Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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Inorganic chemistry is the study of
a. | non-carbon related compounds. | b. | the chemistry of living
things. | c. | mathematical modeling. | d. | the identification of the composition of
materials. |
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2.
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A true statement about mass is that
a. | mass if often measured with a spring scale. | b. | mass is expressed in
pounds. | c. | as the force of Earth's gravity on an object increases, the object's mass
increases. | d. | mass is determined by comparing the mass of an object with a set of standard masses
that are part of a balance. |
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3.
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Noble gases are in Group 18, and are best known because they are
a. | unreactive. | c. | rare. | b. | excellent conductors. | d. | lanthanides. |
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4.
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Which of the following is an example of a homogeneous mixture?
a. | air | c. | raw milk | b. | orange juice | d. | marble |
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5.
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Applied research is carried out in order to
a. | to solve a particular problem. | b. | by accident. | c. | to learn basic
information. | d. | in order to make money. |
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6.
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A measure of the quantity of matter is
a. | density. | c. | volume. | b. | weight. | d. | mass. |
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7.
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The vertical columns on the periodic table are called
a. | periods. | c. | groups. | b. | rows. | d. | elements. |
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8.
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A theory is best described as a
a. | series of experimental observations. | b. | generalization that explains a body of known
facts or phenomena. | c. | scientifically proven fact. | d. | testable
statement. |
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9.
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The SI base units for length and time are
a. | centimeter and second. | c. | centimeter and hour. | b. | meter and hour. | d. | meter and
second. |
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10.
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The SI base unit for time is the
a. | day. | c. | minute. | b. | hour. | d. | second. |
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11.
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Which of these statements about mass is true?
a. | Mass is expressed in pounds or newtons. | b. | Mass is usually
measured with a spring scale. | c. | The mass of an object depends on the force of
gravity acting on it. | d. | The mass of an object is determined by
comparing it to an object of known mass. |
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12.
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The number of grams equal to 0.5 kg is
a. | 0.0005. | c. | 500. | b. | 0.005. | d. | 5000. |
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13.
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The result of dividing 107 by 10–3 is
a. | 10–4. | c. | 104. | b. | 102.5. | d. | 1010. |
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14.
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In the equation density = mass/volume, mass divided by
volume has a constant value. This means that the
a. | equation graphs as a straight line. | b. | variables mass and volume are inversely
proportional. | c. | equation graphs as a hyperbola. | d. | product of mass and volume is a
constant. |
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15.
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In oxides of nitrogen, such as N2O, NO, NO2, and
N2O3, atoms combine in small whole-number ratios. This evidence supports the
law of
a. | conservation of mass. | c. | definite composition. | b. | multiple
proportions. | d. | mass
action. |
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16.
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Nuclear forces exists because the particles in the nucleus are
a. | oppositely charged. | c. | highly energized. | b. | close together. | d. | moving very
fast. |
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17.
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The smallest unit of an element that can exist either alone or in combination
with other such particles of the same or different elements is the
a. | electron. | c. | neutron. | b. | proton. | d. | atom. |
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18.
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How many moles of atoms are in 50.15 g of mercury (atomic mass 200.59
amu)?
a. | 0.1001 mol | c. | 0.2500 mol | b. | 0.1504 mol | d. | 0.4000 mol |
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19.
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A sample of tin (atomic mass 118.71 amu) contains 3.01 ´ 1023 atoms. The mass of the sample is
a. | 3.01 g. | c. | 72.6 g. | b. | 59.3 g. | d. | 11 g. |
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20.
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The distance between two successive peaks on adjacent waves is its
a. | frequency. | c. | quantum number. | b. | wavelength. | d. | velocity. |
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21.
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Which is not part of hydrogen's line-emission spectrum?
a. | Balmer series. | c. | Lyman series. | b. | Aufbau series. | d. | Paschen series. |
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22.
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A spherical electron cloud surrounding an atomic nucleus would best
represent
a. | an s orbital. | b. | a px
orbital. | c. | a combination of px and py
orbitals. | d. | a combination of an s and a px
orbital. |
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23.
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An orbital that can never exist according to the quantum description of the atom
is
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24.
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If n is the principal quantum number of a main energy level, the number
of electrons in that energy level is
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25.
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How many more electrons are needed to completely fill the third main energy
level if it already contains 8 electrons?
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26.
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The main energy level that can hold only two electrons is the
a. | first. | c. | third. | b. | second. | d. | fourth. |
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27.
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What are the radioactive elements with atomic numbers from 90 to 103
called?
a. | the noble gases | c. | the actinides | b. | the lanthanides | d. | the rare-earth
elements |
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28.
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What are the elements with atomic numbers from 58 to 71 called?
a. | the lanthanides | c. | the actinides | b. | the noble gases | d. | the alkali
metals |
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29.
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Elements to the right side of the periodic table (p-block elements) have
properties most associated with
a. | gases. | c. | metals. | b. | nonmetals. | d. | metalloids. |
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30.
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The group of 14 f block elements in the sixth period is the
a. | actinides. | c. | transition elements. | b. | lanthanides. | d. | metalloids. |
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31.
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Within the p-block elements, the elements at the top of the table,
compared with those at the bottom,
a. | have larger radii. | c. | have lower ionization energies. | b. | are more
metallic. | d. | are less
metallic. |
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32.
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The first member of the noble gas family, whose highest energy level consists of
an octet of electrons, is
a. | helium. | c. | neon. | b. | argon. | d. | krypton. |
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33.
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When an electron is added to a neutral atom, a certain amount of energy
is
a. | always absorbed. | b. | always released. | c. | either released or
absorbed. | d. | transferred to the more electronegative element. |
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34.
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The energy required to remove an electron from an atom is the atom's
a. | electron affinity. | c. | electronegativity. | b. | electron energy. | d. | ionization
energy. |
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35.
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The element that has the greatest electronegativity is
a. | oxygen. | c. | chlorine. | b. | sodium. | d. | fluorine. |
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36.
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The electrons involved in the formation of a chemical bond are called
a. | dipoles. | c. | Lewis electrons. | b. | s electrons. | d. | valence
electrons. |
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37.
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Atoms naturally move
a. | toward high potential energy. | c. | toward less
stability. | b. | toward low potential energy. | d. | away from each
other. |
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38.
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After drawing a Lewis structure, one should
a. | determine the number of each type of atom in the molecule. | b. | add unshared pairs
of electrons around nonmetal atoms. | c. | confirm that the total number of valence
electrons used equals the number available. | d. | determine the electronegativity of each
atom. |
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39.
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The chemical formula for water, a covalent compound, is H2O. This
formula is an example of a(n)
a. | formula unit. | c. | ionic formula. | b. | Lewis structure. | d. | molecular
formula. |
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40.
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The energy released when 1 mol of an ionic crystalline compound is formed from
gaseous ions is called the
a. | bond energy. | c. | lattice energy. | b. | potential energy. | d. | energy of
crystallization. |
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41.
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Shifting the layers of an ionic crystal causes the crystal to
a. | be drawn into a wire. | c. | become metallic. | b. | shatter. | d. | emit light. |
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42.
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Which hybrid orbitals help explain the bonding in methane,
CH4?
a. | sp3 orbitals | c. | pd3
orbitals | b. | sp orbitals | d. | df3 orbitals |
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43.
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Four hybrid sp3 orbitals are formed from
a. | two s orbitals and two p orbitals. | b. | an s orbital
and a p orbital. | c. | three s orbitals and one p
orbital. | d. | one s orbital and three p orbitals. |
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44.
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A chemical formula includes the symbols of the elements in the compound and
subscripts that indicate
a. | atomic mass of each element. | b. | number of atoms or ions of each element that
are combined in the compound. | c. | formula mass. | d. | charges on the
elements or ions. |
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45.
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What is the formula for the compound formed by calcium ions and chloride
ions?
a. | CaCl | c. | CaCl3 | b. | Ca2Cl | d. | CaCl2 |
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46.
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What is the formula for the compound formed by lead(II) ions and chromate
ions?
a. | PbCrO4 | c. | Pb2(CrO4)3 | b. | Pb2CrO4 | d. | Pb(CrO4)2 |
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47.
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Name the compound Fe(NO3)2.
a. | iron(II) nitrate | c. | iron(III) nitrate | b. | iron(II) nitrite | d. | iron(III)
nitride |
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48.
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What is the oxidation number of a pure element?
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49.
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In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is
equal to
a. | 0. | c. | 10. | b. | the number of atoms in the
ion. | d. | the charge of the
ion. |
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50.
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A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula
for this compound?
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