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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?
iron(III) sulfide
A) Fe2 (SO4 )3
B) Fe2 (SO3 )3
C) FeSO4
D) FeS
E) FeSO3
1)
iron(III) sulfite
iron(II) sulfate
iron(II) sulfide
iron(II) sulfite
2) Which isotope has 36 electrons in an atom?
80
78
34
Kr
Se
Cl
A)
B)
C)
36
34
17
36
Hg
D)
80
3) Which one of the following molecular formulas is also an empirical formula?
A) H2 O2
B) C6 H6O2
C) H2 P4O6
D) C2 H6SO
80
Br
E)
35
E) C6 H6
2)
3)
4) In the Rutherford nuclear-atom model, __________.
A) the heavy subatomic particles, protons and neutrons, reside in the nucleus
B) mass is spread essentially uniformly throughout the atom
C) the light subatomic particles, protons and neutrons, reside in the nucleus
D) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially
the same mass
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
4)
5) Which of the following compounds would you expect to be ionic?
A) SF6
B) CaO
C) NH3
D) H2 O
5)
6) Which metal does not form cations of differing charges?
A) Cu
B) Fe
C) Na
D) Co
E) H2 O2
E) Sn
7) 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.
Isotope
31X
34X
A) 34.02
Abundance (%)
35.16
64.84
B) 33.20
Mass (amu)
31.16
34.30
C) 32.73
1
D) 30.20
E) 35.22
6)
7)
8) An element in the upper right corner of the periodic table __________.
A) is either a metal or metalloid
B) is definitely a metalloid
C) is definitely a non-metal
D) is definitely a metal
E) is either a metalloid or a non-metal
8)
9) Elements in the same group of the periodic table typically have __________.
A) similar physical and chemical properties
B) similar physical properties only
C) similar chemical properties only
D) similar atomic masses
E) similar mass numbers
9)
10) Which species below is the nitride ion?
A) Na +
B) N 3-
10)
C) NO2-
D) NH4+
E) NO3-
11) Cathode rays are deflected away from a negatively charged plate because __________.
A) they are not particles
B) they are negatively charged particles
C) they are positively charged particles
D) they are neutral particles
E) they are emitted by all matter
11)
12) A molecular formula always indicates __________.
A) the simplest whole-number ratio of different atoms in a compound
B) the isotope of each element in a compound
C) which atoms are attached to which in a molecule
D) the geometry of a molecule
E) how many of each atom are in a molecule
12)
13) Which isotope has 45 neutrons?
34
78
Cl
Se
A)
B)
17
34
103
Rh
C)
45
80
Br
D)
35
80
Kr
E)
36
14) 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.
Isotope
15X
17X
16X
A) 17.20
Abundance (%)
28.60
13.30
58.10
B) 17.65
Mass (amu)
15.33
17.26
18.11
C) 16.90
2
D) 16.90
E) 17.11
13)
14)
15) Of the three types of radioactivity characterized by Rutherford, which is/are not particles?
A) -rays, -rays, and -rays
B) -rays and -rays
C) -rays
D) -rays
E) -rays
15)
16) Which pair of elements is most apt to form an ionic compound with each other?
A) nitrogen, hydrogen
B) sulfur, fluorine
C) barium, bromine
D) oxygen, fluorine
E) calcium, sodium
16)
17) Isotopes are atoms that have the same number of __________ but differing number of __________.
A) electrons, protons
B) protons, neutrons
C) neutrons, electrons
D) neutrons, protons
E) protons, electrons
17)
18) Which species below is the nitrate ion?
A) NO3B) NH4+
18)
D) N3-
C) N3 -
19) The atomic number of an atom of 80Br is __________.
A) 45
B) 35
C) 115
D) 73
20) Which one of the following is the formula of hydrochloric acid?
A) HClO
B) HCl
C) HClO2
D) HClO3
21) An atom of 131I contains __________ electrons.
A) 53
B) 131
C) 124
D) 184
E) NO2-
E) 80
E) HClO4
E) 78
19)
20)
21)
22) 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) Cl
B) K
C) Ca
D) Ar
E) None of the above could be the unknown element.
22)
23) Of the following, only __________ is not a metalloid.
A) Ge
B) Si
C) As
23)
3
D) Al
E) B
24) Which compounds do not have the same empirical formula?
A) CO, CO2
24)
B) C2 H4, C3 H6
C) C2 H2, C6 H6
D) C2 H4O2, C6H12O6
E) C2 H5COOCH3 , CH3CHO
25) 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.
Isotope
38X
39X
42X
A) 41.54
Abundance
5.07
15.35
79.85
25)
Mass
37.919
39.017
42.111
B) 38.64
C) 33.33
D) 39.68
E) 39.07
26) The elements in groups 1A, 6A, and 7A are called, __________, respectively.
A) alkali metals, halogens, and noble gases
B) halogens, transition metals, and alkali metals
C) alkaline earth metals, transition metals, and halogens
D) alkali metals, chalcogens, and halogens
E) alkaline earth metals, halogens, and chalcogens
27) Which species has 16 protons?
A) 31P
B) 34S2-
C) 16O
D) 80Br-
26)
E) 36Cl
28) In the symbol below, x is __________.
x
C
6
27)
28)
A) the mass number
B) the number of neutrons
C) the isotope number
D) the atomic number
E) the elemental symbol
29) How many electrons does the Al3+ ion possess?
A) 10
B) 0
C) 6
D) 13
30) Which element forms an ion with the same charge as the ammonium ion?
A) potassium
B) calcium
C) oxygen
D) nitrogen
E) 16
E) chlorine
31) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is __________.
A) Cs
B) Cd
C) Pd
D) Ag
E) Cu
4
29)
30)
31)
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
53X
56X
58X
Abundance
19.61
53.91
26.48
A) 56.11
32)
Mass
52.62
56.29
58.31
B) 55.74
C) 33.33
33) What is the molecular formula for n-propanol?
A) C5 H11OH
B) CH3OH
C) C3 H7OH
D) 57.23
E) 56.29
D) C2 H5OH
E) C4 H9OH
33)
34) Which one of the following does not occur as diatomic molecules in elemental form?
A) oxygen
B) nitrogen
C) bromine
D) hydrogen
E) sulfur
34)
35) There are __________ electrons, __________ protons, and __________ neutrons in an atom of
132
Xe.
54
35)
A) 54, 54, 78
B) 78, 78, 132
C) 78, 78, 54
D) 54, 54, 132
E) 132, 132, 54
36) Which pair of elements is most apt to form a molecular compound with each other?
A) sulfur, fluorine
B) barium, bromine
C) magnesium, iodine
D) potassium, lithium
E) aluminum, oxygen
36)
37) In the absence of magnetic or electric fields, cathode rays __________.
A) bend toward a light source
B) travel in straight lines
C) cannot be detected
D) do not exist
E) become positively charged
37)
38) The correct name for Na2 O2 is _________.
38)
A) disodium oxide
B) sodium peroxide
C) sodium oxide
D) sodium dioxide
E) disodium dioxide
39) Which one of the following is most likely to lose electrons when forming an ion?
A) F
B) S
C) Rh
D) P
5
E) N
39)
40) The molecular formula of a compound is always __________ the empirical formula.
A) the same as
B) an integral multiple of
C) different from
D) more complex than
E) simpler than
40)
41) Which of the following compounds would you expect to be ionic?
A) H2 S
B) SO2
C) H2 O
D) CO2
E) SrCl2
42) Which of the following elements is a metaloid?
A) B
B) Ga
C) C
E) In
D) Se
41)
42)
43) Different isotopes of a particular element contain the same number of __________.
A) protons and neutrons
B) subatomic particles
C) protons, neutrons, and electrons
D) neutrons
E) protons
43)
44) Of the following, the smallest and lightest subatomic particle is the __________.
A) electron
B) neutron
C) proton
D) alpha particle
E) nucleus
44)
45) Which one of the following is not one of the postulates of Dalton's atomic theory?
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.
45)
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?
A) (iii) only
B) (ii) only
C) (i) and (ii)
D) (ii) and (iii)
E) (iii) and (iv)
46)
6
47) Elements __________ exhibit similar physical and chemical properties.
A) with similar atomic masses
B) in the same group of the periodic table
C) with similar chemical symbols
D) on opposite sides of the periodic table
E) in the same period of the periodic table
47)
48) The charge on the iron ion in the salt Fe2 O3 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.
A) phosphate
B) sulfite
C) ammonium
D) sulfide
E) nitrate
49)
50) All atoms of a given element have the same __________.
A) number of electrons and neutrons
B) density
C) number of protons
D) mass
E) number of neutrons
50)
51) Which metal forms cations of differing charges?
A) Sn
B) Cs
C) K
51)
D) Al
E) Ba
52) 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.
Isotope
221X
220X
218X
A) 221.0
Abundance
74.22
12.78
13.00
B) 219.7
52)
Mass
220.9
220.0
218.1
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?
A) Fe
B) Pb
C) Cu
D) Mn
E) Ca
7
53)
54) Which pair of atoms constitutes a pair of isotopes of the same element?
14
12
X
X
A)
6
6
B)
20
X
10
21
X
11
C)
17
X
9
17
X
8
D)
19
X
10
19
X
9
E)
14
X
6
14
X
7
55) In the symbol below, X = __________.
13
X
6
54)
55)
A) K
B) Al
C) C
D) N
E) not enough information to determine
56) Which atom has the largest number of neutrons?
A) calcium-40
B) chlorine-37
C) phosphorus-30
D) potassium-39
E) argon-40
56)
57) The suffix -ide is used primarily __________.
A) to indicate binary acids
B) for polyatomic cation names
C) for monatomic anion names
D) for monoatomic cations
E) for the name of the first element in a molecular compound
57)
58) Gravitational forces act between objects in proportion to their __________.
A) masses
B) charges
C) polarizability
D) volumes
E) densities
58)
59) The nucleus of an atom does not contain __________.
A) subatomic particles
B) protons or neutrons
C) neutrons
D) electrons
E) protons
59)
8
60) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope
of __________.
A) helium
B) hydrogen
C) sodium
D) oxygen
E) carbon
60)
61) An atom of 15N contains __________ neutrons.
A) 15
B) 7
C) 10
61)
D) 8
E) 22
62) Which one of the following basic forces is so small that it has no chemical significance?
A) weak nuclear force
B) electromagnetism
C) Coulomb's law
D) strong nuclear force
E) gravity
62)
63) Which pair of elements would you expect to exhibit the greatest similarity in their physical and
chemical properties?
A) O, S
B) K, Ca
C) C, N
D) H, He
E) Si, P
63)
64) There are __________ protons, __________ neutrons, and __________ electrons in 131I- .
A) 131, 53, and 54
B) 78, 53, and 72
C) 131, 53, and 52
D) 53, 131, and 52
E) 53, 78, and 54
64)
65) 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.
65)
66) Which element forms an ion with the same charge as the sulfate ion?
A) phosphorus
B) iron
C) magnesium
D) copper
E) oxygen
66)
67) The correct name for Ni(CN)2 is __________.
67)
A) 99, 1.0
B) 0.25, 99.75
C) 1.0, 99
A) nickel cyanate
B) nickel (I) nitride
C) nickel (I) cyanide
D) nickel (II) cyanide
E) nickel carbonate
9
D) 49, 51
E) 99.75, 0.25
68) Of the three types of radioactivity characterized by Rutherford, which are particles?
A) -rays
B) -rays, -rays, and -rays
C) -rays and -rays
D) -rays
E) -rays and -rays
68)
69) The charge on an electron was determined in the __________.
A) Millikan oil drop experiment
B) Rutherford gold foil experiment
C) atomic theory of matter
D) Dalton atomic theory
E) cathode ray tube, by J. J. Thompson
69)
70) Which combination of protons, neutrons, and electrons is correct for the isotope of copper,
63
Cu?
29
70)
A) 29 p+ , 34 n°, 29 eB) 63 p+ , 29 n°, 63 eC) 34 p+ , 29 n°, 34 eD) 29 p+ , 29 n°, 63 eE) 34 p+ , 34 n°, 29 e71) The charge on the __________ ion is -3.
A) oxide
B) acetate
C) nitride
D) sulfate
E) permanganate
71)
72) 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) Na2X
B) Na3X2
C) Na3X
D) Na2X2
E) NaX
72)
73) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of
__________.
A) the law of conservation of energy
B) the law of constant composition
C) the law of conservation of mass
D) the law of multiple proportions
E) none of the above
73)
74) 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) 64.8
C) 28.1
D) 64.1
E) 63.8
74)
10
75) Which one of the following compounds is chromium(III) oxide?
A) CrO3
B) Cr2 O3
C) Cr3 O2
D) Cr2 O4
E) Cr3 O
76) Predict the charge of the most stable ion of potassium.
A) 1+
B) 3+
C) 2-
E) 2+
D) 1-
75)
76)
77) The correct name for MgF2 is __________.
77)
78) The nucleus of an atom contains __________.
A) electrons
B) protons and neutrons
C) protons, neutrons, and electrons
D) protons
E) neutrons
78)
79) 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 non-metal
D) definitely a metalloid
E) definitely a non-metal
79)
A) manganese difluoride
B) magnesium fluoride
C) manganese bifluoride
D) monomagnesium difluoride
E) magnesium difluoride
80) The species __________ contains 16 neutrons.
A) 80BrB) 36Cl
C) 31P
D) 16O
E) 34S2-
81) The proper formula for the hydronium ion is __________.
A) HB) H3 O+
C) N-3
D) OH-
E) NH4+
82) In the symbol shown below, x = __________.
13
C
x
80)
81)
82)
A) 7
B) 13
C) 6
D) 12
E) not enough information to determine
83) Which one of the following is a nonmetal?
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 __________.
A) 17Ne2+
B) 17O2-
C) 19F+
11
D) 17O2+
E) 19F-
83)
84)
85) Different isotopes of a particular element contain different numbers of __________.
A) protons, neutrons, and electrons
B) protons and neutrons
C) protons
D) neutrons
E) None of the above is correct.
86) Which one of the following species has as many electrons as it has neutrons?
A) 19FB) 1 H
C) 14C2+
D) 40Ca2+
85)
E) 14C
86)
87) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically
charged?
A) -rays and -rays
B) -rays, -rays, and -rays
C) -rays
D) -rays
E) -rays and -rays
87)
88) An atom of 17O contains __________ protons.
A) 8
B) 11
C) 25
88)
89) Cathode rays are __________.
A) x-rays
B) protons
D) 17
C) atoms
D) neutrons
E) 9
E) electrons
90) Which type of formula provides the most information about a compound?
A) molecular
B) empirical
C) chemical
D) simplest
E) structural
91) Of the following, __________ contains the greatest number of electrons.
A) P3+
B) P3C) P2D) P
E) P2+
92) Which one of the following compounds is copper(I) chloride?
A) CuCl
B) Cu2Cl
C) Cu3Cl2
E) CuCl2
D) Cu2Cl3
89)
90)
91)
92)
93) In the periodic table, the elements are arranged in __________.
A) alphabetical order
B) reverse alphabetical order
C) order of increasing neutron content
D) order of increasing metallic properties
E) order of increasing atomic number
93)
94) The correct name for HNO2 is __________.
94)
A) hydrogen nitrate
B) nitric acid
C) pernitric acid
D) hyponitrous acid
E) nitrous acid
12
95) A correct name for Fe(NO3)2 is __________.
95)
96) Which formula/name pair is incorrect?
magnesium nitrite
A) Mg3N2
96)
A) ferric nitrate
B) iron nitrite
C) ferrous nitrate
D) ferric nitrite
E) ferrous nitrite
manganese(II) nitrite
B) Mn(NO2 )2
C) Mg(MnO4 )2 magnesium permanganate
D) Mg(NO3 )2
E) Mn(NO3 )2
magnesium nitrate
manganese(II) nitrate
97) The gold foil experiment performed in Rutherford's lab __________.
A) was the basis for Thomson's model of the atom
B) confirmed the plum-pudding model of the atom
C) proved the law of multiple proportions
D) utilized the deflection of beta particles by gold foil
E) led to the discovery of the atomic nucleus
97)
98) In the symbol below, x = __________.
x
C
6
98)
A) 6
B) 7
C) 13
D) 19
E) not enough information to determine
99) Which pair of elements below should be the most similar in chemical properties?
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?
A) -rays, -rays, and -rays
B) -rays
C) -rays
D) -rays and -rays
E) -rays and -rays
13
99)
100)