CHEM Chapter 2 - Multiple Choice

10) In the Rutherford nuclear-atom model, ________. A) the heavy subatomic particles, protons and neutrons, reside in the nucleus B) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass C) the light subatomic particles, protons and neutrons, reside in the nucleus D) mass is spread essentially uniformly throughout the atom E) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and mass is spread essentially uniformly throughout the atom

A

100) Which metal does not form cations of differing charges? A) Na B) Cu C) Co D) Fe E) Sn

A

2) Which one of the following is not one of the postulates of Dalton's atomic theory? A) Atoms are composed of protons, neutrons, and electrons. B) All atoms of a given element are identical; the atoms of different elements are different and have different properties. C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions. D) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. E) Each element is composed of extremely small particles called atoms.

A

24) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, Cu A) 29 p+, 34 n°, 29 e- B) 29 p+, 29 n°, 63 e- C) 63 p+, 29 n°, 63 e- D) 34 p+, 29 n°, 34 e- E) 34 p+, 34 n°, 29 e-

A

27) Which isotope has 36 electrons in an atom? A) Kr B) Br C) Se D) Cl E) Hg

A

31) Different isotopes of a particular element contain the same number of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) subatomic particles

A

42) Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 41.54 B) 39.68 C) 39.07 D) 38.64 E) 33.33

A

47) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 17.20 B) 16.90 C) 17.65 D) 17.11 E) 16.90

A

48) Vanadium has two naturally occurring isotopes, 50V with an atomic mass of 49.9472 amu and 51V with an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. The percent abundances of the vanadium isotopes are ________% 50V and ________% 51V. A) 0.25, 99.75 B) 99.75, 0.25 C) 49, 51 D) 1.0, 99 E) 99, 1.0

A

49) An unknown element is found to have three naturally occurring isotopes with atomic masses of 35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown element? A) Ar B) K C) Cl D) Ca E) None of the above could be the unknown element.

A

53) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) O, S B) C, N C) K, Ca D) H, He E) Si, P

A

62) Of the choices below, which one is not an ionic compound? A) PCl5 B) MoCl6 C) RbCl D) PbCl2 E) NaCl

A

64) A molecular formula always indicates ________. A) how many of each atom are in a molecule B) the simplest whole-number ratio of different atoms in a compound C) which atoms are attached to which in a molecule D) the isotope of each element in a compound E) the geometry of a molecule

A

72) The species ________ contains 16 neutrons. A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O

A

77) Which species has 48 electrons? A) Sn+2 B) Sn+4 C) Cd+2 D) Ga E) Ti

A

79) Which pair of elements is most apt to form an ionic compound with each other? A) barium, bromine B) calcium, sodium C) oxygen, fluorine D) sulfur, fluorine E) nitrogen, hydrogen

A

84) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is ________. A) Ag B) Pd C) Cd D) Cu E) Cs

A

88) The suffix -ide is used primarily ________. A) for monatomic anion names B) for polyatomic cation names C) for the name of the first element in a molecular compound D) to indicate binary acids E) for monoatomic cations

A

89) Which one of the following compounds is chromium(III) oxide? A) Cr2O3 B) CrO3 C) Cr3O2 D) Cr3O E) Cr2O4

A

90) Which one of the following compounds is copper(I) chloride? A) CuCl B) CuCl2 C) Cu2Cl D) Cu2Cl3 E) Cu3Cl2

A

94) The correct name for HNO2 is ________. A) nitrous acid B) nitric acid C) hydrogen nitrate D) hyponitrous acid E) pernitric acid

A

98) Which element forms an ion with the same charge as the ammonium ion? A) potassium B) chlorine C) calcium D) oxygen E) nitrogen

A

1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of ________. A) the law of multiple proportions B) the law of constant composition C) the law of conservation of mass D) the law of conservation of energy E) none of the above

B

13) In the absence of magnetic or electric fields, cathode rays ________. A) do not exist B) travel in straight lines C) cannot be detected D) become positively charged E) bend toward a light source

B

14) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged? A) β-rays B) α-rays and β-rays C) α-rays, β-rays, and γ-rays D) α-rays E) α-rays and γ-rays

B

19) All atoms of a given element have the same ________. A) mass B) number of protons C) number of neutrons D) number of electrons and neutrons E) density

B

20) Which atom has the smallest number of neutrons? A) carbon-14 B) nitrogen-14 C) oxygen-16 D) fluorine-19 E) neon-20

B

25) Which isotope has 45 neutrons? A) Kr B) Br C) Se D) Cl E) Rh

B

26) Which pair of atoms constitutes a pair of isotopes of the same element? A) X X B) X X C) X X D) X X E) X X

B

32) Different isotopes of a particular element contain different numbers of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) None of the above is correct.

B

34) In the symbol below, X = ________. X A) N B) C C) Al D) K E) not enough information to determine

B

38) Gravitational forces act between objects in proportion to their ________. A) volumes B) masses C) charges D) polarizability E) densities

B

4) Which pair of substances could be used to illustrate the law of multiple proportions? A) SO2, H2SO4 B) CO, CO2 C) H2O, O2 D) CH4, C6H12O6 E) NaCl, KCl

B

41) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 219.7 B) 220.4 C) 220.42 D) 218.5 E) 221.0

B

45) The element X has two naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 30.20 B) 33.20 C) 34.02 D) 35.22 E) 32.73

B

50) In the periodic table, the elements are arranged in ________. A) alphabetical order B) order of increasing atomic number C) order of increasing metallic properties D) order of increasing neutron content E) reverse alphabetical order

B

55) The elements in groups 1A, 6A, and 7A are called ________, respectively. A) alkaline earth metals, halogens, and chalcogens B) alkali metals, chalcogens, and halogens C) alkali metals, halogens, and noble gases D) alkaline earth metals, transition metals, and halogens E) halogens, transition metals, and alkali metals

B

58) An element that appears in the lower left corner of the periodic table is ________. A) either a metal or metalloid B) definitely a metal C) either a metalloid or a nonmetal D) definitely a nonmetal E) definitely a metalloid

B

60) Which one of the following molecular formulas is also an empirical formula? A) C6H6O2 B) C2H6SO C) H2O2 D) H2P4O6 E) C6H6

B

61) Which compounds do not have the same empirical formula? A) C2H2, C6H6 B) CO, CO2 C) C2H4, C3H6 D) C2H4O2, C6H12O6 E) C2H5COOCH3, CH3CHO

B

69) Which species has 54 electrons? A) Xe+ B) Te2- C) Sn2+ D) Cd E) Xe2+

B

70) Which species has 16 protons? A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O

B

71) Which species has 18 electrons? A) 39K B) 32S2- C) 35Cl D) 27Al3+ E) 64Cu2+

B

76) There are ________ protons, ________ neutrons, and ________ electrons in U+5. A) 146, 92, 92 B) 92, 146, 87 C) 92, 146, 92 D) 92, 92, 87 E) 146, 92, 146

B

8) ________-rays consist of fast-moving electrons. A) Alpha B) Beta C) Gamma D) X E) none of the above

B

9) The gold foil experiment performed in Rutherford's lab ________. A) confirmed the plum-pudding model of the atom B) led to the discovery of the atomic nucleus C) was the basis for Thomson's model of the atom D) utilized the deflection of beta particles by gold foil E) proved the law of multiple proportions

B

99) The formula for the compound formed between aluminum ions and phosphate ions is ________. A) Al3(PO4)3 B) AlPO4 C) Al(PO4)3 D) Al2(PO4)3 E) AlP

B

103) What is the molecular formula for 1-propanol? A) CH4O B) C2H6O C) C3H8O D) C4H10O E) C5H12O

C

11) Cathode rays are ________. A) neutrons B) X-rays C) electrons D) protons E) atoms

C

15) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged? A) α-rays B) α-rays, β-rays, and γ-rays C) γ-rays D) α-rays and β-rays E) α-rays and γ-rays

C

18) Of the following, the smallest and lightest subatomic particle is the ________. A) neutron B) proton C) electron D) nucleus E) alpha particle

C

28) Isotopes are atoms that have the same ________ but differing ________. A) atomic masses, charges B) mass numbers, atomic numbers C) atomic numbers, mass numbers D) charges, atomic masses E) mass numbers, charges

C

3) Consider the following selected postulates of Dalton's atomic theory: (i) Each element is composed of extremely small particles called atoms. (ii) Atoms are indivisible. (iii) Atoms of a given element are identical. (iv) Atoms of different elements are different and have different properties. Which of the postulates is(are) no longer considered valid? A) (i) and (ii) B) (ii) only C) (ii) and (iii) D) (iii) only E) (iii) and (iv)

C

30) The subatomic particles located in the nucleus with no overall charges are ________. A) electrons B) protons C) neutrons D) protons and neutrons E) protons, neutrons, and electrons

C

36) In the symbol below, x is ________. C A) the number of neutrons B) the atomic number C) the mass number D) the isotope number E) the elemental symbol

C

39) Silver has two naturally occurring isotopes with the following isotopic masses: Ar Ar 106.90509 108.9047 The average atomic mass of silver is 107.8682 amu. The fractional abundance of the lighter of the two isotopes is ________. A) 0.24221 B) 0.48168 C) 0.51835 D) 0.75783 E) 0.90474

C

43) The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 161.75 B) 162.03 C) 162.35 D) 163.15 E) 33.33

C

44) The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. A) 33.33 B) 55.74 C) 56.11 D) 57.23 E) 56.29

C

52) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) H, Li B) Cs, Ba C) Ca, Sr D) Ga, Ge E) C, O

C

54) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) As, Br B) Mg, Al C) I, At D) Br, Kr E) N,O

C

56) Which pair of elements below should be the most similar in chemical properties? A) C and O B) B and As C) I and Br D) K and Kr E) Cs and He

C

65) An empirical formula always indicates ________. A) which atoms are attached to which in a molecule B) how many of each atom are in a molecule C) the simplest whole-number ratio of different atoms in a compound D) the isotope of each element in a compound E) the geometry of a molecule

C

66) The molecular formula of a compound is always ________ the empirical formula. A) more complex than B) different from C) an integral multiple of D) the same as E) simpler than

C

7) The charge on an electron was determined in the ________. A) cathode ray tube, by J. J. Thomson B) Rutherford gold foil experiment C) Millikan oil drop experiment D) Dalton atomic theory E) atomic theory of matter

C

73) Which species is an isotope of 39Cl? A) 40Ar+ B) 34S2- C) 36Cl- D) 80Br E) 39Ar

C

75) There are ________ protons, ________ neutrons, and ________ electrons in I-. A) 131, 53, 54 B) 131, 53, 52 C) 53, 78, 54 D) 53, 131, 52 E) 78, 53, 72

C

78) Which of the following compounds would you expect to be ionic? A) H2O B) CO2 C) SrCl2 D) SO2 E) H2S

C

80) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine C) sulfur, fluorine D) potassium, lithium E) barium, bromine

C

93) A correct name for Fe(NO3)2 is ________. A) iron nitrite B) ferrous nitrite C) ferrous nitrate D) ferric nitrite E) ferric nitrate

C

97) Which one of the following polyatomic ions has the same charge as the hydroxide ion? A) ammonium B) carbonate C) nitrate D) sulfate E) phosphate

C

102) The correct name for Ni(CN)2 is ________. A) nickel (I) cyanide B) nickel cyanate C) nickel carbonate D) nickel (II) cyanide E) nickel (I) nitride

D

12) Cathode rays are deflected away from a negatively charged plate because ________. A) they are not particles B) they are positively charged particles C) they are neutral particles D) they are negatively charged particles E) they are emitted by all matter

D

17) Of the three types of radioactivity characterized by Rutherford, which type does not become deflected by a magnetic field? A) β-rays B) α-rays and β-rays C) α-rays D) γ-rays E) α-rays, β-rays, and γ-rays

D

21) Which atom has the largest number of neutrons? A) phosphorus-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40

D

22) There are ________ electrons, ________ protons, and ________ neutrons in an atom of Xe. A) 132, 132, 54 B) 54, 54, 132 C) 78, 78, 54 D) 54, 54, 78 E) 78, 78, 132

D

33) In the symbol shown below, x = ________. C A) 7 B) 13 C) 12 D) 6 E) not enough information to determine

D

37) Which one of the following basic forces is so small that it has no chemical significance? A) weak nuclear force B) strong nuclear force C) electromagnetism D) gravity E) Coulomb's law

D

40) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of ________. A) hydrogen B) oxygen C) sodium D) carbon E) helium

D

46) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. The other isotope has an abundance of 30.9%. The atomic weight (amu) of the second isotope is ________ amu. A) 63.2 B) 63.8 C) 64.1 D) 64.8 E) 28.1

D

5) Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric field? A) Both beta and gamma are deflected in the same direction, while alpha shows no response. B) Both alpha and gamma are deflected in the same direction, while beta shows no response. C) Both alpha and beta are deflected in the same direction, while gamma shows no response. D) Alpha and beta are deflected in opposite directions, while gamma shows no response. E) Only alpha is deflected, while beta and gamma show no response.

D

57) An element in the upper right corner of the periodic table ________. A) is either a metal or metalloid B) is definitely a metal C) is either a metalloid or a nonmetal D) is definitely a nonmetal E) is definitely a metalloid

D

63) Which type of formula provides the most information about a compound? A) empirical B) molecular C) simplest D) structural E) chemical

D

68) Of the following, ________ contains the greatest number of electrons. A) P3+ B) P C) P2- D) P3- E) P2+

D

74) Which one of the following species has as many electrons as it has neutrons? A) 1H B) 40Ca2+ C) 14C D) 19F- E) 14C2+

D

82) Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. What would be the most likely formula for the compound formed between sodium and the polyatomic ion X? A) NaX B) Na2X C) Na2X2 D) Na3X E) Na3X2

D

83) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group ________ of the Periodic Table of Elements. A) 3A B) 4A C) 5A D) 6A E) 7A

D

85) Which formula/name pair is incorrect? A) Mn(NO2)2 manganese(II) nitrite B) Mg(NO3)2 magnesium nitrate C) Mn(NO3)2 manganese(II) nitrate D) Mg3N2 magnesium nitrite E) Mg(MnO4)2 magnesium permanganate

D

87) Which one of the following is the formula of hydrochloric acid? A) HClO3 B) HClO4 C) HClO D) HCl E) HClO2

D

92) The correct name for NaHCO3 is ________. A) sodium hydride B) persodium carbonate C) persodium hydroxide D) sodium bicarbonate E) carbonic acid

D

95) The proper formula for the hydronium ion is ________. A) H- B) OH- C) N3- D) H3O+ E) NH4+

D

101) Which metal forms cations of differing charges? A) K B) Cs C) Ba D) Al E) Sn

E

16) Of the three types of radioactivity characterized by Rutherford, which are particles? A) β-rays B) α-rays, β-rays, and γ-rays C) γ-rays D) α-rays and γ-rays E) α-rays and β-rays

E

23) An atom of the most common isotope of gold, Au, has ________ protons, ________ neutrons, and ________ electrons. A) 197, 79, 118 B) 118, 79, 39 C) 79, 197, 197 D) 79, 118, 118 E) 79, 118, 79

E

29) The nucleus of an atom does not contain ________. A) protons B) protons or neutrons C) neutrons D) subatomic particles E) electrons

E

35) In the symbol below, x = ________. O A) 17 B) 8 C) 6 D) 7 E) not enough information to determine

E

51) Elements ________ exhibit similar physical and chemical properties. A) with similar chemical symbols B) with similar atomic masses C) in the same period of the periodic table D) on opposite sides of the periodic table E) in the same group of the periodic table

E

59) Elements in the same group of the periodic table typically have ________. A) similar mass numbers B) similar physical properties only C) similar chemical properties only D) similar atomic masses E) similar physical and chemical properties

E

6) Which one of the following is not true concerning cathode rays? A) They originate from the negative electrode. B) They travel in straight lines in the absence of electric or magnetic fields. C) They impart a negative charge to metals exposed to them. D) They are made up of electrons. E) The characteristics of cathode rays depend on the material from which they are emitted.

E

67) Formulas that show how atoms are attached in a molecule are called ________. A) molecular formulas B) ionic formulas C) empirical formulas D) diatomic formulas E) structural formulas

E

81) Which species below is the nitride ion? A) Na+ B) NO3- C) NO2- D) NH4+ E) N3-

E

86) Which formula/name pair is incorrect? A) FeSO4 iron(II) sulfate B) Fe2(SO3)3 iron(III) sulfite C) FeS iron(II) sulfide D) FeSO3 iron(II) sulfite E) Fe2(SO4)3 iron(III) sulfide

E

91) The correct name for MgF2 is ________. A) monomagnesium difluoride B) magnesium difluoride C) manganese difluoride D) manganese bifluoride E) magnesium fluoride

E

96) The charge on the ________ ion is -3. A) sulfate B) acetate C) permanganate D) oxide E) nitride

E