Ch. 2 Practice Test

Name___________________________________

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) Which formula/name pair is incorrect? 1)A) Fe2(SO4)3 iron(III) sulfideB) Fe2(SO3)3 iron(III) sulfiteC) FeSO4 iron(II) sulfateD) FeS iron(II) sulfideE) FeSO3 iron(II) sulfite

2) Which isotope has 36 electrons in an atom? 2)

A) 8036

Kr B) 7834

Se C) 3417

Cl D) 3680

Hg E) 8035

Br

3) Which one of the following molecular formulas is also an empirical formula? 3)A) H2O2 B) C6H6O2 C) H2P4O6 D) C2H6SO E) C6H6

4) In the Rutherford nuclear-atom model, __________. 4)A) the heavy subatomic particles, protons and neutrons, reside in the nucleusB) mass is spread essentially uniformly throughout the atomC) the light subatomic particles, protons and neutrons, reside in the nucleusD) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially

the same massE) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially

the same mass and mass is spread essentially uniformly throughout the atom

5) Which of the following compounds would you expect to be ionic? 5)A) SF6 B) CaO C) NH3 D) H2O E) H2O2

6) Which metal does not form cations of differing charges? 6)A) Cu B) Fe C) Na D) Co E) Sn

7) The element X has two naturally occurring isotopes. The masses (amu) and % abundances of theisotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope Abundance (%) Mass (amu)31X 35.16 31.1634X 64.84 34.30

7)

A) 34.02 B) 33.20 C) 32.73 D) 30.20 E) 35.22

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8) An element in the upper right corner of the periodic table __________. 8)A) is either a metal or metalloidB) is definitely a metalloidC) is definitely a non-metalD) is definitely a metalE) is either a metalloid or a non-metal

9) Elements in the same group of the periodic table typically have __________. 9)A) similar physical and chemical propertiesB) similar physical properties onlyC) similar chemical properties onlyD) similar atomic massesE) similar mass numbers

10) Which species below is the nitride ion? 10)A) Na+ B) N 3- C) NO2- D) NH4+ E) NO3-

11) Cathode rays are deflected away from a negatively charged plate because __________. 11)A) they are not particlesB) they are negatively charged particlesC) they are positively charged particlesD) they are neutral particlesE) they are emitted by all matter

12) A molecular formula always indicates __________. 12)A) the simplest whole-number ratio of different atoms in a compoundB) the isotope of each element in a compoundC) which atoms are attached to which in a moleculeD) the geometry of a moleculeE) how many of each atom are in a molecule

13) Which isotope has 45 neutrons? 13)

A) 3417

Cl B) 7834

Se C) 10345

Rh D) 8035

Br E) 8036

Kr

14) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of theisotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope Abundance (%) Mass (amu)15X 28.60 15.3317X 13.30 17.2616X 58.10 18.11

14)

A) 17.20 B) 17.65 C) 16.90 D) 16.90 E) 17.11

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15) Of the three types of radioactivity characterized by Rutherford, which is/are not particles? 15)A) -rays, -rays, and -raysB) -rays and -raysC) -raysD) -raysE) -rays

16) Which pair of elements is most apt to form an ionic compound with each other? 16)A) nitrogen, hydrogenB) sulfur, fluorineC) barium, bromineD) oxygen, fluorineE) calcium, sodium

17) Isotopes are atoms that have the same number of __________ but differing number of __________. 17)A) electrons, protonsB) protons, neutronsC) neutrons, electronsD) neutrons, protonsE) protons, electrons

18) Which species below is the nitrate ion? 18)A) NO3- B) NH4+ C) N3- D) N3- E) NO2-

19) The atomic number of an atom of 80Br is __________. 19)A) 45 B) 35 C) 115 D) 73 E) 80

20) Which one of the following is the formula of hydrochloric acid? 20)A) HClO B) HCl C) HClO2 D) HClO3 E) HClO4

21) An atom of 131I contains __________ electrons. 21)A) 53 B) 131 C) 124 D) 184 E) 78

22) An unknown element is found to have three naturally occurring isotopes with atomic masses of35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknownelement?

22)

A) ClB) KC) CaD) ArE) None of the above could be the unknown element.

23) Of the following, only __________ is not a metalloid. 23)A) Ge B) Si C) As D) Al E) B

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24) Which compounds do not have the same empirical formula? 24)A) CO, CO2B) C2H4, C3H6C) C2H2, C6H6D) C2H4O2, C6H12O6E) C2H5COOCH3, CH3CHO

25) Element X has three naturally occurring isotopes. The masses (amu) and % abundances of theisotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope Abundance Mass38X 5.07 37.91939X 15.35 39.01742X 79.85 42.111

25)

A) 41.54 B) 38.64 C) 33.33 D) 39.68 E) 39.07

26) The elements in groups 1A, 6A, and 7A are called, __________, respectively. 26)A) alkali metals, halogens, and noble gasesB) halogens, transition metals, and alkali metalsC) alkaline earth metals, transition metals, and halogensD) alkali metals, chalcogens, and halogensE) alkaline earth metals, halogens, and chalcogens

27) Which species has 16 protons? 27)A) 31P B) 34S2- C) 16O D) 80Br- E) 36Cl

28) In the symbol below, x is __________.x6

C

28)

A) the mass numberB) the number of neutronsC) the isotope numberD) the atomic numberE) the elemental symbol

29) How many electrons does the Al3+ ion possess? 29)A) 10 B) 0 C) 6 D) 13 E) 16

30) Which element forms an ion with the same charge as the ammonium ion? 30)A) potassium B) calcium C) oxygen D) nitrogen E) chlorine

31) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is __________. 31)A) Cs B) Cd C) Pd D) Ag E) Cu

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32) 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.

Isotope Abundance Mass53X 19.61 52.6256X 53.91 56.2958X 26.48 58.31

32)

A) 56.11 B) 55.74 C) 33.33 D) 57.23 E) 56.29

33) What is the molecular formula for n-propanol? 33)A) C5H11OH B) CH3OH C) C3H7OH D) C2H5OH E) C4H9OH

34) Which one of the following does not occur as diatomic molecules in elemental form? 34)A) oxygen B) nitrogen C) bromine D) hydrogen E) sulfur

35) There are __________ electrons, __________ protons, and __________ neutrons in an atom of13254

Xe.

35)

A) 54, 54, 78B) 78, 78, 132C) 78, 78, 54D) 54, 54, 132E) 132, 132, 54

36) Which pair of elements is most apt to form a molecular compound with each other? 36)A) sulfur, fluorineB) barium, bromineC) magnesium, iodineD) potassium, lithiumE) aluminum, oxygen

37) In the absence of magnetic or electric fields, cathode rays __________. 37)A) bend toward a light sourceB) travel in straight linesC) cannot be detectedD) do not existE) become positively charged

38) The correct name for Na2O2 is _________. 38)A) disodium oxideB) sodium peroxideC) sodium oxideD) sodium dioxideE) disodium dioxide

39) Which one of the following is most likely to lose electrons when forming an ion? 39)A) F B) S C) Rh D) P E) N

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40) The molecular formula of a compound is always __________ the empirical formula. 40)A) the same asB) an integral multiple ofC) different fromD) more complex thanE) simpler than

41) Which of the following compounds would you expect to be ionic? 41)A) H2S B) SO2 C) H2O D) CO2 E) SrCl2

42) Which of the following elements is a metaloid? 42)A) B B) Ga C) C D) Se E) In

43) Different isotopes of a particular element contain the same number of __________. 43)A) protons and neutronsB) subatomic particlesC) protons, neutrons, and electronsD) neutronsE) protons

44) Of the following, the smallest and lightest subatomic particle is the __________. 44)A) electronB) neutronC) protonD) alpha particleE) nucleus

45) Which one of the following is not one of the postulates of Dalton's atomic theory? 45)A) Atoms of an element are not changed into different types of atoms by chemical reactions:

atoms are neither created nor destroyed in chemical reactions.B) Atoms are composed of protons, neutrons, and electrons.C) Each element is composed of extremely small particles called atoms.D) All atoms of a given element are identical; the atoms of different elements are different and

have different properties.E) Compounds are formed when atoms of more than one element combine; a given compound

always has the same relative number and kind of atoms.

46) 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?

46)

A) (iii) onlyB) (ii) onlyC) (i) and (ii)D) (ii) and (iii)E) (iii) and (iv)

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47) Elements __________ exhibit similar physical and chemical properties. 47)A) with similar atomic massesB) in the same group of the periodic tableC) with similar chemical symbolsD) on opposite sides of the periodic tableE) in the same period of the periodic table

48) The charge on the iron ion in the salt Fe2O3 is __________. 48)A) +1 B) +3 C) +2 D) -6 E) -5

49) When a fluorine atom forms the fluoride ion, it has the same charge as the __________ ion. 49)A) phosphateB) sulfiteC) ammoniumD) sulfideE) nitrate

50) All atoms of a given element have the same __________. 50)A) number of electrons and neutronsB) densityC) number of protonsD) massE) number of neutrons

51) Which metal forms cations of differing charges? 51)A) Sn B) Cs C) K D) Al E) Ba

52) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of theisotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope Abundance Mass221X 74.22 220.9220X 12.78 220.0218X 13.00 218.1

52)

A) 221.0 B) 219.7 C) 220.4 D) 220.42 E) 218.5

53) Which metal is not required to have its charge specified in the names of ionic compounds it forms? 53)A) Fe B) Pb C) Cu D) Mn E) Ca

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54) Which pair of atoms constitutes a pair of isotopes of the same element? 54)

A) 146

X 126

X

B) 2010

X 2111

X

C) 179

X 178

X

D) 1910

X 199

X

E) 146

X 147

X

55) In the symbol below, X = __________.136

X

55)

A) KB) AlC) CD) NE) not enough information to determine

56) Which atom has the largest number of neutrons? 56)A) calcium-40B) chlorine-37C) phosphorus-30D) potassium-39E) argon-40

57) The suffix -ide is used primarily __________. 57)A) to indicate binary acidsB) for polyatomic cation namesC) for monatomic anion namesD) for monoatomic cationsE) for the name of the first element in a molecular compound

58) Gravitational forces act between objects in proportion to their __________. 58)A) massesB) chargesC) polarizabilityD) volumesE) densities

59) The nucleus of an atom does not contain __________. 59)A) subatomic particlesB) protons or neutronsC) neutronsD) electronsE) protons

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60) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotopeof __________.

60)

A) helium B) hydrogen C) sodium D) oxygen E) carbon

61) An atom of 15N contains __________ neutrons. 61)A) 15 B) 7 C) 10 D) 8 E) 22

62) Which one of the following basic forces is so small that it has no chemical significance? 62)A) weak nuclear forceB) electromagnetismC) Coulomb's lawD) strong nuclear forceE) gravity

63) Which pair of elements would you expect to exhibit the greatest similarity in their physical andchemical properties?

63)

A) O, S B) K, Ca C) C, N D) H, He E) Si, P

64) There are __________ protons, __________ neutrons, and __________ electrons in 131I-. 64)A) 131, 53, and 54B) 78, 53, and 72C) 131, 53, and 52D) 53, 131, and 52E) 53, 78, and 54

65) Vanadium has two naturally occurring isotopes, 50V with an atomic mass of 49.9472 amu and 51Vwith an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. The percentabundances of the vanadium isotopes are __________% 50V and __________% 51V.

65)

A) 99, 1.0 B) 0.25, 99.75 C) 1.0, 99 D) 49, 51 E) 99.75, 0.25

66) Which element forms an ion with the same charge as the sulfate ion? 66)A) phosphorusB) ironC) magnesiumD) copperE) oxygen

67) The correct name for Ni(CN)2 is __________. 67)A) nickel cyanateB) nickel (I) nitrideC) nickel (I) cyanideD) nickel (II) cyanideE) nickel carbonate

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68) Of the three types of radioactivity characterized by Rutherford, which are particles? 68)A) -raysB) -rays, -rays, and -raysC) -rays and -raysD) -raysE) -rays and -rays

69) The charge on an electron was determined in the __________. 69)A) Millikan oil drop experimentB) Rutherford gold foil experimentC) atomic theory of matterD) Dalton atomic theoryE) cathode ray tube, by J. J. Thompson

70) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 6329

Cu? 70)

A) 29 p+, 34 n°, 29 e-

B) 63 p+, 29 n°, 63 e-

C) 34 p+, 29 n°, 34 e-

D) 29 p+, 29 n°, 63 e-

E) 34 p+, 34 n°, 29 e-

71) The charge on the __________ ion is -3. 71)A) oxideB) acetateC) nitrideD) sulfateE) permanganate

72) Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. Whatwould be the most likely formula for the compound formed between sodium and the polyatomicion X?

72)

A) Na2X B) Na3X2 C) Na3X D) Na2X2 E) NaX

73) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of__________.

73)

A) the law of conservation of energyB) the law of constant compositionC) the law of conservation of massD) the law of multiple proportionsE) none of the above

74) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One ofthe isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. Theother isotope has an abundance of 30.9%. The atomic weight (amu) of the second isotope is__________ amu.

74)

A) 63.2 B) 64.8 C) 28.1 D) 64.1 E) 63.8

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75) Which one of the following compounds is chromium(III) oxide? 75)A) CrO3 B) Cr2O3 C) Cr3O2 D) Cr2O4 E) Cr3O

76) Predict the charge of the most stable ion of potassium. 76)A) 1+ B) 3+ C) 2- D) 1- E) 2+

77) The correct name for MgF2 is __________. 77)A) manganese difluorideB) magnesium fluorideC) manganese bifluorideD) monomagnesium difluorideE) magnesium difluoride

78) The nucleus of an atom contains __________. 78)A) electronsB) protons and neutronsC) protons, neutrons, and electronsD) protonsE) neutrons

79) An element that appears in the lower left corner of the periodic table is __________. 79)A) either a metal or metalloidB) definitely a metalC) either a metalloid or a non-metalD) definitely a metalloidE) definitely a non-metal

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

81) The proper formula for the hydronium ion is __________. 81)A) H- B) H3O+ C) N-3 D) OH- E) NH4+

82) In the symbol shown below, x = __________.13x

C

82)

A) 7B) 13C) 6D) 12E) not enough information to determine

83) Which one of the following is a nonmetal? 83)A) Ir B) Os C) Sr D) Br E) W

84) An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is __________. 84)

A) 17Ne2+ B) 17O2- C) 19F+ D) 17O2+ E) 19F-

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85) Different isotopes of a particular element contain different numbers of __________. 85)A) protons, neutrons, and electronsB) protons and neutronsC) protonsD) neutronsE) None of the above is correct.

86) Which one of the following species has as many electrons as it has neutrons? 86)A) 19F- B) 1H C) 14C2+ D) 40Ca2+ E) 14C

87) Of the three types of radioactivity characterized by Rutherford, which is/are not electricallycharged?

87)

A) -rays and -raysB) -rays, -rays, and -raysC) -raysD) -raysE) -rays and -rays

88) An atom of 17O contains __________ protons. 88)A) 8 B) 11 C) 25 D) 17 E) 9

89) Cathode rays are __________. 89)A) x-rays B) protons C) atoms D) neutrons E) electrons

90) Which type of formula provides the most information about a compound? 90)A) molecular B) empirical C) chemical D) simplest E) structural

91) Of the following, __________ contains the greatest number of electrons. 91)A) P3+ B) P3- C) P2- D) P E) P2+

92) Which one of the following compounds is copper(I) chloride? 92)A) CuCl B) Cu2Cl C) Cu3Cl2 D) Cu2Cl3 E) CuCl2

93) In the periodic table, the elements are arranged in __________. 93)A) alphabetical orderB) reverse alphabetical orderC) order of increasing neutron contentD) order of increasing metallic propertiesE) order of increasing atomic number

94) The correct name for HNO2 is __________. 94)A) hydrogen nitrateB) nitric acidC) pernitric acidD) hyponitrous acidE) nitrous acid

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95) A correct name for Fe(NO3)2 is __________. 95)A) ferric nitrateB) iron nitriteC) ferrous nitrateD) ferric nitriteE) ferrous nitrite

96) Which formula/name pair is incorrect? 96)A) Mg3N2 magnesium nitriteB) Mn(NO2)2 manganese(II) nitriteC) Mg(MnO4)2 magnesium permanganateD) Mg(NO3)2 magnesium nitrateE) Mn(NO3)2 manganese(II) nitrate

97) The gold foil experiment performed in Rutherford's lab __________. 97)A) was the basis for Thomson's model of the atomB) confirmed the plum-pudding model of the atomC) proved the law of multiple proportionsD) utilized the deflection of beta particles by gold foilE) led to the discovery of the atomic nucleus

98) In the symbol below, x = __________.x6

C

98)

A) 6B) 7C) 13D) 19E) not enough information to determine

99) Which pair of elements below should be the most similar in chemical properties? 99)A) Cs and He B) C and O C) I and Br D) B and As E) K and Kr

100) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged? 100)A) -rays, -rays, and -raysB) -raysC) -raysD) -rays and -raysE) -rays and -rays

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