barron's regents exam prep · according to one acid-base theory, water can act as a base...

4/22/2016 Barron's Regents Exam Prep

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Name_________________________________

MAY 2, 2016

REVIEW: CHEMISTRY I & 2

Ms. Narvaez

1. According to one acid-base theory, water can act as a base because a water molecule can

1. donate an H+ ion 3. donate an H- ion

2. accept an H+ ion 4. accept an H- ion

2. Which ion in the ground state has the same electron configuration as an atom of argon in the ground state?

1. A13+ 3. K+

2. O2-4. F-

3. An aqueous solution has a mass of 490 grams containing 8.5 × 10-3 gram of calcium ions. The concentration of calcium ions in this solution is1. 4.3 ppm 3. 17 ppm2. 8.5 ppm 4. 34 ppm

4. Compared to distilled water, an aqueous salt solution has1. better electrical conductivity 3. a lower boiling point at standard pressure2. poorer electrical conductivity 4. a higher freezing point at standard pressure

5. What is the volume of 0.30 M NaOH(aq) needed to completely neutralize 15.0 milliliters of 0.80 M HCl(aq)?1. 3.6 mL 3. 20. mL2. 5.6 mL 4. 40. mL

6. An open flask is half filled with water at 25oC. Phase equilibrium can be reached after1. more water is added to the flask 3. the temperature is decreased to 15oC2. the flask is stoppered 4. the temperature is increased to 35oC

7. A compound is broken down by chemical means during1. chromatography 3. electrolysis2. distillation 4. filtration

8. Which list includes three types of chemical formulas for organic compounds?1. covalent, metallic, isotopic 3. empirical, structural, isotopic2. covalent, metallic, molecular 4. empirical, structural, molecular

9. What is the chemical formula of iron(III) sulfide?1. FeS 3. FeSO3

2. Fe2S3 4. Fe2(SO3)3

10. Given the balanced equation representing a reaction:4Al(s) + 3O2(g) → 2Al2O3(s)How many moles of Al(s) react completely with 4.50 moles of O2(g) to produce 3.00 moles of Al2O3(s)?



1. 1.50 mol 3. 6.00 mol2. 2.00 mol 4. 4.00 mol

11. What is the percent composition by mass of hydrogen in NH4HCO3 (gram-formula mass = 79 grams/mole)?

1. 5.1% 3. 10.%2. 6.3% 4. 50.%

12. Which formula represents strontium phosphate?1. SrPO4 3. Sr2(PO4)32. Sr3PO8 4. Sr3(PO4)2

13. The chemical formula for nickel (II) bromide is1. Ni2Br 3. N2Br

2. NiBr2 4. NBr2

14. Given the reaction: . . . (see image)How many moles of C6H12O6(s) are needed to produce 24 moles of carbon dioxide?

1. 1.0 mole 3. 24 moles2. 12 moles 4. 4.0 moles

15. The percent by mass of hydrogen in NH3 is equal to

16. What is the empirical formula for the compound C6H12O6?

1. CH2O 3. C3H6O3

2. C2H4O2 4. C6H12O6

17. Given the balanced equation representing a reaction:

F2(g) + H2(g) --> 2HF(g)

What is the mole ratio of H2(g) to HF(g) in this reaction?

1. 1:1 3. 2:12. 1:2 4. 2:3

18. Which formula represents lead(II) chromate?1. PbCrO4 3. Pb2CrO4

2. Pb(CrO4)2 4. Pb2(CrO4)3



19. Which substance can be decomposed by chemical means?1. aluminum 3. silicon2. octane 4. xenon

20. Expressed to the correct number of significant figures, the sum of two masses is 445.2 grams. Which two masses produce this answer?1. 210.10 g + 235.100 g 3. 210.1 g + 235.1 g2. 210.100 g + 235.10 g 4. 210.10 g + 235.10 g

21. A student measures the mass and volume of a piece of aluminum. The measurements are 25.6 grams and 9.1 cubic centimeters. The student calculates thedensity of the aluminum. What is the percent error of the student's calculated density of aluminum?

1. 1% 3. 3%2. 2% 4. 4%

22. The accepted value for the percent by mass of water in a hydrate is 36.0%. In a laboratory activity, a student determined the percent by mass of water in thehydrate to be 37.8%. What is the percent error for the student's measured value?

1. 5.0% 3. 1.8%2. 4.8% 4. 0.05%

23. Which kelvin temperature is equal to 56oC?1. –329 K 3. 217 K2. –217 K 4. 329 K

24. Which quantity of heat is equal to 200. joules?

1. 20.0 kJ 3. 0.200 kJ2. 2.00 kJ 4. 0.0200 kJ

25. Which of these elements has physical and chemical properties most similar to silicon (Si)?1. germanium (Ge) 3. phosphorus (P)2. lead (Pb) (4) 4. chlorine (Cl)

26. The elements in the Periodic Table are arranged in order of increasing1. atomic number 3. mass number2. atomic radius 4. neutron number

27. An atom of which element has the largest atomic radius?1. Fe 3. Si2. Mg 4. Zn

28. An atom of helium-4 differs from an atom of lithium-7 in that the atom of helium-4 has1. one more proton 3. two less protons2. one more neutron 4. two less neutrons



29. Which elements have the most similar chemical properties?

1. Si, As, and Te 3. Mg, Sr, and Ba

2. N2, O2, and F2 4. Ca, Cs, and Cu

30. Which of the following Group 15 elements has the greatest metallic character?

1. nitrogen 3. antimony

2. phosphorus 4. bismuth

31. Which statement correctly describes two forms of oxygen, O2 and O3?

1. They have identical molecular structures and identical properties. 3. They have different molecular structures and identical properties.

2. They have identical molecular structures and different properties. 4. They have different molecular structures and different properties.

32. A metal, M, forms an oxide compound with the general formula M2O. In which group on the Periodic Table could metal M be found?

1. Group 1 3. Group 16

2. Group 2 4. Group 17

33. What is the mass number of a carbon atom that contains six protons, eight neutrons, and six electrons?

1. 6 3. 14

2. 8 4. 20

34. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has

1. more protons than neutrons 3. a total of two valence electrons

2. more neutrons than protons 4. a total of eight valence electrons

35. Which atom in the ground state requires the least amount of energy to remove its valence electron?

1. lithium atom 3. rubidium atom

2. potassium atom 4. sodium atom

36. Which element is a liquid at 305 K and 1.0 atmosphere?

1. magnesium 3. gallium

2. fluorine 4. iodine

37. The isotopes K-37 and K-42 have the same

1. decay mode 3. mass number for their atoms

2. bright-line spectrum 4. total number of neutrons in their atoms

38. The atomic mass of titanium is 47.88 atomic mass units. This atomic mass represents the

1. total mass of all the protons and neutrons in an atom of Ti 3. weighted average mass of the most abundant isotope of Ti

2. total mass of all the protons, neutrons, and electrons in an atom of Ti 4. weighted average mass of all the naturally occurring isotopes of Ti



39. The atoms in a sample of an element are in excited states. A bright-line spectrum is produced when these atoms1. absorb energy 3. emit energy2. absorb positrons 4. emit positrons

40. Compared to an atom of hydrogen in the ground state, an atom of hydrogen in the excited state has1. absorbed energy, only 3. neither released nor absorbed energy2. released energy, only 4. both released and absorbed energy

41. Which quantity can vary among atoms of the same element?1. mass number 3. number of protons2. atomic number 4. number of electrons

42. The atomic masses and the natural abundances of the two naturally occurring isotopes of lithium are shown on the accompanying table.

Which numerical setup can be used to determine the atomic mass of lithium?

1. (0.075)(6.02 u) + (0.925)(7.02 u) 3. (7.5)(6.02 u) + (92.5)(7.02 u)2. (0.925)(6.02 u) + (0.075)(7.02 u) 4. (92.5)(6.02 u) + (7.5)(7.02 u)

43. Which notations represent different isotopes of the element sodium?

1. 32S and 34S 3. Na+ and Na0

2. S2- and S6+ 4. 22Na and 23Na

44. In which pair do the particles have approximately the same mass?1. proton and electron 3. neutron and electron2. proton and neutron 4. neutron and beta particle

45. A student constructs a model for comparing the masses of subatomic particles. The student selects a small, metal sphere with a mass of 1 gram to representan electron. A sphere with which mass would be most appropriate to represent a proton?

1. 1 g 3. 1/2000 g2. 1/2 g 4. 2000 g

46. What is the total number of protons in an atom with the electron configuration 2-8-18-32-18-1?1. 69 3. 1182. 79 4. 197

47. Which subatomic particle is negatively charged?1. electron 3. positron



2. neutron 4. proton

48. Which electron configuration represents an atom in an excited state?1. 2-7 3. 2-8-12. 2-6-2 4. 2-8-8-2

49. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at thefoil

1. passed through the foil 3. were deflected by the nuclei in gold atoms2. remained trapped in the foil 4. were deflected by the electrons in gold atoms

50. What must occur when an electron in an atom returns from a higher energy state to a lower energy state?1. A specific amount of energy is released. 3. The atom undergoes transmutation.2. A random amount of energy is released. 4. The atom spontaneously decays.

51. Which electron-dot structure represents a nonpolar molecule?

52. Which formula represents a compound that is formed primarily by sharing electrons?1. KCl 3. CrCl32. CaCl2 4. CCl4

53. As an atom becomes an ion, its mass number1. decreases 3. remains the same2. increases

54. What is the total number of electrons in a Cu+ ion?1. 28 3. 302. 29 4. 36

55. Which statement explains why H2O has a higher boiling point than N2?

1. H2O has greater molar mass than N2. 3. H2O has stronger intermolecular forces than N2.

2. H2O has less molar mass than N2. 4. H2O has weaker intermolecular forces than N2.



56. Which type of molecule is CF4?

1. polar, with a symmetrical distribution of charge 3. nonpolar, with a symmetrical distribution of charge2. polar, with an asymmetrical distribution of charge 4. nonpolar, with an asymmetrical distribution of charge

57. Which element is malleable and can conduct electricity in the solid phase?1. iodine 3. sulfur2. phosphorus 4. tin

58. What is the total number of electrons in a S2- ion?1. 10 3. 162. 14 4. 18

59. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are1. shared to form an ionic bond 3. transferred to form an ionic bond2. shared to form a covalent bond 4. transferred to form a covalent bond

60. Which type of bonding is found in all molecular substances?1. covalent bonding 3. ionic bonding2. hydrogen bonding 4. metallic bonding

61. Based on Table S, an atom of which element has the weakest attraction for electrons in a chemical bond?1. polonium 3. selenium2. sulfur 4. tellurium

62. Which electron-dot symbol correctly represents an atom of its given element?

63. Based on Reference Table I, which change occurs when pellets of solid NaOH are added to water and stirred?1. The water temperature increases as chemical energy is converted toheat energy.

3. The water temperature decreases as chemical energy is converted toheat energy.

2. The water temperature increases as heat energy is stored as chemicalenergy.

4. The water temperature decreases as heat energy is stored aschemical energy.

64. Note: This question may require the use of the Reference Tables for Physical Setting/Chemistry.Which process would most effectively separate two liquids with different molecular polarities?

1. filtration 3. distillation2. fermentation 4. conductivity



65. Note: This question may require the use of the Reference Tables for Physical Setting/Chemistry.What is the total number of joules released when a 5.00-gram sample of water changes from liquid to solid at 0oC?

1. 334 J 3. 2260 J2. 1670 J 4. 11,300 J

66. A sample of a gas is contained in a closed rigid cylinder. According to kinetic molecular theory, what occurs when the gas inside the cylinder is heated?1. The number of gas molecules increases. 3. The average velocity of the gas molecules increases.2. The number of collisions between gas molecules per unit timedecreases.

4. The volume of the gas decreases.

67. At room temperature, the solubility of which solute in water would be most affected by a change in pressure?1. methanol 3. carbon dioxide2. sugar 4. sodium nitrate

68. A sample of gas is held at constant pressure. Increasing the kelvin temperature of this gas sample causes the average kinetic energy of its molecules to1. decrease and the volume of the gas sample to decrease 3. increase and the volume of the gas sample to decrease2. decrease and the volume of the gas sample to increase 4. increase and the volume of the gas sample to increase

69. When 5 grams of KCl are dissolved in 50. grams of water at 25oC, the resulting mixture can be described as1. heterogeneous and unsaturated 3. homogeneous and unsaturated2. heterogeneous and supersaturated 4. homogeneous and supersaturated

70. Which aqueous solution of KI freezes at the lowest temperature?1. 1 mol of KI in 500. g of water 3. 1 mol of KI in 1000. g of water2. 2 mol of KI in 500. g of water 4. 2 mol of KI in 1000. g of water

71. According to kinetic molecular theory, collisions between gas particles in a sample of an ideal gas1. increase the energy content of the gas sample 3. result in a net loss of energy by the gas sample2. produce strong attractive forces between the gas particles 4. transfer energy between the gas particles

72. A dilute, aqueous potassium nitrate solution is best classified as a1. homogeneous compound 3. heterogeneous compound2. homogeneous mixture 4. heterogeneous mixture

73. Two solid samples each contain sulfur, oxygen, and sodium, only. These samples have the same color, melting point, density, and reaction with an aqueousbarium chloride solution. It can be concluded that the two samples are the same

1. compound 3. mixture2. element 4. solution

74. Which sample at STP has the same number of molecules as 5 liters of NO2(g) at STP?

1. 5 grams of H2(g) 3. 5 moles of O2(g)



2. 5 liters of CH4(g) 4. 5 x 1023 molecules of CO2(g)

75. A 1.0-gram sample of which element will uniformly fill a closed 2.0-liter container at STP?1. antimony 3. tellurium2. sulfur 4. xenon

76. Under which conditions of temperature and pressure would a real gas behave most like an ideal gas?1. 200. K and 50.0 kPa 3. 600. K and 50.0 kPa2. 200. K and 200.0 kPa 4. 600. K and 200.0 kPa

77. Which term is defined as a measure of the average kinetic energy of the particles in a sample?1. temperature 3. thermal energy2. pressure 4. chemical energy

78. At standard pressure, which element has a freezing point below standard temperature?1. In 3. Hf2. Ir 4. Hg

79. Which two particle diagrams represent mixtures of diatomic elements?

1. A and B 3. B and C2. A and C 4. B and D

80. Which sample of matter can be separated into different substances by physical means?1. LiCl(aq) 3. NH3(g)

2. LiCl(s) 4. NH3(l)

81. At STP, 1.0 liter of helium contains the same total number of atoms as1. 1.0 L of Ne 3. 0.5 L of Rn2. 2.0 L of Kr 4. 1.5 L of Ar

82. Which compound has the strongest hydrogen bonding between its molecules?1. HBr 3. HF2. HCl 4. HI

83. Which property of an unsaturated solution of sodium chloride in water remains the same when more water is added to the solution?



1. density of the solution 3. mass of sodium chloride in the solution2. boiling point of the solution 4. percent by mass of water in the solution

84. Which ion combines with Ba2+ to form a compound that is most soluble in water?

1. S2- 3. CO32-

2. OH- 4. SO42-

85. Which grouping of the three phases of bromine is listed in order from left to right for increasing distance between bromine molecules?1. gas, liquid, solid 3. solid, gas, liquid2. liquid, solid, gas 4. solid, liquid, gas

86. Which sample of water has the lowest vapor pressure?

1. 100 mL at 50oC 3. 300 mL at 40oC

2. 200 mL at 30oC 4. 400 mL at 20oC

87. A sealed flask containing 1.0 mole of H2(g) and a sealed flask containing 2.0 moles of He(g) are at the same temperature. The two gases must have equal

1. masses 3. average kinetic energies2. volumes 4. numbers of molecules

88. Two basic properties of the gas phase are1. a definite shape and a definite volume 3. no definite shape but a definite volume2. a definite shape but no definite volume 4. no definite shape and no definite volume

89. The temperature at which the solid and liquid phases of matter exist in equilibrium is called its1. melting point 3. heat of fusion2. boiling point 4. heat of vaporization

90. In aqueous solution, a chloride ion is attracted to which end of the water molecule?1. the hydrogen end, which is the positive pole 3. the oxygen end, which is the positive pole2. the hydrogen end, which is the negative pole 4. the oxygen end, which is the negative pole

91. According to Reference Table G, how many grams of KNO3 would be needed to saturate 200 grams of water at 70oC?

1. 43 g 3. 134 g2. 86 g 4. 268 g

92. According to Reference Table G, which of these substances is most soluble at 60oC?1. NaCl 3. KClO3

2. KCl 4. NH4Cl

93. In which material are the particles arranged in a regular geometric pattern?



1. CO2(g) 3. H2O(l)

2. NaCl(aq) 4. C12H22O11(s)

94. Which change is exothermic?1. freezing of water 3. vaporization of ethanol2. melting of iron 4. sublimation of iodine

95. Which type of change must occur to form a compound?1. chemical 3. nuclear2. physical 4. phase

96. Which statement correctly describes an endothermic chemical reaction?

97. The solubility of KClO3(s) in water increases as the

1. temperature of the solution increases 3. pressure on the solution increases2. temperature of the solution decreases 4. pressure on the solution decreases

98. In which process does a solid change directly into a vapor?1. condensation 3. deposition2. sublimation 4. solidification

99. Which molecule contains a nonpolar covalent bond?

100. Given the simple representations for atoms of two elements in the accompanying diagram:

Which particle diagram represents molecules of only one compound in the gaseous phase?



101. Which ion, when combined with chloride ions, Cl-, forms an insoluble substance in water?

1. Fe2+ 3. Pb2+

2. Mg2+ 4. Zn2+

barron's regents exam prep · according to one acid-base theory, water can act as a base...

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