Midterm exam review with Answers

Physical Science
GOOD LUCK :)
Semester 1 Midterm Exam REVIEW!
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 1.
object.
a.
b.
Temperature is a measure of the average _____ energy of the particles in the
____
a.
b.
2.
____
a.
b.
3.
____
a.
b.
4.
____
a.
b.
5.
____
a.
b.
6.
thermal
kinetic
c.
d.
potential
chemical
The process of a liquid becoming a gas is called
sublimation.
condensation.
c.
d.
evaporation.
freezing.
The process of a liquid becoming a solid is called
condensation.
freezing.
c.
d.
evaporation.
melting.
The only state of matter that is not a fluid is
water.
gas.
c.
d.
liquid.
solid.
Which state of matter has a definite volume, but not shape?
plasma
c.
gas
d.
liquid
solid
The heavier a particle, the _____ it moves.
slower
faster
less
more
c.
d.
____ 7.
Archimedes’ principle states that the buoyant force on a(n) _____ is equal to the
weight of the displaced volume of fluid.
a.
object in the fluid
c.
b.
____
a.
b.
object floating on the fluid
8.
When ice melts to form water, energy
is created.
is destroyed.
d.
c.
d.
fluid mixing with another
liquid
substance dissolving into the
fluid
is released.
is absorbed.
____ 9.
pressure
a.
b.
Pascal’s principle states that a fluid in equilibrium enclosed by a vessel exerts
upwards.
towards the vessel’s opening.
c.
d.
equally in all directions.
downwards.
____
a.
b.
10.
The resistance of a fluid to flow is referred to as
pressure.
energy.
c.
d.
viscosity.
shape.
____
a.
b.
11.
____
a.
b.
12.
____
a.
b.
13.
____
a.
b.
14.
____
a.
b.
15.
____
a.
b.
16.
Which state of matter will hold its shape without a container?
solid
c.
liquid
d.
gas
plasma
The change of a substance from a solid directly to a gas is called
condensation.
c.
evaporation.
d.
melting.
sublimation.
The ability to change or to move matter is referred to as
kinetic theory.
c.
energy.
d.
evaporation.
heating.
Evaporation refers to the change of state from a
liquid to a gas.
gas to a liquid.
solid to a liquid.
liquid to a solid.
c.
d.
The law of conservation of mass states that mass cannot be
burned.
c.
changed in form.
d.
created or destroyed.
heated or cooled.
Ice floats in water because it is
more dense than water.
less dense than water.
colder than water.
warmer than water.
c.
d.
____
a.
b.
17.
____
a.
b.
18.
____
a.
b.
19.
____ 20.
liquid.
a.
b.
Boyle’s law relates the pressure of a gas to its
container.
volume.
c.
d.
molecular composition.
temperature.
Charles’s law relates the volume of a gas to its
container.
pressure.
c.
d.
molecular composition.
temperature.
Gay-Lussac’s law relates the temperature of a gas to its
container.
c.
volume.
d.
molecular composition.
pressure.
Buoyant force is the _____ force exerted on an object immersed or floating on a
lateral
upward
c.
d.
downward
tensile
.
____
a.
b.
21.
____
a.
b.
22.
____
a.
b.
23.
____
a.
b.
24.
Matter is defined as anything that
can be seen and touched.
has mass and takes up space.
c.
d.
The science of what matter is made of and how it changes is called
chemistry.
c.
physics.
d.
kinetics.
engineering.
A substance that cannot be broken down into simpler substances is
a compound.
c.
a mixture.
d.
an element.
an atom.
The smallest unit of a substance that behaves like the substance is
an element.
c.
an atom.
d.
a molecule.
a compound.
____ 25.
The chemical symbol for sulfuric acid is H2SO4. How many atoms are contained
in each molecule of sulfuric acid?
a.
3
c.
b.
5
d.
____
26.
can be weighed.
contains kinetic or potential
energy.
6
7
The chemical formula for water, H2O, means that each water molecule contains
a.
b.
c.
d.
two hydrogen atoms and two oxygen atoms.
two hydrogen atoms and one oxygen atom.
two hydrogen atoms and zero oxygen atoms.
one hydrogen atom and two oxygen atoms.
____
a.
b.
27.
____
a.
28.
b.
Which of the following is an example of a gas-liquid mixture?
the air we breathe
c.
a carbonated drink
d.
Knowing the chemical properties of a substance will tell you how the substance
looks.
c.
smells.
____
a.
b.
29.
____
a.
b.
30.
____
a.
b.
31.
A physical property of gold is its
density.
reactivity with powerful acids.
a helium balloon
ice cubes
d.
can be broken down into
atoms.
reacts with other substances.
c.
d.
non-flammability.
None of the above
Which of the following is not an example of a physical property?
freezing point
c.
boiling point
d.
reactivity
density
Which of the following is an example of a physical change?
dissolving salt in water
c.
burning wood into charcoal
d.
cooking an egg
rusting iron
____
a.
b.
32.
____
a.
b.
33.
____
a.
b.
34.
____
a.
b.
35.
____
a.
b.
36.
Grinding quartz crystals down to produce sand is an example of a
change of state.
c.
chemical change.
d.
chemical reaction.
physical change.
Digesting food is an example of
physical change.
change of state.
chemical change.
buoyancy.
c.
d.
Which of the following is an example of chemical change?
strumming a guitar
c.
converting matter into energy
d.
grilling a burger
melting of copper
Which of the following is an example of a chemical change?
ice melting
c.
paint fading
d.
pounding gold into a coin
a puddle of water evaporating
Which of the following is not a potential sign of chemical change?
release of gas
c.
evaporation of water
d.
change of color
production of gas
.
____
a.
b.
37.
____
a.
b.
38.
____
39.
a.
b.
The forces that hold different atoms or ions together are
electric currents.
c.
chemical bonds.
d.
physical bonds.
nuclear forces.
Each molecule of hydrochloric acid, HCl, contains one atom of hydrogen and
one atom of chlorine.
c.
one atom of oxygen.
d.
two atoms of chlorine.
two atoms of oxygen.
Each molecule of table sugar, C12H22O11, contains
0 atoms of carbon.
1 atom of carbon.
c.
d.
6 atoms of carbon.
12 atoms of carbon.
____
a.
b.
c.
d.
40.
An ionic bond is a bond that forms between
____
a.
b.
41.
____
a.
b.
42.
____
a.
b.
c.
d.
43.
The name dinitrogen tetroxide tells you that this compound contains
two nitrogen atoms and two oxygen atoms.
four nitrogen atoms and two oxygen atoms.
two nitrogen atoms and four oxygen atoms.
four nitrogen atoms and four oxygen atoms.
____
a.
b.
44.
A carbon atom can bond to four other atoms because it has
four different cations.
c.
four valence electrons.
d.
____
45.
ions with opposite charges.
atoms with neutral charges.
one atom’s nucleus and another atom’s electrons.
the electrons of two different atoms.
Covalent bonds are formed between
ions.
metal atoms.
c.
d.
nonmetal atoms.
compounds.
In which type of bond do atoms share electrons?
covalent bonds
metallic bonds
c.
d.
ionic bonds
polyatomic bonds
An atom that acquires an electrical charge by gaining or losing electrons is
two inner energy levels.
no protons in its nucleus.
known as:
a.
b.
c.
d.
____
an ion.
a free radical.
a hydrate.
a monatomic molecule.
46.
The diagram that best represents the Lewis dot diagram of a chlorine atom is:
a.
A
b.
B
c.
C
d.
D
The Mg atom becomes the ion, Mg2+, when it:
____
a.
b.
c.
d.
47.
____
a.
b.
c.
d.
48.
____
a.
b.
c.
d.
49.
How many valence electrons are in an atom of aluminum, atomic number 13?
1
2
3
4
____
a.
b.
50.
Which of the following is NOT a binary compound?
gains two electrons.
loses two electrons.
gains two protons.
loses two protons.
Ionic bonds form:
between oppositely charged atoms.
molecules.
by sharing electrons.
only between pairs of atoms.
NaCl
H2O
c.
Fe2O3
LiOH
d.
____ 51.
What is the chemical formula for a compound that contains the aluminum ion
(Al3+) and the hydroxide ion (OH-)?
a.
Al(OH)3
AlO3H3
b.
c.
AlOH3
None of the above
d.
____
a.
b.
52.
Which of the following contains a polyatomic ion?
NaCl
H2O
c.
Fe2O3
LiOH
d.
____
a.
b.
c.
d.
53.
____
a.
b.
54.
____
a.
b.
c.
d.
55.
____
a.
56.
b.
All organic compounds contain the element:
nitrogen.
carbon.
hydrogen.
oxygen.
The charge of an electron is
−2.
−1.
c.
d.
0.
+1.
Atoms have no electric charge because they
have an equal number of charged and noncharged particles.
have neutrons in their nuclei.
have an equal number of electrons and protons.
have an equal number of neutrons and protons.
The order of elements in the periodic table is based on
the number of protons in the
c.
nucleus.
the electric charge of the
d.
nucleus.
the number of neutrons in the
nucleus.
atomic mass.
a.
the number of protons in the
nucleus.
the electric charge of the
nucleus.
b.
____
a.
b.
57.
____
a.
b.
58.
____
a.
59.
b.
c.
d.
the number of neutrons in the
nucleus.
atomic mass.
Atoms of elements that are in the same group have the same number of
protons.
c.
neutrons.
d.
valence electrons.
protons and neutrons.
Oxygen’s atomic number is 8. This means that an oxygen atom has
eight neutrons in its nucleus.
c.
a total of eight protons and
d.
neutrons.
eight protons in its nucleus.
a total of eight neutrons and
electrons.
An atom’s mass number equals the number of
protons plus the number of
electrons.
protons plus the number of
neutrons.
c.
protons.
d.
neutrons.
____
a.
b.
c.
d.
60.
Which statement about the alkali metals is correct?
____
a.
b.
61.
____
a.
b.
c.
d.
62.
____
a.
b.
c.
d.
63.
Carbon and other nonmetals are found in which area of the periodic table?
on the left-most side
on the right side
in the middle column of the periodic table
in the bottom rows
____
a.
b.
64.
A mole is an SI base unit that describes the
mass of a substance.
amount of a substance.
____
a.
b.
c.
d.
65.
They are located in the left-most column of the periodic table.
They are extremely nonreactive.
They are usually gases.
They form negative ions with a 1- charge.
Which of the following elements is an alkali metal?
calcium
c.
magnesium
d.
mercury
sodium
Group 18 noble gases are inert because
they readily form positive ions.
they can have either a positive or a negative charge.
their outermost energy level is missing one electron.
their outermost energy level is full.
c.
d.
A particle with zero charge found in the nucleus of an atom is called a(n):
electron.
proton.
neutron.
positron.
____ 66.
Atoms of the same element whose nucleus contains different numbers of
neutrons are called:
a.
isotopes.
b.
nucleotides.
c.
ions.
d.
isobars.
____
are:
a.
b.
c.
d.
67.
____
a.
b.
c.
d.
68.
____
a.
b.
c.
d.
69.
Atoms with a net charge due to having different number of protons and electrons
isotopes.
nucleotides.
ions.
isobars
The number of protons in an atom is the:
atomic weight.
mass number.
atomic number.
atomic mass.
Which of the following is the charge on a proton?
+1
+2
-1
Zero
volume of a substance.
electric charge of a substance.
____
a.
b.
c.
d.
70.
Protons and neutrons are found grouped together in the:
electron cloud.
charge.
nucleus.
periodic table.
____
71.
Do any of the atom diagrams below represent atoms of the same element?
a.
b.
c.
d.
No, they are all different elements.
Yes, atom A and atom B are the same element.
Yes, all of the atoms are the same element.
Yes, atom A and atom C are the same element.
____
a.
b.
c.
d.
72.
The vertical columns of the periodic table are:
____
a.
b.
c.
d.
73.
A way of organizing the elements based on their chemical properties is the:
energy level.
periodic table.
nucleus.
isotope.
____
a.
b.
c.
d.
74.
Most of the elements in the periodic table can be described as:
metals.
nonmetals.
metalloids.
halogens.
____
a.
b.
c.
d.
75.
Horizontal rows on the periodic table are called:
____
a.
b.
c.
d.
76.
Where are the transition elements located on the periodic table?
groups 1-2
groups 3-12
groups 10-15
groups 13-18
____
a.
b.
c.
d.
77.
Which of the following is a characteristic of metals?
____
a.
b.
c.
d.
78.
Which of the following is a characteristic of non-metals?
Ductile
Shiny
Good conductor
Brittle
____
a.
b.
c.
d.
79.
Most non-metals on the periodic table are located on the:
left side.
bottom.
right side.
top.
periods.
groups.
halogens.
isotopes.
periods.
groups.
columns.
boxes.
Dull
Poor conductor
Ductile
Brittle
____ 80.
Which of the following is an example of a metalloid, an element with properties
between metals and non-metals?
a.
Iron
b.
Silicon
c.
Oxygen
d.
Copper
____ 81.
The elements that do not naturally form compounds with other atoms belong to
the group known as:
a.
alkali metals.
b.
halogens.
c.
noble gases.
d.
transition metals.
a.
b.
c.
d.
alkali metals.
halogens.
noble gases.
transition metals.
____
a.
b.
c.
d.
82.
Two elements are normally gases at room temperature. They are:
mercury and bromine.
hydrogen and oxygen.
water and alcohol.
boron and magnesium.
____
a.
b.
83.
All of the elements on the periodic table want to be as cool as...
alkali metals
c.
transition metals
d.
halogens
noble gases
____
a.
b.
84.
The sample contained the same number of pennies for which two years?
1988 and 1992
c.
1988 and 1991
d.
1994 and 1997
1994 and 1998
____
a.
b.
85.
For which year was the smallest number of pennies found?
1988
c.
1989
d.
1990
1991
____
a.
b.
86.
The two main branches of science are
physics and chemistry.
natural and social science.
natural and physical science.
biological and earth science.
____
a.
b.
87.
____
a.
b.
88.
____
a.
b.
89.
____
a.
b.
c.
d.
90.
____
a.
91.
c.
d.
Which of the following is not a branch of biology?
geology
c.
ecology
d.
zoology
medicine
The main branches of natural science are
physics and chemistry.
biology, zoology, and ecology.
c.
d.
medicine and agriculture.
life, physical, and earth
science.
Technology can best be defined as
science that uses computers.
new inventions.
c.
d.
applied science.
the use of lenses and
microscopes.
Pure science is best defined as the
continuing search for new knowledge.
use of science to solve human problems.
study of the makeup of living things.
application of scientific knowledge.
b.
For a scientific theory to be valid, it must allow you to
perform experiments.
c.
obtain new results each time.
____
a.
b.
c.
d.
92.
____
a.
b.
93.
____
a.
b.
94.
____
a.
b.
95.
____
a.
b.
96.
____
a.
b.
97.
d.
find a new, more complex
explanation.
make predictions.
Scientific theories can be changed or replaced when
new technology is invented.
new discoveries are made.
scientists decide to work on different problems.
scientists make models of events or objects.
A series of logical steps that is followed in order to solve a problem is called the
experimental process.
c.
scientific theory.
d.
scientific method.
model method.
The first step in the scientific method is usually
making an observation.
forming a hypothesis.
c.
d.
collecting data.
testing a hypothesis.
Scientists test a hypothesis by
formulating questions.
designing models.
c.
d.
doing experiments.
drawing conclusions.
The SI unit for measuring temperature is the
degree.
kelvin.
c.
d.
mole.
ampere.
Which SI prefix means one million?
kilomega-
c.
d.
gigamilli-
a.
b.
kilomega-
____
a.
b.
98.
____
a.
b.
99.
____
a.
b.
c.
d.
100.
____
a.
101.
gigamilli-
Which SI prefix means one one-hundredth ()?
nanomicro-
c.
d.
millicenti-
The decimal equivalent of 10−2 is
100.
10.
c.
d.
0.1.
0.01.
A precise measurement is one that
contains the correct number of significant figures.
contains at least three significant figures.
is close to the true value.
is as exact as possible.
b.
____
a.
c.
d.
A measurement that is accurate is one that
is as exact as possible.
is close to the true value.
102.
b.
____
a.
b.
103.
____
a.
b.
104.
____
a.
105.
b.
A change in the color of a solution is a sign that
a chemical change is taking
place.
a physical change has just
occurred.
c.
d.
contains at least four
significant figures.
contains five decimal places.
c.
oxygen is present.
d.
organic chemicals are present.
A substance that undergoes a change in a chemical reaction is
a product.
c.
a chemical.
d.
a reactant.
an enzyme.
What happens in a chemical reaction?
Atoms are destroyed.
Atoms are created.
Molecules are created.
Atoms are rearranged.
c.
d.
In an exothermic reaction, energy is transferred from
the reactants to the
c.
surroundings.
the surroundings to the
d.
reactants.
one reactant to another.
the container to the chemicals.
____
a.
b.
c.
d.
106.
Which statement about endothermic reactions is correct?
Energy is always created in the form of heat.
Energy is transferred from the surroundings to the reactants.
Energy is used to force electrons to move to higher energy levels.
Energy is transferred from the reactants to the surroundings.
____
a.
107.
Chemical energy is energy that is
added to a reaction in the form
of heat.
present within atoms and
molecules.
b.
The energy source in photosynthesis is
light energy.
chemical energy.
c.
d.
caused by the movement of
electricity.
released only when oxygen is
present.
____
a.
b.
108.
____
a.
b.
109.
____
a.
b.
c.
d.
110.
A synthesis reaction is a reaction between at least two compounds in which
one breaks down into at least two products.
a compound is decomposed by an electric current.
a compound burns in the presence of oxygen.
a new, more complex compound is formed.
____
a.
b.
111.
What kind of reaction occurs when potassium is placed in water?
a single-displacement reaction c.
a double-displacement reaction d.
____
a.
b.
c.
d.
112.
c.
d.
Most of the energy in an isooctane reaction is released in the form of
heat and light.
c.
electrical energy.
d.
heat energy.
kinetic energy.
water.
sound.
a decomposition reaction
electrolysis
Which of the following is an example of a decomposition reaction?
photosynthesis
digestion
polymerization
exchange of ions between two compounds
a.
b.
c.
d.
photosynthesis
digestion
polymerization
exchange of ions between two compounds
____
a.
b.
113.
____
a.
b.
114.
____
a.
b.
115.
The product of the synthesis reaction between sodium and chlorine gas is
polyethylene.
c.
carbon dioxide.
d.
sodium chloride.
copper (II) chloride.
When methane reacts with abundant amounts of oxygen, the products are
carbon dioxide and water.
c.
carbon monoxide and water.
d.
soot and water.
simple sugar and oxygen.
When water is broken down by electrolysis, the products are
water and carbon dioxide.
c.
hydrogen and oxygen ions.
d.
hydrogen gas and oxygen gas.
oxygen and methane.
____ 116.
called
a.
b.
Fragments of molecules that have at least one electron available for bonding are
____
a.
b.
117.
In a redox reaction, the substance that accepts electrons is said to be
reduced.
c.
oxidized.
d.
electrified.
clarified.
____
a.
b.
118.
When iron reacts with oxygen to form rust, each iron atom
loses three ions.
c.
loses three electrons.
d.
gains three ions.
gains three electrons.
____
a.
b.
119.
A chemical equation is balanced by changing or adding
chemical symbols.
c.
subscripts.
d.
coefficients.
reactants.
____ 120.
necessary for
a.
b.
ions.
orbits.
c.
d.
protons.
radicals.
A balanced chemical equation shows the proportions of reactants and products
the reaction to occur.
mass to be conserved.
c.
d.
____ 121.
In the reaction 2H2O → 2H2 + O2, if you start with 2 mol of water, how many
moles of hydrogen gas are produced?
a.
1 mol
c.
b.
2 mol
d.
energy use to be minimized.
electrolysis to occur.
3 mol
4 mol
____ 122.
In the reaction 2H2O2 → 2H2O + O2, if you start with 4 mol of H2O2, how
many moles of O2 will you end up with?
a.
b.
4 mol
3 mol
c.
d.
____ 123.
If you start with 5 mol of O2 in the reaction 2Mg + O2 → 2MgO, how many
moles of Mg will you need?
a.
4 mol
c.
b.
5 mol
d.
2 mol
1 mol
8 mol
10 mol
____ 124.
In the reaction H2S + 2O2 → H2SO4, the law of definite proportions predicts
that for every mole of H2S you will need how many moles of O2?
a.
b.
1 mol
2 mol
c.
d.
3 mol
4 mol
____ 125.
In the reaction 2Mg + O2 → 2MgO, the law of definite proportions states that for
every 2 moles of Mg you will need how many moles of O2?
a.
b.
____
a.
b.
1 mol
2 mol
126.
c.
d.
In a balanced chemical reaction, the total mass of the products always equals the
molar mass of the reactants.
c.
atomic mass of the reactants.
d.
3 mol
4 mol
total mass of the reactants.
proportional masses of the
reactants.
____ 127.
A balanced chemical equation indicates both the number of particles of reactants
and products and the number of
a.
orbits.
c.
b.
electrons.
d.
nuclei.
moles.
____
a.
b.
higher temperature.
presence of a catalyst.
128.
All of the following factors may speed up a chemical reaction except
smaller surface area.
c.
higher pressure.
d.
____
a.
b.
129.
____
a.
b.
c.
d.
130.
What could you do to make yeast dough rise more slowly?
Add more yeast to the mixture. c.
Knead the dough more
d.
vigorously.
Add mold spores to the dough.
Reduce the temperature.
An enzyme is a special kind of catalyst that works to
speed up a specific biochemical reaction.
break down chemical elements.
slow down a chemical reaction.
maintain the correct temperature for a reaction.
____ 131.
When a chemical reaction and its reverse are occurring at the same time and at
the same rate, the reaction has achieved
a.
displacement.
c.
b.
equilibrium.
d.
imbalance.
decomposition.
____ 132.
What is the relationship between chemical equilibrium and the rates of forward
and reverse reaction?
a.
In equilibrium, the forward reaction rate must be greater than the
reverse reaction rate.
b.
In equilibrium, the forward reaction rate must be less than the
reverse reaction rate.
c.
In equilibrium, the forward and reverse reaction rates must be
equal.
d.
In equilibrium, both forward and reverse reactions must stop.
____
a.
b.
133.
Le Châtelier’s principle states that increasing temperature favors a reaction that
releases energy as heat.
c.
requires energy as heat.
d.
____ 134.
Increasing the concentration of one substance in an equilibrium reaction favors
the reaction that
a.
absorbs energy as heat.
c.
b.
releases energy as heat.
d.
involves a chemical catalyst.
involves an enzyme.
produces less of that substance.
produces more of that
substance.
____
a.
b.
c.
d.
135.
Which of the following is evidence that a chemical change has occurred?
A material changes from liquid to solid.
The temperature of a material changes from 10°C to 20°C.
A material is hammered from a round shape to a flat shape.
A material changes color from blue to red.
____
136.
How many atoms of reactant are represented in the equation below?
2KClO3 → 2KCl + 3O2
2
5
6
10
a.
b.
c.
d.
____ 137.
When you activate an instant cold pack, water mixes with a chemical and the
pack gets very cold. This is an example of:
a.
an endothermic reaction.
b.
an exothermic reaction.
c.
a combustion reaction.
d.
a physical change.
____
138.
Classify the following reaction:
3CuSO4 + 2Al Al2(SO4)3 + 3Cu
a.
b.
c.
d.
____
Synthesis
Single-displacement
Double-displacement
Decomposition
139.
Classify the following reaction:
Cu(NO3)2 + 2NaOH Cu(OH)2 + 2NaNO3
a.
b.
c.
d.
____
a.
b.
c.
d.
Synthesis
Single-displacement
Double-displacement
Decomposition
140.
Classify the following reaction:
Cu(OH)2 CuO + H2O
Synthesis
Single-displacement
Double-displacement
Decomposition
a.
b.
c.
d.
Synthesis
Single-displacement
Double-displacement
Decomposition
____
a.
b.
c.
d.
141.
Which of the following is an example of an exothermic reaction?
Refining aluminum ore
Activating an instant cold pack
Burning of gasoline in an automobile engine
Changing water to steam
____
a.
b.
c.
d.
142.
Which of the following is an example of an exothermic reaction?
Refining aluminum ore
Activating an instant cold pack
Burning of gasoline in an automobile engine
Changing water to steam
Completion
Complete each statement.
143.
Charles’s law relates the volume of a gas to the ____________________ of a gas.
144.
of a gas.
Gay-Lussac’s law relates the temperature of a gas to the ____________________
145.
Boyle’s law relates the pressure of a gas to the ____________________ of a gas.
146.
The buoyant force exerts a(n) ____________________ force on any object
immersed in or floating on a fluid.
147.
of the object.
When an object floats, the buoyant force is ____________________ the weight
148.
The most common state of matter in the universe is called
____________________.
149.
The law of mass conservation states that mass
___________________________________________________.
150.
For any change of state to occur, ____________________ must be transferred.
151.
Energy may be converted from one form to another, but it cannot be
________________________________________.
152.
A liquid has a definite volume, but no definite ____________________.
153.
Matter that always has exactly the same composition is classified as a(an)
________________________________________.
.
154.
An element has a fixed composition because it contains only one type of
____________________________.
.
155.
The substances in a(an) ___________________________ mixture are evenly
distributed throughout the mixture.
.
156.
In a(an) ___________________________ mixture, the parts of the mixture are
noticeably different from one another.
.
157.
A(An) __________________________ change occurs when a material changes
shape or size but the composition of the material does not change.
.
158.
_________________________ properties can be observed only when the
substances in a sample of matter are changing into different substances.
.
159.
A solid that forms and separates from a liquid mixture is a(an)
_________________________.
.
.
160.
Aluminum, oxygen, and carbon are examples of ________________________.
161.
A substance that is made of atoms of more than one type bound together is called
a __________________________.
.
162.
The _________________________ of a substance is defined as its mass divided
by its volume.
.
163.
When elements combine to form a(n) __________________________________,
the resulting properties may be very different from those of the elements that make it.
164.
The melting and boiling points of quartz are very high because of the
compound’s __________________________________________________.
165.
Atoms bond in compounds when their
__________________________________________ interact.
166.
When atoms form bonds and fill their outermost energy levels, they have an
electronic arrangement similar to that of a(n)
_____________________________________________.
167.
electrons.
A ______________________________ bond is formed when atoms share
168.
subunits.
_________________________________ are compounds that have repeating
169.
electrons.
A(n) _____________________________ bond is formed when atoms transfer
.
170.
Chemistry and physics are the two branches of ____________________ science.
171.
Life science, physical science, and earth science make up
____________________ science.
.
.
172.
Pure science is the continuing search for scientific ____________________.
173.
The application of science for practical purposes is referred to as
____________________.
.
174.
A ____________________ description of a scientific law would use a
mathematical equation.
.
.
175.
A possible answer to a scientific problem is called a ____________________.
176.
To view objects that are very small, a scientist would use a
_________________________________.
.
177.
Length, mass, time, and temperature, are four of the seven SI
_______________________.
.
178.
In the SI system, the prefix ____________________ means one billion.
.
179.
When bread rises, this is a sign that a chemical reaction is producing
____________________.
180.
A change of color is a sign that a ____________________ is taking place.
181.
The changes that are visible during a chemical reaction are signs that the
____________________ in the reactants have been rearranged.
182.
In a chemical reaction, atoms are ____________________, but they are not
created or destroyed.
183.
A chemical reaction that transfers energy from the reactants to the surroundings
is referred to as ____________________.
184.
A(n) ____________________ reaction is one in which heat is transferred from
the surroundings to the reactants.
185.
____________________ is an exothermic reaction in which living things
produce light.
186.
The general formula for a synthesis reaction is ____________________.
187.
In a(n) ____________________ reaction, the reactants are broken down into
other substances.
188.
Aluminum undergoes a single-displacement reaction with copper (II) sulfate to
form aluminum sulfate and ____________________.
189.
Balance the following chemical equation by filling in the correct coefficient on
the right-hand side. H2 + Cl2 → ____________________ HCl
190.
Balance the following chemical equation by filling in the correct coefficients.
____________________ KI + Br2 → ____________________ KBr + I2
191.
The law of definite proportions states that a compound always contains the same
____________________ in the same ____________________.
Short Answer
192.
Use the diagram of the periodic table below to answer the following questions:
The Periodic Table of the Elements
1
18
1
2
H
He
1
Hydrogen
1.0
9
10
Li
Be
B
C
N
O
F
Ne
2
Lithium
6.9
Beryllium
9.0
Boron
10.8
Carbon
12.0
Nitrogen
14.0
Oxygen
16.0
Fluorine
19.0
Neon
20.2
3
2
13
4
14
5
6
12
11
Na
3
Sodium
23.0
3
4
5
6
7
8
9
10
11
12
13
14
Al
Si
Aluminum
27.0
Silicon
28.1
25
4
7
16
8
17
Helium
4.0
15
Mg
Magnesiu
m
24.3
15
20
21
22
23
24
Ca
Sc
Ti
V
Cr
Potassium
39.1
Calcium
40.1
Scandium
45.0
Titanium
47.9
Vanadium
50.9
Chromium
52.0
17
18
S
Cl
Ar
Sulfur
32.1
16
Chlorine
35.5
Argon
39.9
32
Mn
19
K
P
Phosphoru
s
31.0
Manganes
e
54.9
26
27
28
29
30
31
Fe
Co
Ni
Cu
Zn
Ga
Iron
55.8
Cobalt
58.9
Nickel
58.7
Copper
63.5
Zinc
65.4
Gallium
69.7
Ge
Germaniu
m
72.6
33
34
35
36
As
Se
Br
Kr
Arsenic
74.9
Selenium
79.0
Bromine
79.9
Krypton
83.8
43
5
37
38
39
40
41
42
Rb
Sr
Y
Zr
Nb
Mo
Rubidium
85.5
Strontium
87.6
Yttrium
88.9
Zirconium
91.2
Niobium
92.9
Molybdenum
95.9
Tc
44
Technetiu
m
(97.9)
46
47
49
50
53
54
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Ruthenium
101.1
Rhodium
102.9
45
Palladium
106.4
Silver
107.9
Cadmium
112.4
48
Indium
114.8
Tin
118.7
Antimony
121.8
51
Tellurium
127.6
52
Iodine
126.9
Xenon
131.3
57
6
7
55
56
Cs
Ba
Cesium
132.9
La
78
79
80
81
82
85
86
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Barium
137.3
Lanthanu
m
138.9
Hafnium
178.5
72
Tantalum
180.9
73
Tungsten
183.8
Rhenium
186.2
Osmium
190.2
Iridium
192.2
Platinum
195.1
110
Gold
197.0
111
Mercury
200.6
Thallium
204.4
Lead
207.2
Bismuth
209.0
Polonium
(209.0)
Astatine
(210.0)
Radon
(222.0)
118
87
88
89
104
105
106
107
108
109
Uu
Uu
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Francium
(223.0)
Radium
(226.0)
Actinium
(227.0)
Rutherfordium
(261.1)
Dubnium
(262.1)
Seaborgium
(263.1)
Bohrium
(262.1)
Hassium
(265)
Meitnerium
(266)
Ununniliu
m
(271)
Unununiu
m
(272)
58
76
77
114
116
Uu
Uu
b
q
Ununbium
(277)
Ununquadium
(285)
61
68
69
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Promethium
(144.9)
Samarium
150.4
Europium
152.0
Gadolinium
157.3
Terbium
158.9
Dysprosium
162.5
Holmium
164.9
Erbium
167.3
Thulium
168.9
Ytterbium
173.0
Lutetium
175.0
94
97
98
67
Ununhexium
(289)
60
93
66
o
Ununoctiu
m
(293)
Nd
92
65
Uu
h
Neodymium
144.2
Pa
64
112
Uu
Pr
Protactiniu
m
231.0
63
u
84
Praseodymium
140.9
91
90
62
n
83
Cerium
140.1
Th
59
75
Ce
Thorium
232.0
Figure 12-1
74
101
70
102
71
95
96
99
100
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Uranium
238.0
Neptunium
(237.0)
Plutonium
244.1
Americium
(243.1)
Curium
(247.1)
Berkelium
(247.1)
Californium
(251.1)
Einsteinium
(252.1)
Fermium
(257.1)
Mendelevium
(258.1)
Nobelium
(259.1)
Lawrencium
(262.1)
103
32. Which group number on the periodic table contain alkaline earth elements?
.____________________________________________________________________
193.
In which group are the halogens found?
_____________________________________________________________________
194.
In which group(s) are the transition elements found?
_____________________________________________________________________
195.
Identify three alkali metals.
_____________________________________________________________________
196.
In which group are the noble gases located?
_____________________________________________________________________
197.
List the SI Unit for the following:
a. length = ______________
b. mass = ______________
c. temperature = ________________
d. volume (liquid) = _____________
Problem
One of the largest helicopters in the world weighs 1.0 X 106 N. If you
were to place this helicopter on a large piston of a hydraulic lift, what force would need
2
to be applied to the small piston with an area of 0.7m , in order to lift the helicopter?
2
The area of the large piston is 140m .
198.
Use Pascal’s principle to solve. F = F
A A
cm3.
199.
Calculate the density of a sample of gas with a mass of 30 g and volume of 7500
.
200.
of 585 g.
Calculate the density of a sample of liquid with a volume of 130 ml and a mass
.
cm3.
201.
Calculate the mass of a solid with a density of 14.2 g/cm3 and volume of 350
202.
Calculate the volume of a liquid with a density of 1.7 g/ml and a mass of 144.5 g.
203.
Calculate the volume of a solid with a density of 5.3 g/cm3 and a mass of 371 g.
.
.
.
204.
A 5k (5 kilometer) running race has how many meters?
205.
What is the formula mass for Sodium Hydroxide? (NaOH)
206.
375 cm equals ____________________ m.
207.
5675 g equals ____________________ kg.
.
.
.
.
208.
The number 0.0034 would be written as ___________________________ in
scientific notation.
.
209.
In scientific notation, the number 46,500,000 would be written
____________________.
.
210.
The number 0.0009234 would be written in scientific notation as
_________________________________.
.
211.
The number 56,780,000,000 would be written in scientific notation as
___________________________.
.
212.
Balance the following chemical equation:
Al + O2 → Al2O3
.
213.
Balance the following equation:
K + H2O → KOH + H2
.
214.
Balance the following chemical equation:
HgO → Hg + O2
.
Other
215.
Draw a Lewis dot diagram to represent an atom of silicon. (make your marks for
the electrons dark enough for me to easily see)
.
216.
Write the chemical formula for an ionic bond of Sodium and Oxygen.
217.
Write the chemical formula for a compound containing Aluminum and Oxygen.
.
.
218.
and Nitrogen.
Write the chemical formula for a compound containing the element of Calcium
.
219.
Name the following ionic compound: BeO.
220.
Name the following ionic compound: AlBr2
221.
Name the following covalent compound: P4S5
.
.
.
Physical Science
GOOD LUCK :)
Answer Section
Semester 1 Midterm Exam REVIEW!
MULTIPLE CHOICE
1.
OBJ: 2
2.
OBJ: 4
3.
OBJ: 4
4.
OBJ: 3
5.
OBJ: 3
6.
OBJ: 1
7.
OBJ: 2
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
2
8.
OBJ: 5
9.
OBJ: 4
10.
OBJ: 5
11.
OBJ: 3
12.
OBJ: 4
13.
OBJ: 2
14.
OBJ: 4
15.
OBJ: 5
16.
OBJ: 3
17.
OBJ: 2
18.
OBJ: 3
19.
OBJ: 2
20.
OBJ: 1
21.
OBJ: 1
22.
OBJ: 1
23.
OBJ: 2
24.
OBJ: 3
25.
OBJ: 4
26.
OBJ: 4
27.
OBJ: 5
28.
OBJ: 1
29.
OBJ: 1
30.
OBJ: 1
31.
OBJ: 1
32.
OBJ: 1
33.
OBJ: 2
34.
OBJ: 2
35.
OBJ: 2
36.
OBJ: 4
37.
OBJ: 1
38.
OBJ: 2
39.
OBJ: 2
40.
OBJ: 2
41.
OBJ: 2
42.
OBJ: 3
43.
OBJ: 1
44.
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
3
ANS: D
PTS: 1
DIF: 1
REF:
3
ANS: D
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 2
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
3
ANS: D
PTS: 1
DIF: 1
REF:
3
ANS: C
PTS: 1
DIF: 1
REF:
3
ANS: C
PTS: 1
DIF: 2
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 2
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 2
REF:
3
ANS: B
PTS: 1
DIF: 2
REF:
4
OBJ: 1
45.
13.1
46.
section 13.1
47.
section 13.1
48.
section 13.1
49.
section 13.1
50.
section 13.2
51.
section 13.2
52.
section 13.2
53.
section 13.3
54.
OBJ: 2
55.
OBJ: 2
56.
OBJ: 1
57.
OBJ: 1
58.
OBJ: 3
59.
OBJ: 3
60.
OBJ: 1
61.
OBJ: 1
62.
OBJ: 3
63.
OBJ: 3
64.
OBJ: 1
65.
12.1
66.
12.1
67.
12.1
68.
12.1
69.
12.1
70.
12.1
71.
section 12.1
72.
12.2
73.
12.2
74.
12.2
75.
12.3
76.
12.3
77.
12.3
78.
12.3
79.
12.3
80.
section 12.3
ANS: A
PTS: 1
DIF: basic
REF:
section
ANS: D
PTS: 1
DIF: intermediate
REF:
ANS: B
PTS: 1
DIF: intermediate
REF:
ANS: A
PTS: 1
DIF: intermediate
REF:
ANS: C
PTS: 1
DIF: advanced
REF:
ANS: D
PTS: 1
DIF: intermediate
REF:
ANS: A
PTS: 1
DIF: intermediate
REF:
ANS: D
PTS: 1
DIF: intermediate
REF:
ANS: B
PTS: 1
DIF: intermediate
REF:
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 2
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
4
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: A
PTS: 1
DIF: basic
REF:
section
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: A
PTS: 1
DIF: basic
REF:
section
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: D
PTS: 1
DIF: intermediate
REF:
ANS: B
PTS: 1
DIF: basic
REF:
section
ANS: B
PTS: 1
DIF: basic
REF:
section
ANS: A
PTS: 1
DIF: basic
REF:
section
ANS: A
PTS: 1
DIF: basic
REF:
section
ANS: B
PTS: 1
DIF: basic
REF:
section
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: D
PTS: 1
DIF: basic
REF:
section
ANS: C
PTS: 1
DIF: basic
REF:
section
ANS: B
PTS: 1
DIF: intermediate
REF:
12.3
12.4
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
81.
ANS: C
PTS: 1
DIF: basic
REF:
section
82.
ANS: B
PTS: 1
DIF: basic
REF:
section
83.
84.
1
85.
1
86.
1
87.
1
88.
1
89.
2
90.
2
91.
3
92.
3
93.
1
94.
2
95.
2
96.
4
97.
5
98.
5
99.
2
100.
4
101.
4
102.
1
103.
2
104.
2
105.
3
106.
3
107.
4
108.
4
109.
4
110.
1
111.
1
112.
1
113.
2
114.
2
115.
2
116.
3
117.
3
ANS: D
ANS: C
PTS: 1
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 2
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: D
PTS: 1
DIF: 1
REF:
2
ANS: D
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
3
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: C
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: B
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: A
PTS: 1
DIF: 1
REF:
1
ANS: D
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
2
ANS: D
PTS: 1
DIF: 1
REF:
2
ANS: A
PTS: 1
DIF: 1
REF:
2
118.
OBJ: 3
119.
OBJ: 1
120.
OBJ: 1
121.
OBJ: 2
122.
OBJ: 2
123.
OBJ: 2
124.
OBJ: 3
125.
OBJ: 3
126.
OBJ: 5
127.
OBJ: 5
128.
OBJ: 1
129.
OBJ: 1
130.
OBJ: 2
131.
OBJ: 3
132.
OBJ: 3
133.
OBJ: 4
134.
OBJ: 4
135.
14.1
136.
section 14.1
137.
14.2
138.
section 14.2
139.
section 14.2
140.
section 14.2
141.
section 14.2
142.
section 14.2
ANS: B
PTS: 1
DIF: 1
REF:
2
ANS: C
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 1
REF:
3
ANS: B
PTS: 1
DIF: 2
REF:
3
ANS: C
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 2
REF:
3
ANS: B
PTS: 1
DIF: 2
REF:
3
ANS: A
PTS: 1
DIF: 2
REF:
3
ANS: C
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 2
REF:
3
ANS: A
PTS: 1
DIF: 2
REF:
3
ANS: D
PTS: 1
DIF: 2
REF:
4
ANS: A
PTS: 1
DIF: 2
REF:
4
ANS: B
PTS: 1
DIF: 1
REF:
4
ANS: C
PTS: 1
DIF: 1
REF:
4
ANS: B
PTS: 1
DIF: 1
REF:
4
ANS: C
PTS: 1
DIF: 1
REF:
4
ANS: D
PTS: 1
DIF: basic
REF:
section
ANS: D
PTS: 1
DIF: advanced
REF:
ANS: A
PTS: 1
DIF: basic
section
ANS: B
PTS: 1
DIF: intermediate
REF:
ANS: C
PTS: 1
DIF: intermediate
REF:
ANS: D
PTS: 1
DIF: intermediate
REF:
ANS: C
PTS: 1
DIF: intermediate
REF:
ANS: C
PTS: 1
DIF: intermediate
REF:
COMPLETION
143.
ANS: temperature
PTS: 1
144.
DIF: 1
ANS: pressure
REF: 3
OBJ: 2
PTS: 1
145.
DIF: 1
ANS: volume
REF: 3
OBJ: 2
PTS: 1
146.
DIF: 1
ANS: upward
REF: 3
OBJ: 2
PTS: 1
147.
DIF: 1
ANS: equal to
REF: 2
OBJ: 1
PTS: 1
148.
DIF: 1
ANS: plasma
REF: 2
OBJ: 1
PTS: 1
149.
DIF: 1
REF: 1
OBJ: 3
ANS: mass can be neither created nor destroyed
REF:
PTS: 1
150.
DIF: 1
ANS: energy
REF: 1
OBJ: 5
PTS: 1
151.
DIF: 1
REF: 1
ANS: created or destroyed
OBJ: 4
PTS: 1
152.
DIF: 1
ANS: shape
REF: 1
OBJ: 5
PTS: 1
153.
pure substance
substance
DIF: 1
ANS:
REF: 1
OBJ: 3
PTS: 1
154.
DIF: L1
ANS: atom
OBJ: 2.1.1
PTS: 1
155.
DIF: L1
OBJ: 2.1.2
ANS: homogeneous
PTS: 1
156.
DIF: L1
OBJ: 2.1.5
ANS: heterogeneous
PTS: 1
157.
DIF: L2
ANS: physical
OBJ: 2.1.5
PTS: 1
158.
DIF: L1
ANS: Chemical
OBJ: 2.2.5
PTS: 1
159.
DIF: L1
ANS: precipitate
OBJ: 2.3.1
PTS: 1
160.
DIF: L1
ANS: elements
OBJ: 2.3.2
PTS: 1
161.
DIF: 1
ANS: compound
REF: 1
OBJ: 2
PTS: 1
162.
DIF: 1
ANS: density
REF: 1
OBJ: 2
PTS: 1
163.
DIF: 1
ANS: compound
REF: 2
OBJ: 2
PTS: 1
164.
DIF: 1
REF: 1
ANS: network structure
OBJ: 1
PTS: 1
165.
DIF: 1
REF: 1
ANS: valence electrons
OBJ: 4
PTS: 1
166.
DIF: 1
ANS: noble gas
REF: 2
OBJ: 1
PTS: 1
167.
DIF: 1
ANS: covalent
REF: 2
OBJ: 1
PTS: 1
168.
DIF: 1
ANS: Polymers
REF: 2
OBJ: 4
PTS: 1
169.
DIF: 1
ANS: ionic
REF: 4
OBJ: 2
PTS: 1
170.
ANS: physical
PTS: 1
171.
DIF: 1
ANS: natural
REF: 1
OBJ: 1
PTS: 1
172.
DIF: 1
ANS: knowledge
REF: 1
OBJ: 1
PTS: 1
173.
DIF: 1
ANS: technology
REF: 1
OBJ: 2
STA: C.9-10.C
STA: C.9-10.C
PTS: 1
174.
DIF: 1
ANS: quantitative
REF: 1
OBJ: 2
PTS: 1
175.
DIF: 2
ANS: hypothesis
REF: 1
OBJ: 3
PTS: 1
176.
DIF: 1
REF: 2
ANS: light microscope
OBJ: 2
PTS: 1
177.
DIF: 1
ANS: base units
REF: 2
OBJ: 3
PTS: 1
178.
DIF: 1
ANS: giga-
REF: 2
OBJ: 4
PTS: 1
179.
DIF: 1
REF: 2
ANS: carbon dioxide gas
OBJ: 5
PTS: 1
180.
DIF: 1
REF: 1
ANS: chemical reaction
OBJ: 1
PTS: 1
181.
DIF: 1
ANS: atoms
REF: 1
OBJ: 1
PTS: 1
182.
DIF: 1
ANS: rearranged
REF: 1
OBJ: 2
PTS: 1
183.
DIF: 1
ANS: exotheremic
REF: 1
OBJ: 2
PTS: 1
184.
DIF: 1
ANS: endothermic
REF: 1
OBJ: 3
PTS: 1
185.
DIF: 1
REF: 1
ANS: Bioluminescence
OBJ: 3
PTS: 1
186.
DIF: 1
REF: 1
ANS: A + B → AB
OBJ: 4
PTS: 1
187.
DIF: 1
REF: 2
ANS: decomposition
OBJ: 1
PTS: 1
188.
DIF: 1
ANS: copper
REF: 2
OBJ: 1
PTS: 1
189.
DIF: 1
ANS: 2
REF: 2
OBJ: 2
PTS: 1
190.
DIF: 2
ANS: 2; 2
REF: 3
OBJ: 1
PTS: 1
191.
DIF: 2
REF: 3
ANS: elements; proportions
OBJ: 1
PTS: 1
DIF: 1
OBJ: 3
REF: 3
SHORT ANSWER
192.
groups 2
ANS:
PTS: 1
193.
group 17
DIF: intermediate
ANS:
REF: section 12.3
PTS: 1
194.
groups 3 - 12
DIF: intermediate
ANS:
REF: section 12.3
PTS: 1
DIF: intermediate REF: section 12.3
195.
ANS:
Answers may vary but must include three of the following:
lithium, sodium, potassium, rubidium, cesium, francium
PTS: 1
196.
group 18
DIF: intermediate
ANS:
REF: section 12.3
PTS: 1
197.
see question
DIF: intermediate
ANS:
REF: section 12.3
PTS: 1
PROBLEM
5000N
198.
PTS: 1
199.
0.004 g/cm3
ANS:
ANS:
PTS: 1
200.
4.5 g/ml
DIF: 2
ANS:
REF: 2
OBJ: 2
PTS: 1
201.
4990 g
DIF: 2
ANS:
REF: 2
OBJ: 2
PTS: 1
202.
85 ml
DIF: 2
ANS:
REF: 2
OBJ: 2
PTS: 1
203.
70 g/cm3
DIF: 2
ANS:
REF: 2
OBJ: 2
PTS: 1
204.
5000
DIF: 1
ANS:
REF: 2
OBJ: 2
PTS: 1
205.
40 g
ANS:
PTS: 1
206.
3.75
ANS:
PTS: 1
207.
5.675
DIF: 2
ANS:
REF: 2
OBJ: 5
PTS: 1
208.
3.4 X 10−3
DIF: 2
ANS:
REF: 2
OBJ: 5
PTS: 1
209.
4.65 × 107
DIF: 2
ANS:
REF: 3
OBJ: 2
PTS: 1
210.
9.234 × 10−4
DIF: 2
ANS:
REF: 3
OBJ: 2
PTS: 1
211.
5.678 × 1010
DIF: 2
ANS:
REF: 3
OBJ: 2
PTS: 1
212.
DIF: 2
ANS:
REF: 3
OBJ: 2
4Al + 3O2 → 2Al2O3
PTS: 1
DIF: intermediate
213.
ANS:
2K + 2H2O → 2KOH + H2
REF: section 14.1
PTS: 1
DIF: intermediate
214.
ANS:
2HgO → 2Hg + O2
REF: section 14.1
PTS: 1
REF: section 14.1
DIF: intermediate
OTHER
215.
PTS: 1
216.
Na2O
ANS:
DIF: intermediate
ANS:
PTS: 1
217.
Al2O3
ANS:
PTS: 1
218.
Ca3N2
ANS:
PTS: 1
219.
berellium oxide.
ANS:
PTS: 1
220.
ANS:
Aluminum Bromide
PTS: 1
221.
ANS:
tetraphosphorous pentasulfide
PTS: 1
REF: section 13.1