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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When
two pure substances are combined so that each of the pure substances retains its own properties, the
result is a(n) ____. a. | compound | c. | element | b. | mixture | d. | isotope | | | | |
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2.
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In
general, metals are ____. a. | poor conductors of heat | c. | poor conductors of electricity | b. | brittle | d. | good conductors
of heat | | | | |
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3.
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Which
of these statements about matter is NOT true? a. | During chemical changes, matter is
destroyed. | b. | Matter has mass and takes up space. | c. | Matter can be
divided into pure substances and mixtures. | d. | Matter is made up of atoms. | | |
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4.
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Most
of the mass of an atom is found in its ____. a. | nucleus | c. | atomic number | b. | electron
cloud | d. | mass
number | | | | |
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5.
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Which
of the following CANNOT be classified as matter? a. | an odorless, colorless gas | c. | alpha particles | b. | the heat given
off by a light bulb | d. | an electron
cloud | | | | |
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6.
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The freezing
point of a substance is ____ the melting point of the same substance. a. | greater
than | c. | equal
to | b. | less
than | d. | unrelated
to | | | | |
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7.
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A cork is
able to float on water because it is ____. a. | a crystalline solid | c. | small in size | b. | equal in density to
water | d. | less dense than the
water | | | | |
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8.
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All
of the following are a state of matter EXCEPT ____. a. | solid | c. | liquid | b. | gas | d. | density | | | | |
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9.
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All
of the following are examples of physical changes except ____. a. | melting | c. | burning | b. | evaporating | d. | solidifying | | | | |
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10.
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All
of the following are examples of chemical weathering except ____. a. | acid
rain | c. | rocks breaking
because of ice | b. | cave formations | d. | pollution | | | | |
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11.
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Which
of the following is an example of a physical change? a. | evaporation in a
swamp cooler | c. | digestion of a
hamburger | b. | electricity produced by a dry
cell | d. | rusting of a car
body | | | | |
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12.
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Which
of the following is an example of a chemical change? a. | bending a pop
can | c. | melting
wax | b. | evaporation of
milk | d. | burning
paper | | | | |
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13.
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The
particles that make up an atom are ____. a. | electrons, protons, and nuclei | c. | protons, neutrons, and nuclei | b. | elements, protons, and
electrons | d. | protons, neutrons, and
electrons | | | | |
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14.
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Dot diagrams
are used to represent ____. a. | protons | c. | atomic mass | b. | valence electrons | d. | the structure of the nucleus | | | | |
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15.
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The energy
levels of an atom are occupied by ____. a. | electrons | c. | neutrons | b. | protons | d. | ions | | | | |
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16.
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The maximum
number of electrons in the second energy level of an atom is ____.
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17.
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In the
compound, H2O, the electrons in the bonds are unequally shared between oxygen and
hydrogen, forming ____. a. | cations | c. | nonpolar covalent molecules | b. | ionic
bonds | d. | polar covalent
bonds | | | | |
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18.
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Alkali
metals tend to lose one electron per atom in forming bonds. What family of elements will form ionic
bonds with alkali metals, in a 2-to-1 ratio, alkali metal to other element? a. | alkaline earth
elements | c. | halogens | b. | oxygen family | d. | noble gases | | | | |
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19.
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Some
elements are unlikely to lose or gain electrons, but share electrons to form covalent bonds. Which of
the following elements is most likely to form covalent bonds? a. | silicon
(#14) | c. | chlorine
(#17) | b. | oxygen (#8) | d. | sulfur (#16) | | | | |
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20.
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What is the
group number for elements that have a stable number of electrons in their outer energy
level?
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21.
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How many
dots are shown in the electron dot diagram for calcium, element number 20? a. | one | c. | eight | b. | two | d. | twenty | | | | |
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22.
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Sulfur,
element 16, forms a negative ion. How many dots would you have to show in the electron dot diagram
for the sulfur ion? a. | two | c. | eight | b. | six | d. | sixteen | | | | |
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23.
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What is the
name given to the units that make up covalently bonded compounds? a. | molecules | c. | electrons | b. | ions | d. | energy levels | | | | |
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24.
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Which of the
following elements will likely form a negative ion in its ionic compounds? a. | Li,
lithium | c. | Mg,
magnesium | b. | Al, aluminum | d. | Cl, chlorine | | | | |
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25.
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Each
substance written to the right of the arrow in a chemical equation is a ____. a. | reactant | c. | precipitate | b. | product | d. | catalyst | | | | |
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26.
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According to
the law of conservation of mass, how does the mass of the products in a chemical reaction compare to
the mass of the reactants? a. | There is no relationship. | b. | The mass of products is
sometimes greater. | c. | The mass of reactants is greater. | d. | The masses are always
equal. | | |
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27.
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When the
following chemical reaction is balanced, what number is placed before
NH3?
N2 +
3H2 ® NH3
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28.
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Which
chemical equation is balanced? a. | Na + O2 ® Na2O | c. | 2Na + 2O2 ® 2Na2O | b. | 2Na2 +
O2 ® 2Na2O | d. | 4Na + O2 ® 2Na2O | | | | |
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Matching
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Match
each term with the correct description below. a. | electron | g. | polar molecule | b. | nucleus | h. | compound | c. | positive ion | i. | symbol | d. | negative ion | j. | formula | e. | ionic bond | k. | molecule | f. | covalent bond | l. | subscript | | | | |
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29.
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positively
charged center of atom
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30.
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a charged
atom that has gained one or more electrons
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31.
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positive ion
and negative ion joined together
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32.
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substance
that contains two or more elements
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33.
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particle in
which electrons are shared unequally
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34.
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combination
of symbols
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35.
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represents
number of atoms
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36.
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a charged
atom that has lost one or more electrons
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37.
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negative
particle in an atom
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38.
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atoms joined
together by sharing electrons
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Match
each item with the best description below. a. | physical change | h. | subscript | b. | conservation of mass | i. | endothermic | c. | chemical change | j. | inhibitor | d. | exothermic | k. | reactant | e. | product | l. | rate of reaction | f. | catalyst | m. | enzyme | g. | activation energy | | | | |
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39.
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frying an
egg
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40.
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number of
atoms in a chemical formula
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41.
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present
before chemical reaction
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42.
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reactant
mass equals product mass
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43.
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ice
melting
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44.
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reaction
that releases energy
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45.
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a measure of
how fast a reaction occurs
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46.
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minimum
energy to start reaction
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47.
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speeds up a
chemical reaction
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48.
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used to slow
the spoilage of food
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Completion
Complete each sentence or
statement.
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49.
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All
matter is made up of particles called ____________________.
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50.
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Elements on the left side of the periodic table are classified as
____________________.
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51.
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For
material to be classified as a pure ____________________, every bit of it must have the same
properties.
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52.
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Elements that have properties halfway between those of metals and nonmetals, are
classified as ____________________.
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53.
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Chlorine-35 and chlorine-37 have a different number of
____________________.
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54.
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The change
in state from a gas to a liquid is called ____________________.
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55.
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The
temperature at which ice changes into liquid water is called its ____________________.
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56.
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Vaporization
is when a ____________________ changes into a ____________________.
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Short Answer
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57.
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Scientists used to think electrons moved in orbits around the nucleus. How do
scientists currently describe the movement of electrons?
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58.
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Discuss the likelihood that the current model of the atom will be the final model of
the atom.
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59.
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Draw
models of lithium-6 and lithium-7, two isotopes of lithium. Locate and label the subatomic particles
in each model. How do the two models differ?
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60.
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After an
especially heavy snowstorm, people often shovel the snow off of roofs that are flat. Why don’t
the people just wait for the snow to melt?
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61.
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On a graph
of temperature versus time, the temperature stops rising during melting. Why?
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62.
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Rubbing
alcohol has a slightly lower boiling point than does water. In which liquid are the cohesive forces
greater? Explain your answer.
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63.
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Explain why
a crystalline solid such as a diamond is one of the hardest substances in the world, but it takes
very little force to shatter a pane of ordinary window glass.
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64.
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How
do you determine the density of an object?
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65.
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How
does physical weathering change rocks?
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66.
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How does the
number of electrons in outer energy levels relate to the position of an element in the periodic
table?
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67.
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What is an
ionic bond?
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68.
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Sulfur has
16 electrons in its atoms. Over how many energy levels are the electrons distributed, and how many
are in each energy level?
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Figure 6-1
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69.
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What will
the Figure 6-1A atom do to become more stable?
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70.
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Why is it
wrong to change subscripts when balancing chemical equations?
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71.
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Distinguish
a reactant from a product.
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True/False
Indicate whether the sentence or statement is true
or false.
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72.
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Atoms of
different elements have different numbers of protons.
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73.
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The energy
of an electron varies depending upon which energy level that electron occupies.
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74.
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In an atom,
an electron that is close to the nucleus is on the highest energy level.
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75.
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To become
more stable, an atom that has two electrons in its outer energy level will gain two
electrons.
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76.
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A polar
molecule is one that exists only at low temperatures.
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77.
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According to
the law of conservation of mass, three atoms of calcium can react to produce six atoms of
calcium.
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78.
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Energy is
needed to break bonds in chemical reactions.
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79.
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A chemical
reaction in which more energy is absorbed than is released is endothermic.
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80.
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When a
chemical equation contains the same number of atoms on both sides, the equation is
balanced.
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