Central Science: Chapter 2 Flashcards


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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

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.

B

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

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

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

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

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

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

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

11

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

C

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

13

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

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

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

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

17

Of the three types of radioactivity characterized by Rutherford, which type does not become deflected by a electric 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

18

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

C

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

21

Which of the following atoms has the smallest number of neutrons?
A) carbon-14
B) chlorine-35
C) carbon-12
D) carbon-13
E) bromine-79

C

22

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

D

23

An atom of the most common isotope of gold, 197Au, 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

24

Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 63 29Cu?
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

25
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Which isotope has 45 neutrons?

B

26
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Which pair of atoms constitutes a pair of isotopes of the same element?

B

27
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Which isotope has 36 electrons in an atom?

A

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

29

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

E

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

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

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

33

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

D

34

In the symbol below, X = ________.
13 6X
A) N
B) C
C) Al
D) K
E) not enough information to determine

B

35

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

E

36

In the symbol below, x is ________.
x 6C
A) the number of neutrons
B) the atomic number
C) the mass number
D) the number of electrons
E) the elemental symbol

C

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

38

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

B

39

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

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

41
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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

42
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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

43
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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
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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

45
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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

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

47
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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

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) increasing atomic mass

B

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

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

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

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, Br
D) Br, Kr
E) N, O

C

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

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

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

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

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

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

62

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

A

63

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

D

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

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

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

68

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

D

69
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Which species has 54 electrons?

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) 45Sc3+

B

72

Which of the following species contains 18 electrons?
A) 31P
B) 34S2-
C) 36Cl
D) 80Br-
E) 16O

B

73

Which of the following species is an isotope of 79Br?
A) 40Ar+
B) 34S2-
C) 79Br-
D) 80Br
E) 79Se

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

75

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

C

76

There are ________ protons, ________ neutrons, and ________ electrons in 238U+5.
A) 146, 92, 92
B) 92, 146, 87
C) 92, 146, 92
D) 92, 92, 87
E) 146, 92, 97

B

77
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Which species contains 68 neutrons?

A

78

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

C

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

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

81

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

E

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

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

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

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

87

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

D

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

91

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

E

92

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

D

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

94

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

A

95

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

D

96

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

E

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

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

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

100

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

A

101

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

E

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

103

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

C

104

Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an illustration of the law of ________.
A) constant composition
B) multiple proportions
C) conservation of matter
D) conservation of mass
E) octaves

B

105

________ and ________ reside in the atomic nucleus.
A) Protons, electrons
B) Electrons, neutrons
C) Protons, neutrons
D) Neutrons, only neutrons
E) none of the above

C

106

520 pm is the same as ________ Å.
A) 5200
B) 52
C) 520
D) 5.2
E) 0.00052

D

107

The atomic number indicates ________.
A) the number of neutrons in a nucleus
B) the total number of neutrons and protons in a nucleus
C) the number of protons or electrons in a neutral atom
D) the number of atoms in 1 g of an element
E) the number of different isotopes of an element

C

108

The nucleus of an atom contains ________.
A) electrons
B) protons, neutrons, and electrons
C) protons and neutrons
D) protons and electrons
E) protons

C

109

In the periodic table, the elements touching the steplike line are known as ________.
A) transition elements
B) noble gases
C) metalloids
D) nonmetals
E) metals

C

110

Which group in the periodic table contains only nonmetals?
A) 1A
B) 6A
C) 2B
D) 2A
E) 8A

E

111

Horizontal rows of the periodic table are known as ________.
A) periods
B) groups
C) metalloids
D) metals
E) nonmetals

A

112

Vertical columns of the periodic table are known as ________.
A) metals
B) periods
C) nonmetals
D) groups
E) metalloids

D

113

Elements in Group 1A are known as the ________.
A) chalcogens
B) alkaline earth metals
C) alkali metals
D) halogens
E) noble gases

C

114

Elements in Group 2A are known as the ________.
A) alkaline earth metals
B) alkali metals
C) chalcogens
D) halogens
E) noble gases

A

115

Elements in Group 6A are known as the ________.
A) alkali metals
B) chalcogens
C) alkaline earth metals
D) halogens
E) noble gases

B

116

Elements in Group 7A are known as the ________.
A) chalcogens
B) alkali metals
C) alkaline earth metals
D) halogens
E) noble gases

D

117

Elements in Group 8A are known as the ________.
A) halogens
B) alkali metals
C) alkaline earth metals
D) chalcogens
E) noble gases

E

118

Potassium is a ________ and chlorine is a ________.
A) metal, nonmetal
B) metal, metal
C) metal, metalloid
D) metalloid, nonmetal
E) nonmetal, metal

A

119

Lithium is a ________ and magnesium is a ________.
A) nonmetal, metal
B) nonmetal, nonmetal
C) metal, metal
D) metal, metalloid
E) metalloid, metalloid

C

120

Oxygen is a ________ and nitrogen is a ________.
A) metal, metalloid
B) nonmetal, metal
C) metalloid, metalloid
D) nonmetal, nonmetal
E) nonmetal, metalloid

D

121

Calcium is a ________ and silver is a ________.
A) nonmetal, metal
B) metal, metal
C) metalloid, metal
D) metal, metalloid
E) nonmetal, metalloid

B

122

________ are found uncombined, as monatomic species in nature.
A) Noble gases
B) Chalcogens
C) Alkali metals
D) Alkaline earth metals
E) Halogens

A

123

When a metal and a nonmetal react, the ________ tends to lose electrons and the ________ tends to gain electrons.
A) metal, metal
B) nonmetal, nonmetal
C) metal, nonmetal
D) nonmetal, metal
E) None of the above; these elements share electrons.

C

124

The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is ________.
A) C12H14O6
B) CHO
C) CH2O
D) C6H7O3
E) C2H4O

D

125

________ only form ions with a 2+ charge.
A) Alkaline earth metals
B) Halogens
C) Chalcogens
D) Alkali metals
E) Transition metals

A

126

What is the formula of the compound formed between strontium ions and nitrogen ions?
A) SrN
B) Sr3N2
C) Sr2N3
D) SrN2
E) SrN3

B

127

Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X?
A) K2X
B) KX2
C) K2X3
D) K2X2
E) KX

A

128

The charge on the manganese in the salt MnF3 is ________.
A) 1+
B) 1-
C) 2+
D) 2-
E) 3+

E

129

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be ________.
A) oxygen
B) fluorine
C) chlorine
D) nitrogen
E) sulfur

D

130

Sodium forms an ion with a charge of ________.
A) 1+
B) 1-
C) 2+
D) 2-
E) 0

A

131

Potassium forms an ion with a charge of ________.
A) 2+
B) 1-
C) 1+
D) 2-
E) 0

C

132

Calcium forms an ion with a charge of ________.
A) 1-
B) 2-
C) 1+
D) 2+
E) 0

D

133

Barium forms an ion with a charge of ________.
A) 1+
B) 2-
C) 3+
D) 3-
E) 2+

E

134

Aluminum forms an ion with a charge of ________.
A) 2+
B) 3-
C) 1+
D) 3+
E) 1-

D

135

Fluorine forms an ion with a charge of ________.
A) 1-
B) 1+
C) 2+
D) 3+
E) 3-

A

136

Iodine forms an ion with a charge of ________.
A) 7-
B) 1+
C) 2-
D) 2+
E) 1-

E

137

Oxygen forms an ion with a charge of ________.
A) 2-
B) 2+
C) 3-
D) 3+
E) 6+

A

138

Sulfur forms an ion with a charge of ________.
A) 2+
B) 2-
C) 3+
D) 6-
E) 6+

B

139

Predict the empirical formula of the ionic compound that forms from sodium and fluorine.
A) NaF
B) Na2F
C) NaF2
D) Na2F3
E) Na3F2

A

140

Predict the empirical formula of the ionic compound that forms from magnesium and fluorine.
A) Mg2F3
B) MgF
C) Mg2F
D) Mg3F2
E) MgF2

E

141

Predict the empirical formula of the ionic compound that forms from magnesium and oxygen.
A) Mg2O
B) MgO
C) MgO2
D) Mg2O2
E) Mg3O2

B

142

Predict the empirical formula of the ionic compound that forms from aluminum and oxygen.
A) AlO
B) Al3O2
C) Al2O3
D) AlO2
E) Al2O

C

143

The correct name for K2S is ________.
A) potassium sulfate
B) potassium disulfide
C) potassium bisulfide
D) potassium sulfide
E) dipotassium sulfate

D

144

The correct name for Al2O3 is ________.
A) aluminum oxide
B) dialuminum oxide
C) dialuminum trioxide
D) aluminum hydroxide
E) aluminum trioxide

A

145

The correct name for CaH2 is ________.
A) hydrocalcium
B) calcium dihydride
C) calcium hydroxide
D) calcium dihydroxide
E) calcium hydride

E

146

The correct name for SO is ________.
A) sulfur oxide
B) sulfur monoxide
C) sulfoxide
D) sulfate
E) sulfite

B

147

The correct name for CCl4 is ________.
A) carbon chloride
B) carbon tetrachlorate
C) carbon perchlorate
D) carbon tetrachloride
E) carbon chlorate

D

148

The correct name for N2O5 is ________.
A) nitrous oxide
B) nitrogen pentoxide
C) dinitrogen pentoxide
D) nitric oxide
E) nitrogen oxide

C

149

The correct name for H2CO3 is ________.
A) carbonous acid
B) hydrocarbonate
C) carbonic acid
D) carbohydrate
E) carbohydric acid

C

150

The correct name for H2SO3 is ________.
A) sulfuric acid
B) sulfurous acid
C) hydrosulfuric acid
D) hydrosulfic acid
E) sulfur hydroxide

B

151

The correct name for H2SO4 is ________.
A) sulfuric acid
B) sulfurous acid
C) hydrosulfuric acid
D) hydrosulfic acid
E) sulfur hydroxide

A

152

The correct name for HNO3 is ________.
A) nitrous acid
B) nitric acid
C) hydronitroxide acid
D) nitroxide acid
E) nitrogen hydroxide

B

153

The correct name for HClO3 is ________.
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hydrochlorous acid

C

154

The correct name for HClO is ________.
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hypochlorous acid

E

155

The correct name for HBrO4 is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hydrobromous acid

B

156

The correct name for HBrO is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hypobromous acid

E

157

The correct name for HBrO2 is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hydrobromous acid

D

158

The correct name for HClO2 is ________.
A) perchloric acid
B) chloric acid
C) hypochlorous acid
D) hypychloric acid
E) chlorous acid

E

159

The correct name of the compound Na3N is ________.
A) sodium nitride
B) sodium azide
C) sodium trinitride
D) sodium(III) nitride
E) trisodium nitride

A

160

The formula of bromic acid is ________.
A) HBr
B) HBrO4
C) HBrO
D) HBrO3
E) HBrO2

D

161

The correct formula for molybdenum (IV) hypochlorite is ________.
A) Mo(ClO3)4
B) Mo(ClO)4
C) Mo(ClO2)4
D) Mo(ClO4)4
E) MoCl4

B

162

The name of PCl3 is ________.
A) potassium chloride
B) phosphorus trichloride
C) phosphorous(III) chloride
D) monophosphorous trichloride
E) trichloro potassium

B

163

The ions Ca2+ and PO43- form a salt with the formula ________.
A) CaPO4
B) Ca2(PO4)3
C) Ca2PO4
D) Ca(PO4)2
E) Ca3(PO4)2

E

164

The correct formula of iron (III) bromide is ________.
A) FeBr2
B) FeBr3
C) FeBr
D) Fe3Br3
E) Fe3Br

B

165

Magnesium and sulfur form an ionic compound with the formula ________.
A) MgS
B) Mg2S
C) MgS2
D) Mg2S2
E) Mg2S3

A

166

The formula of ammonium carbonate is ________.
A) (NH4)2CO3
B) NH4CO2
C) (NH3)2CO4
D) (NH3)2CO3
E) N2(CO3)3

A

167

The formula of the chromate ion is ________.
A) CrO4 2-
B) CrO2 3-
C) CrO-
D) CrO32-
E) CrO2-

A

168

The formula of the carbonate ion is ________.
A) CrO22-
B) CrO32-
C) CrO33-
D) CO2 -
E) CO-

B

169

The correct name for Mg(ClO3)2 is ________.
A) magnesium chlorate
B) manganese chlorate
C) magnesium chloroxide
D) magnesium perchlorate
E) manganese perchlorate

A

170

What is the correct formula for ammonium sulfide?
A) NH4SO3
B) (NH4)2SO4
C) (NH4)2S
D) NH3S
E) N2S3

C

171

When calcium reacts with sulfur the compound formed is ________.
A) Ca2S2
B) Ca3S2
C) CaS
D) CaS2
E) Ca2S3

C

172

Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is ________.
A) chromium chlorine
B) chromium (III) chloride
C) monochromium trichloride
D) chromium (III) trichloride
E) chromic trichloride

B

173

Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this compound is ________.
A) iron chlorine
B) iron (III) chloride
C) moniron trichloride
D) iron (III) trichloride
E) ferric trichloride

B

174

Copper and chlorine form an ionic compound whose formula is CuCl2. The name of this compound is ________.
A) copper chlorine
B) copper (III) dichloride
C) monocopper dichloride
D) copper (II) dichloride
E) cupric chloride

E

175

The name of the binary compound N2O4 is ________.
A) nitrogen oxide
B) nitrous oxide
C) nitrogen (IV) oxide
D) dinitrogen tetroxide
E) oxygen nitride

D

176

The formula for zinc phosphate is Zn3(PO4)2. What is the formula for cadmium arsenate?
A) Cd4(AsO2)3
B) Cd3(AsO4)2
C) Cd3(AsO3)4
D) Cd2(AsO4)3
E) Cd2(AsO4)4

B

177

The formula for aluminum hydroxide is ________.
A) AlOH
B) Al3OH
C) Al2(OH)3
D) Al(OH)3
E) Al2O3

D

178

The name of the ionic compound V2O3 is ________.
A) vanadium (III) oxide
B) vanadium oxide
C) vanadium (II) oxide
D) vanadium (III) trioxide
E) divanadium trioxide

A

179

The name of the ionic compound NH4CN is ________.
A) nitrogen hydrogen cyanate
B) ammonium carbonitride
C) ammonium cyanide
D) ammonium hydrogen cyanate
E) cyanonitride

C

180

The name of the ionic compound (NH4)3PO4 is ________.
A) ammonium phosphate
B) nitrogen hydrogen phosphate
C) tetrammonium phosphate
D) ammonia phosphide
E) triammonium phosphate

A

181

What is the formula for perchloric acid?
A) HClO
B) HClO3
C) HClO4
D) HClO2
E) HCl

C

182

The correct name for HIO2 is ________.
A) hypoiodic acid
B) hydriodic acid
C) periodous acid
D) iodous acid
E) periodic acid

D

183

What is the molecular formula for propane?
A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10

C

184

What is the molecular formula for butane?
A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10

E

185

What are the primary atoms found in alkanes?
A) carbon, hydrogen, and oxygen
B) carbon and nitrogen
C) oxygen and hydrogen
D) carbon and oxygen
E) carbon and hydrogen

E

186

What is the correct name for the following alkane, C5H12?
A) heptane
B) propane
C) hexane
D) pentane
E) butane

D

187

How many carbon and hydrogen atoms are found in decane?
A) 10 carbons and 22 hydrogens
B) 9 carbons and 20 hydrogens
C) 10 carbons and 20 hydrogens
D) 9 carbons and 18 hydrogens
E) 10 carbons and 24 hydrogens

A

188

What is the molecular formula for heptane?
A) C6H12
B) C6H14
C) C7H14
D) C7H16
E) C7H18

D

189

What is the molecular formula for 1-hexanol?
A) C6H13O
B) C6H14O
C) C6H15O
D) C7H14O
E) C7H15O

B

190

A certain mass of carbon reacts with 128 g of oxygen to form carbon monoxide. ________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions.
A) 25.6
B) 64.0
C) 128
D) 1280
E) 256

E

191

An atom of 13C contains ________ protons.
A) 6
B) 19
C) 7
D) 9
E) 13

A

192

Of the following, the subatomic particle with the smallest mass is the ________.
A) proton
B) neutron
C) electron
D) alpha particle
E) isotope

C

193

An atom of 118Xe contains ________ neutrons.
A) 54
B) 172
C) 64
D) 110
E) 118

C

194

There are ________ protons, ________ electrons, and ________ neutrons in an atom of Xe.
A) 129, 129, 129
B) 129, 129, 75
C) 54, 75, 129
D) 54, 54, 75
E) 54, 54, 129

D

195

An atom of 14C contains ________ electrons.
A) 14
B) 20
C) 8
D) 10
E) 6

E

196

87 pm is the same as ________ Angstroms.
A) 870
B) 8.7
C) 87
D) .87
E) .087

D

197

200 pm is the same as ________ Å.
A) 2000
B) 20
C) 200
D) 2
E) 0.0002

D

198

In the symbol below, X = ________.
40 19X
A) Zr
B) K
C) Sc
D) Br
E) not enough information to determine

B

199

In the symbol below, x = ________.
X 17Cl
A) 17
B) 34
C) 16
D) 36
E) not enough information to determine

E

200

The mass number of an atom of 14C is ________.
A) 6
B) 20
C) 8
D) 14
E) 10

D

201

Which atom has the largest number of neutrons?
A) silicon-30
B) sulfur-36
C) argon-38
D) calcium-44
E) magnesium-24

D

202

How many neutrons are there in one atom of 184W?
A) 74
B) 112
C) 258
D) 110
E) 184

D

203

How many protons are there in one atom of 71Ga?
A) 40
B) 70
C) 71
D) 31
E) 13

D

204

How many electrons are there in one atom of 71Ga?
A) 40
B) 70
C) 71
D) 31
E) 13

D

205
card image

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

B

206

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

B

207

How many total electrons are in the Li+ ion?
A) 2
B) 3
C) 4
D) 7
E) 8

A

208

How many total electrons are in the O2- ion?
A) 10
B) 8
C) 6
D) 16
E) 4

A

209

If a iron atom loses 2 electrons to make an ion, what is the charge on that ion?
A) 2+
B) 1+
C) 3+
D) 2-
E) 1-

A

210

If an atom gains 3 electrons to make an ion, what is the charge on that ion?
A) 3+
B) 1+
C) 2+
D) 1-
E) 3-

E

211
card image

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) 33.333
B) 220.40
C) 220.24
D) 219.00
E) 219.67

B

212
card image

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) 159.4
B) 162.0
C) 163.1
D) 161.5
E) 163.0

B

213
card image

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) 52.62
B) 56.14
C) 55.70
D) 55.40
E) 55.74

B

214

The element ________ is the most similar to helium in chemical and physical properties.
A) O
B) Mg
C) Be
D) Ar
E) Sr

D

215

Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?
A) Li, F
B) Sr, Te
C) O, S
D) In, Sb
E) Ti, Ne

C

216

Which one of the following is a metalloid?
A) Se
B) Hf
C) Zr
D) Xe
E) Si

E

217

The element lithium is in a group known as the ________.
A) transition metals
B) alkaline earth metals
C) noble gases
D) halogens
E) alkali metals

E

218

The element chlorine is in a group known as the ________.
A) transition metals
B) noble gases
C) alkali metals
D) alkaline earth metals
E) halogens

E

219

The element calcium is in a group known as the ________.
A) transition metals
B) alkali metals
C) halogens
D) noble gases
E) alkaline earth metals

E

220

Of the following, only ________ is not a metalloid.
A) B
B) Po
C) Si
D) Ge
E) As

B

221

Which of the following elements is a nonmetal?
A) At
B) Rh
C) Tc
D) Mo
E) Zr

A

222

Which one of the following will occur as diatomic molecules in elemental form?
A) helium
B) argon
C) chlorine
D) phosphorous
E) sodium

C

223

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

B

224

How many protons does the Br- ion possess?
A) 34
B) 36
C) 6
D) 8
E) 35

E

225

Which one of the following is most likely to gain electrons when forming an ion?
A) Mn
B) Zn
C) F
D) Li
E) Al

C

226

The formula of a salt is XCl2 . The X-ion in this salt has 24 electrons. The metal X is ________.
A) Ni
B) Fe
C) Zn
D) Cr
E) Ti

B

227

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

D

228

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

E

229

Which of the following compounds would you expect to be ionic?
A) C2H6
B) NH3
C) H2O2
D) LiBr
E) None of the above.

D

230

Which species below is the sulfate ion?
A) CN-
B) SO4 2-
C) OH-
D) SO3 2-
E) None of the above

B

231

Which species below is the nitrate ion?
A) NO2-
B) NO3-
C) ClO3-
D) ClO4-
E) MnO4-

B

232

Which species below is the chromate ion?
A) Cr2O7 2-
B) CrO4 2-
C) CH3COO-
D) CO3 2-
E) None of the above

B

233

The correct name for CaO is ________.
A) calcium oxide
B) calcium hydroxide
C) calcium peroxide
D) calcium monoxide
E) calcium dioxide

A

234

Element M reacts with fluorine to form an ionic compound with the formula M . The M-ion has 21 electrons. Element M is ________.
A) Al
B) Cr
C) Mn
D) Fe
E) Sc

B

235

The charge on the copper ion in the salt CuO is ________.
A) +1
B) +2
C) +4
D) +3
E) +5

B

236

The charge on the silver ion in the salt AgCl is ________.
A) +2
B) +1
C) +3
D) +4
E) +5

B

237

The name of the ionic compound NaBrO4 is ________.
A) sodium perbromate
B) sodium bromate
C) sodium hypobromate
D) sodium perbromite
E) sodium bromide

A

238

When a bromine atom forms the bromide ion, it has the same charge as the ________ ion.
A) sulfide
B) ammonium
C) nitrate
D) phosphate
E) sulfite

C

239

Which element forms an ion with the same charge as the sulfate ion?
A) magnesium
B) sodium
C) fluorine
D) vanadium
E) sulfur

E

240

The correct name for Na2O2 is ________.
A) sodium oxide
B) sodium dioxide
C) disodium dioxide
D) sodium peroxide
E) disodium oxide

D

241

Which metal is not required to have its charge specified in the names of ionic compounds it forms?
A) Cr
B) Ni
C) Zr
D) Na
E) Mo

D

242

The following hypothetical element : x : can be found in which group on the periodic table?

VIA

243

Which element is found in Period 2 and Group VIIA?

fluorine

244

The formula for potassium sulfide is ________.

K2S

245

What is the name of an alcohol derived from hexane?

hexanol

246

The possible oxidation numbers for iron are +1 and +2.

false

247

The formula for chromium (II) iodide is CrI2.

true

248

H2SeO4 is called selenic acid.

true

249

The correct name for Na3N is sodium azide.

false