Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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The
shape of a book is a ________________ a. | chemical change | c. | chemical property | b. | physical
change | d. | physical
property | | | | |
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2.
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A
student took a flask containing a colorless liquid and evaporated the liquid. After the liquid
had evaporated, she observed a yellow, crystalline solid in the flask. The liquid was most
likely a __________ a. | mixture | c. | element | b. | metal | d. | compound | | | | |
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3.
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A
container holds a mixture of sugar and tiny bits of glass. How can the mixture be
separated? a. | Use a
magnet. | c. | Dissolve in
water, filter and collect sugar on filter paper. | b. | Pick the glass
out of the sugar with your bare hands. | d. | Dissolve in water, filter, and collect the glass on filter
paper. | | | | |
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4.
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Directions: Use the following diagram to answer the
question.
The diagram above shows the same substance in
different states of matter (A, B, C). Which of the following statements is a true
interpretation of the diagram? a. | The particles in “A” exhibit absolutely no
motion. | c. | The particles in
“C” represent the gaseous state | b. | The particles in “B” occupy the entire volume of the
container. | d. | The particles in
“B” represent the condensed state of the particles in
“A”. | | | | |
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5.
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Directions: Use the following diagram to answer the
question.
Which statement correctly describes the
compressibility of solids, liquids, and gases?
a. | Solids, liquids,
and gases cannot be compressed. | c. | Solids and gases
can be greatly compressed; liquids cannot be greatly compressed. | b. | Solids, liquids,
and gases can all be greatly compressed. | d. | Solids and liquids cannot be greatly compressed; gases can be
greatly compressed. | | | | |
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6.
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The
following is a list of observations from the lab activity.
Which step(s) of the lab involve(s) a chemical
change?
a. | Steps I and
II | c. | Step
IV | b. | Step
II | d. | Steps I, II and
III | | | | |
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7.
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An
irregularly shaped solid object made of copper is placed into a graduated cylinder containing
water. The density of copper is 8.96 g/mL.
The approximate volume of the irregularly shaped
object would be __________. a. | 21.0 mL | c. | 13.0 mL | b. | 20.5
mL | d. | 8.0
mL | | | | |
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8.
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The
volume of another copper (density = 8.96 g.mL) object is found to be 13.0 mL. The mass of this
object, calculated to the correct number of significant digits, would be __________ a. | 116
g | c. | 4.04
g | b. | 22.0
g | d. | 0.689
g | | | | |
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9.
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A
group of students collected samples of equal volume of several different liquids, such as dish
detergent, vinegar, molasses, and shampoo. They placed the liquids in identical graduated
cylinders and measured the amount of time it took for a marble to drop from the top of the liquid to
the bottom. What were the students measuring?
a. | buoyancy | c. | density | b. | pressure | d. | viscosity | | | | |
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10.
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How
many electrons does an atom of element 97 contain?
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11.
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Air
mainly contains the gases: oxygen, nitrogen, and carbon dioxide. It could be classified
as ________ a. | an
element | c. | a
compound | b. | a mixture | d. | a colloid | | | | |
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12.
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The
nucleus of an atom has a _______ charge. a. | positive | c. | neutral | b. | negative | d. | positive
and negative | | | | |
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13.
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All
atoms of the same element have the same _____________.
a. | mass
number | c. | number of
neutrons | b. | number of protons | d. | atomic | | | | |
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14.
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An
isotope of bromine (Br) has 40 neutrons. What is the mass number for this
isotope?
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15.
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To
determine the atomic mass of an element, you must consider the ________________ of every isotope of
that element.
a. | electron
configuration | c. | number of
protons and electrons | b. | number of neutrons | d. | weighted average of the masses | | | | |
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16.
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Which
of the following characteristics did Mendeleev use to arrange the periodic table? a. | atomic
mass | c. | atomic
number | b. | isotopics mass | d. | electron charge | | | | |
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17.
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The
element Boron in group 3 would have a valence number of _______.
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18.
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Directions: Use the diagram below to help you answer the
question.
The electron configuration of the element X is shown
in the above diagram. What is element X?
a. | helium | c. | manganese | b. | calcium | d. | magnesium | | | | |
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19.
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Directions: Use the diagram below to help you answer the
question.
An “s” sublevel can hold a maximum of how
many electrons?
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20.
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Directions: Use the diagram below to help you answer the
question.
The maximum number of electrons that can occupy the
third energy level is ______.
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21.
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Directions. Refer to the periodic tables, located at the front of this
test booklets, to help you answer the question.
Which element is correctly matched to its electron
configuration?
a. | sodium -
1s22s22p63s23p4 | c. | nickel -
1s22s22p63s23p64s23d6 | b. | potassium -
1s22s22p63s23p3 | d. | oxygen -
1s22s22p4 | | | | |
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22.
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Directions. Refer to the periodic tables, located at the front of this
test booklets, to help you answer the question.
Which element has an electron configuration of
1s22s22p63s23p5?
a. | carbon | c. | chlorine | b. | calcium | d. | neon | | | | |
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23.
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Directions. Refer to the periodic tables, located at the front of this
test booklets, to help you answer the question.
The placement of the elements into the columns on the periodic table
is based on the
a. | order that elements were
discovered. | c. | similarity of
color of the elements. | b. | similarity of chemical and physical
properties. | d. | alphabetical
order of the elements. | | | | |
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24.
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From
its position on the periodic table, which element would be most likely to lose an
electron? (Hint: This element will have a positive charge).
a. | calcium
(Ca) | c. | sulfur
(S) | b. | chlorine
(Cl) | d. | neon
(Ne) | | | | |
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25.
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From
its position on the periodic table, the element with the highest ionization energy is
______. a. | beryllium
(Be) | c. | fluorine
(F) | b. | strontium
(Sr) | d. | xenon
(Xe) | | | | |
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26.
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An
anion is any atom or group of atoms with
a. | a positive
charge. | c. | no
charge. | b. | a negative charge. | d. | more electrons that the corresponding
atoms. | | | | |
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27.
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The
compound MgCl2, would
a. | share electrons. | c. | be a polar covalent compound. | b. | be electrically
neutral. | d. | form double and
triple bonds. | | | | |
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28.
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What
is the name of the Cl1- ion?
a. | chloride ion | c. | chlorate ion | b. | chlorine
ion | d. | chlorous
ion | | | | |
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29.
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The
formula for the ammonium ion is __________.
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30.
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What
is the name of AgNO3?
a. | silver nitrate | c. | silver nitrogen trioxide | b. | argon
nitrate | d. | argon nitrogen
trioxide | | | | |
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31.
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What
is the chemical formula for copper (II) phosphate?
a. | Co3(PO4)2 | c. | Cu3(PO4)2 | b. | Cu2PO4 | d. | Cu2(PO4)3 | | | | |
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32.
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What
is the name of Ca(OH)2?
a. | calcium dioxygen dihydride | c. | calcium dihydroxide | b. | calcium
hydroxide (II) | d. | calcium
hydroxide | | | | |
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33.
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The
element magnesium usually foms +2 ions. Sulfate, a polyatomic ion, has a charge of -2.
What is the formula for magnesium sulfate?
a. | Mg2SO4 | c. | Mg2(SO4)2 | b. | MgSO4 | d. | Mg2SO2 | | | | |
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34.
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A
sodium ion has a charge of +1. The formula for the polyatomic ion, carbonate, is
CO32-. What is the formula for sodium carbonate?
a. | NaCO3 | c. | CO3Na2 | b. | Na(CO3)2 | d. | Na2CO3 | | | | |
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35.
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What
is the name of BaCl2?
a. | barium chloride | c. | barium (II) chloride | b. | monobarium
chloride | d. | barium
bichloride | | | | |
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36.
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What
is the formula for potassium fluoride?
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