Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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Technological development often occurs
a. | by accident. | b. | long after the basis research is
complete. | c. | in order go learn basic information. | d. | only to make
money. |
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2.
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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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3.
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A measure of the quantity of matter is
a. | density. | c. | volume. | b. | weight. | d. | mass. |
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4.
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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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5.
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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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6.
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If a mixture is not uniform throughout, it is called
a. | homogeneous. | c. | chemically bonded. | b. | heterogeneous. | d. | a solution. |
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7.
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The symbol mm represents
a. | micrometer. | c. | milliliter. | b. | millimeter. | d. | meter. |
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8.
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Which of these metric units is used to measure mass?
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9.
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The liter is defined as
a. | 1000 m3. | c. | 1000 g3. | b. | 1000 cm3. | d. | 1000
c3. |
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10.
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Which of these symbols represents a unit of volume?
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11.
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Which of these is a measure of the amount of material?
a. | density | c. | volume | b. | weight | d. | mass |
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12.
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A sample of gold has a mass of 96.5 g and a volume of 5.00 cm3. The
density of gold is
a. | 0.0518 g/cm3. | c. | 101.5
g/cm3. | b. | 19.3 g/cm3. | d. | 483
g/cm3. |
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13.
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What is the density of 37.72 g of material whose volume is 6.80
cm3?
a. | 0.180 g/cm3 | c. | 30.9 g/cm3 | b. | 5.55
g/cm3 | d. | 256.
g/cm3 |
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14.
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100 milliliters is equivalent to
a. | 1 hectoliter. | c. | 1 centiliter. | b. | 1 microliter. | d. | 1 deciliter. |
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15.
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The number of significant figures in the measurement 0.000 305 kg is
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16.
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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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17.
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Dalton's atomic theory agrees with modern atomic theory except for
the statement that
a. | all matter is made up of small particles. | b. | atoms are not
divided in chemical reactions. | c. | atoms of the same element are chemically
alike. | d. | all atoms of the same element have the same mass. |
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18.
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Because most particles fired at metal foil passed straight through, Rutherford
concluded that
a. | atoms were mostly empty space. | c. | electrons formed the
nucleus. | b. | atoms contained no charged particles. | d. | atoms were
indivisible. |
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19.
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The tritium atom consists of
a. | one proton, two neutrons, and two electrons. | b. | one proton, one
neutron, and one electron. | c. | one proton, two neutrons, and one
electron. | d. | two protons, one neutron, and one electron. |
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20.
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In determining the atomic mass of elements, the standard is the
a. | C-12 atom. | c. | H-1 atom. | b. | C-14 atom. | d. | O-16 atom. |
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21.
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Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils,
has
a. | 6 neutrons. | c. | 10 neutrons. | b. | 8 neutrons. | d. | 14 neutrons. |
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22.
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The number of atoms in 1 mol of carbon is
a. | 6.022 ´ 1022. | c. | 5.022 ´ 1022. | b. | 6.022 ´
1023. | d. | 5.022
´ 1023. |
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23.
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To determine the molar mass of an element, one must know the
element's
a. | Avogadro constant. | c. | number of isotopes. | b. | atomic number. | d. | average atomic
mass. |
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24.
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The mass of 1 mol of chromium (atomic mass 51.996 amu) is
a. | 12 g. | c. | 51.996 g. | b. | 198 g. | d. | 6.02 ´
1023 g. |
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25.
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A prospector finds 39.39 g of pure gold (atomic mass 196.9665 amu). She
has
a. | 1.204 ´ 1023 atoms of Au. | c. | 4.306 ´ 1023 atoms of Au. | b. | 2.308 ´ 1023 atoms of Au. | d. | 6.022 ´
1023 atoms of Au. |
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26.
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The emission of electrons from metals that have absorbed photons is called
the
a. | interference effect. | c. | quantum effect. | b. | photoelectric effect. | d. | dual effect. |
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27.
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The specific wavelengths of light seen through a prism that are made when
high-voltage current is passed through a tube of hydrogen gas at low pressure is a
a. | line-emission spectrum. | c. | photoelectric
effect. | b. | electron configuration. | d. | continuous electromagnetic spectrum. |
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28.
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Because excited hydrogen atoms always produce the same line-emission spectrum,
scientists concluded that hydrogen
a. | had no electrons. | b. | did not release photons. | c. | released photons of
only certain energies. | d. | could only exist in the ground
state. |
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29.
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The equation E = hn helped Louis de
Broglie determine
a. | how protons and neutrons behave in the nucleus. | b. | how electron wave
frequencies correspond to specific energies. | c. | whether electrons behave as
particles. | d. | whether electrons exist in a limited number of orbits with different
energies. |
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30.
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Which model of the atom explains why excited hydrogen gas gives off certain
colors of light?
a. | the Bohr model | c. | Rutherford's model | b. | the de Broglie
model | d. | Planck's
theory |
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31.
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According to the quantum theory of an atom, in an orbital
a. | an electron's position cannot be known precisely. | b. | an electron has no
energy. | c. | electrons cannot be found. | d. | electrons travel around the nucleus on paths of
specific radii. |
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32.
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What values can the angular momentum quantum number have when n =
2?
a. |  | c. | 0, 1, 2 | b. |  | d. | 0,
1 |
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33.
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Each atomic orbital is described by its principal quantum number followed by
the
a. | value of the electron's spin state. | c. | number of electrons in the
sublevel. | b. | magnetic quantum number. | d. | letter of the sublevel. |
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34.
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How many electrons are needed to completely fill the fourth energy level?
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35.
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The statement that an electron occupies the lowest available energy orbital
is
a. | Hund's rule. | c. | Bohr's law. | b. | the Aufbau principle. | d. | the Pauli exclusion
principle. |
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36.
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The Pauli exclusion principle states that no two electrons in the same atom
can
a. | occupy the same orbital. | b. | have the same spin quantum
numbers. | c. | have the same set of quantum numbers. | d. | be at the same main energy
level. |
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37.
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Mendeleev predicted that the spaces in his periodic table represented
a. | isotopes. | c. | unstable elements. | b. | radioactive elements. | d. | undiscovered
elements. |
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38.
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The discovery of what elements added a new column to Mendeleev's periodic
table?
a. | noble gases | c. | transition elements | b. | radioactive elements | d. | metalloids |
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39.
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The principle that states that the physical and chemical properties of the
elements are periodic functions of their atomic numbers is
a. | the periodic table. | c. | the law of properties. | b. | the periodic
law. | d. | Mendeleev's
law. |
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40.
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The periodic law states that
a. | no two electrons with the same spin can be found in the same place in an
atom. | b. | the physical and chemical properties of the elements are functions of their atomic
numbers. | c. | electrons exhibit properties of both particles and waves. | d. | the chemical
properties of elements can be grouped according to periodicity but physical properties
cannot. |
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41.
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Elements in a group or column in the periodic table can be expected to have
similar
a. | atomic masses. | c. | numbers of neutrons. | b. | atomic numbers. | d. | properties. |
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42.
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The electron configurations of the noble gases from neon to radon in the
periodic table make these elements part of the
a. | f block. | c. | s block. | b. | d block. | d. | p block. |
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43.
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The electron configuration of an element is [Kr] 4d6
5s1. To what group does this element belong?
a. | Group 4 | c. | Group 7 | b. | Group 5 | d. | Group 9 |
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44.
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The group of soft, silvery, reactive metals, all of which have one electron in
an s orbital, is known as the
a. | alkaline-earth metals. | c. | alkali metals. | b. | transition metals. | d. | metalloids. |
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45.
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In the alkaline-earth group, atoms with the smallest radii
a. | are the most reactive. | b. | have the largest volume. | c. | are all
gases. | d. | have the highest ionization energies. |
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46.
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Which is the best reason that the atomic radius generally increases with atomic
number in each group of elements?
a. | The nuclear charge increases. | b. | The number of neutrons
increases. | c. | The number of occupied energy levels increases. | d. | A new octet
forms. |
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47.
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The ionization energies required to remove successive electrons from one mole of
calcium atoms are 590 kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of
calcium is probably
a. | Ca+. | c. | Ca3+. | b. | Ca2+. | d. | Ca4+. |
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48.
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As independent particles, most atoms are
a. | at relatively high potential energy. | c. | very stable. | b. | at relatively low
potential energy. | d. | part of a
chemical bond. |
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49.
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The B—F bond in BF3 (electronegativity for B is 2.0;
electronegativity for F is 4.0) is
a. | polar covalent. | c. | nonpolar covalent. | b. | ionic. | d. | metallic. |
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50.
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What is the correct Lewis structure for hydrogen chloride, HCl?  
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51.
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The chemical formula for an ionic compound represents the
a. | number of atoms in each molecule. | b. | number of ions in each
molecule. | c. | ratio of the combined ions present in a sample. | d. | total number of ions
in the crystal lattice. |
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52.
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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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53.
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In an ionic compound, the orderly arrangement of ions in a crystal is the state
of
a. | maximum potential energy. | c. | average potential
energy. | b. | minimum potential energy. | d. | zero potential energy. |
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54.
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If the lattice energy of compound A is greater than that of compound B,
a. | compound A is not an ionic compound. | b. | the bonds in compound A are stronger than the
bonds in compound B. | c. | compound B is probably a
gas. | d. | compound A has larger crystals than compound B. |
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55.
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How many electrons must be shown in the Lewis structure of the hydroxide ion,
OH–?
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56.
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The shiny appearance of a metal is most closely related to the
metal's
a. | highly mobile valence electrons. | c. | brittle crystalline
structure. | b. | covalent bonds. | d. | positive ions. |
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57.
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VSEPR theory is a model for predicting
a. | the strength of metallic bonds. | c. | lattice energy
values. | b. | the shape of molecules. | d. | ionization energy. |
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58.
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According to VSEPR theory, the shape of an AB3 molecule is
a. | trigonal-planar. | c. | linear. | b. | tetrahedral. | d. | bent. |
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59.
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The mixing of two or more atomic orbitals of similar energies on the same atom
to produce new orbitals of equal energies is called
a. | VSEPR theory. | c. | hybridization. | b. | malleability. | d. | dipole-dipole
interaction. |
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60.
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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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61.
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What is the formula for barium hydroxide?
a. | BaOH | c. | Ba(OH)2 | b. | BaOH2 | d. | Ba(OH) |
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62.
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Name the compound CF4.
a. | calcium fluoride | c. | carbon tetrafluoride | b. | carbon fluoride | d. | monocalcium
quadrafluoride |
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63.
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Name the compound SO3.
a. | sulfur trioxide | c. | selenium trioxide | b. | silver trioxide | d. | sodium trioxide |
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64.
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What is the oxidation number of oxygen in H2O2?
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65.
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What is the oxidation number of sulfur in SO2?
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66.
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Name the compound N2O2 using the Stock system.
a. | dinitrogen monoxide | c. | nitrogen(II) oxide | b. | nitrogen dioxide | d. | nitrogen
oxide(II) |
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67.
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The molar mass of an element is the mass of one
a. | atom of the element. | c. | gram of the element. | b. | crystal of the element. | d. | mole of the
element. |
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68.
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What is the sum of the atomic masses of all the atoms in a formula for a
compound?
a. | molecular mass | c. | atomic mass | b. | formula mass | d. | actual mass |
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69.
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The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37
g?
a. | 0.3998 mol | c. | 2.500 mol | b. | 1.333 mol | d. | 36.32 mol |
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70.
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What is the mass of 0.240 mol glucose,
C6H12O6?
a. | 24.0 g | c. | 180.16 g | b. | 43.2 g | d. | 750. g |
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71.
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The empirical formula is always the accepted formula for a(n)
a. | atom. | c. | molecular compound. | b. | molecule. | d. | ionic compound. |
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72.
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A compound's empirical formula is NO2. If the formula mass is 92
amu, what is the molecular formula?
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73.
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What is the molecular formula of a compound that has a formula mass of 50.48 amu
and an empirical formula of CH3Cl?
a. | CHCl | c. | CH3Cl | b. | CH2Cl | d. | CH2Cl2 |
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74.
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In a chemical reaction
a. | the mass of the reactants equals the mass of the products. | b. | the mass of the
products is greater than the mass of reactants. | c. | the number of atoms in the reactants and
products must change. | d. | energy as heat must be added to the
reactants. |
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75.
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When a solid produced by a chemical reaction separates from the solution it is
called
a. | a precipitate. | c. | a molecule. | b. | a reactant. | d. | the mass of the
product. |
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76.
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Which coefficients correctly balance the formula equation
NH4NO2(s)® N2(g) +
H2O(l)?
a. | 1, 2, 2 | c. | 2, 1, 1 | b. | 1, 1, 2 | d. | 2, 2, 2 |
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77.
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The equation AX ® A + X is the general equation
for a
a. | synthesis reaction. | c. | combustion reaction. | b. | decomposition reaction. | d. | single-displacement
reaction. |
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78.
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Some acids, such as carbonic acid, decompose to nonmetal oxides and
a. | water. | c. | oxygen. | b. | a salt. | d. | peroxide. |
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79.
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In a double-displacement reaction, hydrogen chloride and sodium hydroxide react
to produce sodium chloride. Another product is
a. | sodium hydride. | c. | water. | b. | potassium chloride. | d. | hydrogen gas. |
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80.
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Some metals, such as iron, react with steam to produce hydrogen gas and a
a. | metal hydroxide. | c. | metallic acid. | b. | metal hydride. | d. | metal oxide. |
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81.
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If chlorine gas is produced by halogen replacement, the other halogen in the
reaction must be
a. | bromine. | c. | astatine. | b. | iodine. | d. | fluorine. |
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82.
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The formulas for the products of the reaction between sodium hydroxide and
sulfuric acid are
a. | Na2SO4 and H2O. | c. | SI4 and
Na2O. | b. | NaSO4 and H2O. | d. | S + O2 and
Na. |
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83.
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An element in the activity series can replace any element
a. | in the periodic table. | c. | above it on the list. | b. | below it on the
list. | d. | in its
group. |
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84.
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Which branch of chemistry deals with the mass relationships of elements in
compounds and the mass relationships among reactants and products in chemical reactions?
a. | qualitative analysis | c. | chemical kinetics | b. | entropy | d. | stoichiometry |
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Use the table below to answer the following questions.
| Element | Symbol | Atomic
Mass | | Bromine | Br | 79.90 | | Calcium | Ca | 40.08 | | Carbon | C | 12.01 | | Chlorine | Cl | 35.45 | | Cobalt | Co | 58.93 | | Copper | Cu | 63.55 | | Fluorine | F | 19.00 | | Hydrogen | H | 1.01 | | Iodine | I | 126.90 | | Iron | Fe | 55.85 | | Lead | Pb | 207.2 | | Magnesium | Mg | 24.30 | | Mercury | Hg | 200.59 | | Nitrogen | N | 14.01 | | Oxygen | O | 15.00 | | Potassium | K | 39.10 | | Sodium | Na | 22.99 | | Sulfur | S | 32.01 | | | |
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85.
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For the reaction represented by the equation 2H2 + O2
® 2H2O, how many grams of water are produced from 6.00 mol
of hydrogen?
a. | 2.00 g | c. | 54.0 g | b. | 6.00 g | d. | 108 g |
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86.
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For the reaction represented by the equation 2Na + Cl2 ® 2NaCl, how many grams of chlorine gas are required to react completely
with 2.00 mol of sodium?
a. | 35.5 g | c. | 141.8 g | b. | 70.9 g | d. | 212.7 g |
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87.
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According to the kinetic-molecular theory, gases condense into liquids because
of
a. | gravity. | c. | forces between molecules. | b. | atmospheric
pressure. | d. | elastic
collisions. |
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88.
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Which process can be explained by the kinetic-molecular theory?
a. | combustion | c. | condensation | b. | oxidation | d. | displacement
reactions |
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89.
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By which process do gases take the shape of their container?
a. | evaporation | c. | adhesion | b. | expansion | d. | diffusion |
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90.
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Which of these best describes vaporization?
a. | the process by which a liquid changes to a gas | b. | the process by which
a solid changes to a gas | c. | Both (a) and (b) | d. | Neither (a) nor
(b) |
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91.
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The energy of the particles in a solid is
a. | higher than the energy of the particles in a gas. | b. | high enough to allow
the particles to interchange with other particles. | c. | higher than the energy of the particles in a
liquid. | d. | lower than the energy of the particles in liquids and
gases. |
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92.
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In general, most substances are
a. | least dense in the liquid state. | b. | more dense as gases than as
solids. | c. | less dense as solids than as liquids. | d. | most dense in the solid
state. |
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93.
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What is the total three-dimensional array of points that describes the
arrangement of the particles of a crystal called?
a. | unit cell | c. | diffraction pattern | b. | crystal lattice | d. | crystalline
system |
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94.
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According to the figure below, what is the most volatile substance
shown?  a. | benzene | c. | toluene | b. | water | d. | aniline |
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95.
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Convert the pressure 2.50 atm to kPa.
a. | 1 kPa | c. | 760 kPa | b. | 253 kPa | d. | 1000 kPa |
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96.
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According to Avogadro's law, 1 L of H2(g) and 1 L of
O2(g) at the same temperature and pressure
a. | have the same mass. | b. | have unequal volumes. | c. | contain 1 mol of gas
each. | d. | contain equal numbers of molecules. |
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97.
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Knowing the mass and volume of a gas at STP allows one to calculate the
a. | identity of the gas. | c. | condensation point of the gas. | b. | molar mass of the
gas. | d. | rate of diffusion of
the gas. |
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98.
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When pressure, volume, and temperature are known, the ideal gas law can be used
to calculate
a. | the chemical formula. | c. | molar amount. | b. | the ideal gas constant. | d. | rate of
effusion. |
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Use the table below to answer the following questions.
Element | Atomic Mass | | Argon | 39.948 | | Bromine | 79.904 | | Carbon | 12.011 | | Chlorine | 35.453 | | Fluorine | 18.998 | | Helium | 4.0026 | | Hydrogen | 1.0079 | | Nitrogen | 14.007 | | Oxygen | 15.999 | | |
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99.
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How many times greater is the rate of effusion of molecular fluorine than that
of molecular bromine at the same temperature and pressure?
a. | 2.051 | c. | 4.450 | b. | 3.062 | d. | 7.280 |
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100.
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A sample of helium diffuses 4.57 times faster than an unknown gas diffuses. What
is the molar mass of the unknown gas?
a. | 12 g/mol | c. | 38.8 g/mol | b. | 18.2 g/mol | d. | 83.5 g/mol |
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