 6 b) 5 c) 3 d) 2 e) 1

_____106. How many mg are there in 2.34 x 10-2Mg? (M: 106; m: 10-3)

a) 2.34 x 10-2 b) 2.34 x 103 c) 2.34 x 105 d) 2.34 x 107 e) None of these.

_____107. For the view below of a graduated cylinder filled with liquid, what is the correct reading on the volume of liq-uid?

a) 46.7mL b) 42.9mL c) 45.3mL d) 43.6mL

_____108. How many pounds are there in 345.3 grams? (1pound = 16oz; 1oz = 28.35g) a) 12.18 b) 0.7612 c) 156600 d) 21.58 e) None of these.

_____109. Round the following measurement to 3 significant figures and then turn it into scientific notation. 92356700 m. The correct answer is ___________. a) 92.4 x 106 b) 0.924 x 108 c) 9.24 x 107 d) 9.24 x 106 e) none of these

STOICHIOMETRY_____110. For the chemical reaction: 4NH3(g) + 5O2(g) --> 6H2O(g) + 4NO(g). How many moles of oxygen gas

will be needed when 12 moles of NH3 is completely reacted? a) 5 b) 10 c) 15 d) 20 e) None of these.

_____111. When 8 grams of hydrogen are chemically combined with oxygen to form water, the amount of oxy-gen needed is ____. [2H2(g) + O2(g) --> 2H2O(g)] a) 1g b) 16g c) 32g d) 64g e) 128g

_____112. Given the reaction CH4 + 2O2 --> CO2 + 2H2O, what amount of oxygen is needed to completely react with 1 mole of CH4? a) 2 moles b) 2 atoms c) 2 grams d) 2 molecules e) None of these.

_____113. A balanced chemical equation allows one to determine the _____. a) mole ratio of any two substances in the reaction b) energy released in the reaction c) electron configuration of all elements in the reaction d) mechanism involved in the reaction

_____114. In the reaction 2Al2O3 --> 4Al + 3O2, what is the mole ratio of aluminum to oxygen? a) 10:6 b) 3:4 c) 2:3 d) 4:3

_____115. What is the small whole number that appears in front of a formula in a chemical equation? a) a subscript b) a superscript c) a ratio d) a coefficient e) none of these.

116. For the reaction 2Na + 2H2O --> 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol. of water?

a) 40. g b) 80. g c) 120 g d) 240 g

117. Calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is produced in the fol-lowing reaction: 2Al(s) + 3FeO(s) --> 3Fe(s) + Al2O3(s) a) 0.20 mol. b) 0.40 mol. c) 0.60 mol. d) 0.90 mol.

118. Hydrogen gas reacts with oxygen gas to produce water vapor. Balanced chemical equation is: 2H2(g) + O2(g) 2H2O(g). How many moles of hydrogen gas will be consumed for the production of 3.64 moles of water?a) 7.28 mol. b) 3.64 mol. c) 1.82 mol. d) 0.91 mol.

119. For the incomplete combustion of ethane (C2H6), what is the mole ratio between ethane and oxygen gas? [Hint: write skeleton equation of the incomplete combustion reaction, balance it, carry out proper calculations.]

a) 1:2 b) 2:1 c) 5:2 d) 2:5 e) 1:3

INTERMOLECULAR FORCES AND KINETIC MOLECULAR THEORY

120. Which of the following forces that hold matter together is the 2nd weakest?a. London dispersion forces.b. Ionic bonds.

c. Hydrogen bond.d. Dipole-dipole interactions.

121. Which of the following molecule is most likely to be soluble in a nonpolar solvent? Hint: Like dis-solves like.

a. H2S b. SO3 c. SO2 d. HCN

122. London dispersion forces exist ___.a. for all moleculesb. only for molecules with polar bonds

c. only for molecules with nonpolar bonds

d. only for molecules with hydrogen bonding

123. Bromine molecule (Br2) is ______.a. Ionic.b. Metallic.

c. Polar. d. Nonpo-lar.

124. Which of the following substances is likely to have low melting temperature? Hint: phase transition temperature depends on strength of interactions between particles of the substance.

a. Barium sulfate.b. Copper metal.

c. Water.d. Carbon tetrachloride.

125. At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is a solid. This is because ____. Hint: phase transition temperature depends on strength of interactions between particles of the sub-stance.

a. dispersion interactions increase in strength as molecular mass increasesb. polarity increases with molecular sizec. dispersion interactions decrease with molecular sized. dipole-dipole interactions increase with molecular size

126. Which of the following interaction(s) is (are) present in H2O? I. London dispersion forces.

II. Dipole-dipole interactions.III. Hydrogen bonding.IV. Ionic bond.

a. I and II b. II and III c. IV only d. I, II and III

127. Which of the following statement regarding Kinetic Molecular Theory is INCORRECT?a. Particles are constantly moving.b. In liquids, particles are far apart.c. In solids, particles can only vibrate around each other.d. As temperature increases, particles start to move faster.

128. Why are gases easier to compress than a liquid or a solid?a. The space between gas particles is much less than the space between liquid or solid particles.b. Gas molecules are far apart, much larger distances between particles in a gas as compared to

those in a liquid or a solid.c. Gas molecules move very fast in all directions.d. None of these.

129. Which state(s) of matter flows?a. Solid. b. Liquid. c. Gas. d. Liquid and gas.

130. Which of the following compound has the 2nd highest melting temperature? Hint: phase transition temperature depends on strength of interactions between particles of the substance.

a. F2 b. Cl2 c. Br2 d. I2

131. Which of the following compound has only London dispersion forces between molecules?a. CCl4 b. HBr c. NH3 d. SO2

132. Consider the following molecules: NH3, BF3, BeCl2, which one(s) has (have) unusually high boiling temperature? Hint: phase transition temperature depends on strength of interactions between particles of the substance.

a. NH3

b. NH3 and BeCl2

c. NH3 and BF3

d. BF3 and BeCl2

133. Which of the following phase transition will produce the largest decrease in volume of the substance?a. Melting.b. Freezing.

c. Boiling.d. Condensation.

134. Which of the following solvent would be most suitable for dissolving iodine? Hint: Like dissolves like.

a. CCl4 b. H2O c. CH3OH d. NH3

135. Which one of the following molecules will be soluble in polar solvent? Hint: Like dissolves like.a. NO2 b. CS2 c. SF6 d. BF3

136. As the liquid turns into vapor, ___.a. kinetic energy of particles decreasesb. average distance between molecules increasesc. density of the matter increasesd. temperature increases

137. Which of the following statements best describes what happens to water molecules when they freeze?a. They gain energy and escape into the atmosphere.b. They lose energy, slow down and eventually cannot move past each other.c. They lose energy, speed up and gain more freedom of movement.d. They gain energy and get closer to each other.

138. Heat must be removed from the system during which of the following phase transitions?I. Freezing.

II. Sublimation.III. Condensation.

a. II only.b. I and II.

c. II and III.

d. I and III.

139. Which of the following molecules has the highest melting and boiling temperatures?a. SO2 b. SiH4 c. CF4 d. BeCl2

140. According to the Kinetic Molecular Theory, what happens to water molecules as temperature goes up?

a. Water molecules move faster and have higher kinetic energy.b. Water molecules move slower and have lower kinetic energy.c. Water molecules move faster and have lower kinetic energy.d. Water molecules move slower and have higher kinetic energy.

141. Which of the following state(s) of matter has (have) the largest distance between particles?a. Liquid.b. Solid.

c. Gas.d. Liquid and gas

142. Which of the following is NOT part of the classic states of matter?a. Solid.b. Liquid crystal.

c. Gas.d. Liquid.

Answers:1 C 44 D 87 A 130 C2 D 45 B 88 A 131 A3 A 46 A 89 B 132 A4 A 47 A 90 E 133 D5 B 48 B 91 B 134 A6 C 49 B 92 A 135 A7 C 50 C 93 B 136 B8 C 51 C 94 D 137 B9 A 52 D 95 D 138 D10 C 53 B 96 D 139 A11 C 54 D 97 D 140 A12 B 55 C 98 2 141 C13 C 56 B 99 B 142 B14 C 57 D 100 C15 C 58 B 101 B16 B 59 D 102 D17 D 60 C 103 A18 B 61 A 104 C19 C 62 C 105 C20 C 63 B 106 D21 D 64 A 107 B22 A 65 C 108 B23 B 66 A 109 C24 B 67 C 110 C25 D 68 A 111 D26 A 69 B 112 A27 A 70 D 113 A28 C 71 A 114 D29 D 72 B 115 D30 D 73 B 116 C31 A 74 C 117 A32 B 75 C 118 B33 C 76 D 119 D34 A 77 C 120 D35 D 78 B 121 B36 B 79 D 122 A37 B 80 D 123 D38 C 81 C 124 D39 C 82 D 125 A40 A 83 D 126 D41 C 84 A 127 B42 C 85 3 128 B43 A 86 B 129 D