1 Compared to the charge of a proton, the charge
of an electron has
(1) a greater magnitude and the same sign
(2) a greater magnitude and the opposite sign
(3) the same magnitude and the same sign
(4) the same magnitude and the opposite sign
2 Which atom has the largest atomic radius?
(1) potassium (3) francium
(2) rubidium (4) cesium
3 In the wave-mechanical model of the atom, an
orbital is defined as
(1) a region of the most probable proton location
(2) a region of the most probable electron
(3) a circular path traveled by a proton around
(4) a circular path traveled by an electron
around the nucleus
4 When an excited electron in an atom moves to
the ground state, the electron
(1) absorbs energy as it moves to a higher
(2) absorbs energy as it moves to a lower energy
(3) emits energy as it moves to a higher energy
(4) emits energy as it moves to a lower energy
5 Which polyatomic ion is found in the compound
represented by the formula NaHCO 3?
(1) acetate (3) hydrogen sulfate
(2) hydrogen carbonate (4) oxalate
6 The atomic mass of magnesium is the weighted
average of the atomic masses of
(1) all of the artificially produced isotopes of Mg
(2) all of the naturally occurring isotopes of Mg
(3) the two most abundant artificially produced
isotopes of Mg
(4) the two most abundant naturally occurring
isotopes of Mg
7 Which element has atoms that can form halide
(1) iodine (3) strontium
(2) silver (4) xenon
8 Two forms of solid carbon, diamond and
graphite, differ in their physical properties due
to the differences in their
(1) atomic numbers
(2) crystal structures
(3) isotopic abundances
(4) percent compositions
9 Which quantity can be calculated for a solid
compound, given only the formula of the com-
pound and the Periodic Table of the Elements?
(1) the density of the compound
(2) the heat of fusion of the compound
(3) the melting point of each element in the
(4) the percent composition by mass of each
element in the compound
10 Which terms identify types of chemical
(1) decomposition and sublimation
(2) decomposition and synthesis
(3) deposition and sublimation
(4) deposition and synthesis
11 The greatest amount of energy released per
gram of reactants occurs during a
(1) redox reaction
(2) fission reaction
(3) substitution reaction
(4) neutralization reaction
12 Which element has atoms with the strongest
attraction for electrons in a chemical bond?
(1) chlorine (3) fluorine
(2) nitrogen (4) oxygen
13 Compared to the physical and chemical proper-
ties of the compound NO 2, the compound N 2O
(1) different physical properties and different
(2) different physical properties and the same
(3) the same physical properties and different
(4) the same physical properties and the same
14 Which phrase describes a molecule of CH 4, in
terms of molecular polarity and distribution of
(1) polar with an asymmetrical distribution of
(2) polar with a symmetrical distribution of
(3) nonpolar with an asymmetrical distribution
(4) nonpolar with a symmetrical distribution of
15 Which sample of copper has atoms with the
lowest average kinetic energy?
(1) 10. g at 45°C (3) 30. g at 25°C
(2) 20. g at 35°C (4) 40. g at 15°C
16 Which change results in the formation of
(1) burning of propane
(2) melting of NaCl(s)
(3) deposition of CO 2(g)
(4) solidification of water
17 Which substance can not be broken down by a
(1) ammonia (3) propanal
(2) ethanol (4) zirconium
18 According to Table I, which equation represents
a change resulting in the greatest quantity of
(1) 2C(s) + 3H 2(g) → C 2H 6(g)
(2) 2C(s) + 2H 2(g) → C 2H 4(g)
(3) N 2(g) + 3H 2(g) → 2NH 3(g)
(4) N 2(g) + O 2(g) → 2NO(g)
19 Which element is a liquid at STP?
(1) bromine (3) francium
(2) cesium (4) iodine
20 Which statement describes a reversible reaction
(1) The activation energy of the forward
reaction must equal the activation energy of
the reverse reaction.
(2) The rate of the forward reaction must equal
the rate of the reverse reaction.
(3) The concentration of the reactants must
equal the concentration of the products.
(4) The potential energy of the reactants must
equal the potential energy of the products.
21 Given the balanced equation representing a
O 2 → O + O
What occurs during this reaction?
(1) Energy is absorbed as bonds are broken.
(2) Energy is absorbed as bonds are formed.
(3) Energy is released as bonds are broken.
(4) Energy is released as bonds are formed.
22 In terms of entropy and energy, systems in
nature tend to undergo changes toward
(1) lower entropy and lower energy
(2) lower entropy and higher energy
(3) higher entropy and lower energy
(4) higher entropy and higher energy
23 Which term is defined as the difference
between the potential energy of the products
and the potential energy of the reactants in a
(1) activation energy (3) heat of fusion
(2) thermal energy (4) heat of reaction
24 What is the atomic number of the element
whose atoms bond to each other in chains, rings,
(1) 10 (3) 6
(2) 8 (4) 4
25 How many pairs of electrons are shared between
two adjacent carbon atoms in a saturated
(1) 1 (3) 3
(2) 2 (4) 4
26 Given the balanced equation representing a
4Al(s) + 3O 2(g) → 2Al 2O 3(s)
As the aluminum loses 12 moles of electrons,
(1) gains 4 moles of electrons
(2) gains 12 moles of electrons
(3) loses 4 moles of electrons
(4) loses 12 moles of electrons
27 Which compound is an electrolyte?
(1) CH 3CHO (3) CH 3COOH
(2) CH 3OCH 3 (4) CH 3CH 2CH 3
28 Which statement describes one acid-base
(1) An acid is an H + acceptor, and a base is an
H + donor.
(2) An acid is an H + donor, and a base is an H +
(3) An acid is an H - acceptor, and a base is an
H - donor.
(4) An acid is an H - donor, and a base is an H -
29 Which compounds are classified as Arrhenius
(1) HCl and NaOH
(2) HNO 3 and NaCl
(3) NH 3 and H 2CO 3
(4) HBr and H 2SO 4
30 Which statement describes the stability of the
nuclei of potassium atoms?
(1) All potassium atoms have stable nuclei that
(2) All potassium atoms have unstable nuclei
that do not spontaneously decay.
(3) Some potassium atoms have unstable nuclei
that spontaneously decay.
(4) Some potassium atoms have unstable nuclei
that do not spontaneously decay.
31 Which notations represent different isotopes of
the element sodium?
(1) 32S and 34S (3) Na + and Na 0
(2) S 2- and S 6+ (4) 22Na and 23Na
32 Which electron configuration represents the
electrons in an atom of Ga in an excited state?
(1) 2-8-17-3 (3) 2-8-18-3
(2) 2-8-17-4 (4) 2-8-18-4
33 Which statement describes the general trends in
electronegativity and first ionization energy as
the elements in Period 3 are considered in order
from Na to Cl?
(1) Electronegativity increases, and first
ionization energy decreases.
(2) Electronegativity decreases, and first
ionization energy increases.
(3) Electronegativity and first ionization energy
(4) Electronegativity and first ionization energy
34 What is the gram-formula mass of Fe(NO 3) 3?
(1) 146 g/mol (3) 214 g/mol
(2) 194 g/mol (4) 242 g/mol
35 Given the balanced equation representing a
Al 2(SO 4) 3 + 6NaOH → 2Al(OH) 3 + 3Na 2SO 4
The mole ratio of NaOH to Al(OH) 3 is
(1) 1:1 (3) 3:1
(2) 1:3 (4) 3:7