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WorksheetsSemester 1 Final Review (GEARUP)
Total questions: 105
Worksheet time: 2hrs 46mins
Name
Class
Date
1.
During an energy conversion, some energy is always transformed into ______________ energy.
a)
sound
b)
thermal
c)
nuclear
d)
chemical
2.
A skater starts at the top of the ramp. _____ of his energy is _________ potential energy.
a)
50%, gravitaional
b)
100%, chemical
c)
100%, gravitational
d)
50%, chemical
3.
A 100 kg car is traveling at 50 m/s. How much kinetic energy does the car have?
Formula: KE=1/2mv2
Formula: KE=1/2mv2
a)
250,000 J
b)
500,000 J
c)
5,000 J
d)
125,000 J
4.
At which point is the kinetic energy the greatest?
a)
1
b)
2
c)
3
d)
4
5.
A book is moved from the floor to the top shelf. What will happen to the energy of the book?
a)
The book will have more kinetic energy because it is higher.
b)
The book will lose energy.
c)
The book will gain chemical potential energy.
d)
The book will gain gravitational potential energy.
6.
Which sequence best describes the energy transformations taking place in an iPhone?
a)
chemical to electrical to light and sound
b)
electrical to chemical to light and sound
c)
nuclear to electrical to light and sound
d)
thermal to chemical to light and sound
7.
Which answer best describes heat being transferred through radiation?
a)
Heat being passed from a frying pan to an egg.
b)
The air above a sidewalk shimmering on a hot, summer day.
c)
Water boiling on an electric stove.
d)
Heat coming from a lamp and keeping food warm.
8.
Which points represent a solid melting?
a)
A to B
b)
B to C
c)
C to D
d)
D to E
9.
An atom contains 15 protons, 50 neutrons, and 15 electrons.
What best describes it and is the correct name for it?
What best describes it and is the correct name for it?
a)
ion, Phosphorus 65
b)
isotope, Phosphorus 65
c)
ion, Phosphorus 50
d)
isotope, Phosphorus 50
10.
If an ion has a charge of 3+, that means it has __________.
a)
3 more electrons than protons
b)
3 more neutrons than protons
c)
3 more protons than electrons
d)
3 more protons than neutrons
11.
The number of ______ of an element never changes in an atom, isotope, and ion.
a)
protons
b)
electrons
c)
neutrons
d)
electron shells
12.
One side of a cube measure 2 cm. The cube's density is 10/cm3. What is the mass of the cube?
Hint: First calculate volume using
length x width x height.
Hint: First calculate volume using
length x width x height.
a)
20 g
b)
800 g
c)
200 g
d)
80 g
13.
The ability to corrode or tarnish are examples of ___________.
a)
physical properties
b)
chemical properties
c)
physical changes
d)
chemical changes
14.
Cu + AgNO3 ---> Ag + Cu(NO3)2
This is an example of a ____________ reaction.
This is an example of a ____________ reaction.
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
15.
Metals tend to ______ valence electrons while nonmetals ______ them.
a)
gain, lose
b)
lose, gain
c)
share, gain
d)
share, lose
16.
Which types of elements are most similar to one another?
a)
Elements in the same period
b)
Elements that are classified similarly (metals, nonmetals, metalloids)
c)
Elements are not similar to one another
d)
Elements in a group/family together
17.
When a liquid turns into a solid, the particles do what?
a)
Get faster and spread out
b)
Get faster and come closer together
c)
Slow down and spread out
d)
Slow down and come closer together
18.
When dealing with gases in a sealed container, if a gas is heated, what will happen to pressure?
a)
Pressure will go up as the gas is heated
b)
Pressure will go down as the gas is heated
c)
Pressure will not change as the gas is heated
d)
Pressure will go up and down as the gas is heated
19.
Most cleaning products have a pH range between ___________.
a)
1-14
b)
1-7
c)
8-14
d)
4-7
20.
To neutralize a strong acid quickly, you would want to add
a)
strong acid
b)
strong base
c)
both acid and a neutral substance
d)
weak neutral substance
21.
Which properties below best describe the properties of a basic (pH) liquid?
a)
slippery, bitter
b)
slippery, sour
c)
Sticky, sweet
d)
They have no real feel/taste
22.
Blue litmus paper will turn red if exposed to an
a)
neutral substance
b)
water
c)
base
d)
acid
23.
Which options below describe the best way to make sugar melt faster in water?
a)
crushing it and putting it in cold water
b)
crushing it and putting it in hot water
c)
stirring the cube
d)
just dropping the cube in water
24.
When you make coffee with sugar, the sugar is the _____________.
a)
solute
b)
solvent
c)
acid
d)
neutral substance
25.
20 cubic cm of hydrogen gas is put in a sealed container and heated. What would happen to the volume of the gas as it is heated?
a)
The gas would expand
b)
The gas would shrink
c)
Nothing would change
d)
The hydrogen would turn into a liquid
26.
Metals on the far ______________ of the periodic table are the most metallic.
a)
left
b)
right
c)
top
d)
bottom
27.
Which group on the periodic table has the LEAST number of valence electrons?
a)
Group 1
b)
Group 2
c)
Group 17
d)
Group 18
28.
What is the kind of bond between two non-metals called?
a)
Ionic
b)
Covalent
c)
Lattice
d)
Metallic
29.
What is an example of a solute?
a)
Salt
b)
Water
c)
Salt water
d)
Filter
30.
What is an example of an element that doesn't like to bond?
a)
Neon
b)
Oxygen
c)
Hydrogen
d)
Selenium
31.
The formula of sodium sulfate is Na2SO4. How many elements does it contain?
a)
2
b)
3
c)
4
d)
7
32.
An ionic bond is formed between
a)
nonmetal and nonmetal
b)
metal and metal
c)
cation and anion
d)
metal and nonmetal
33.
What is the name given to the electrons in the highest occupied energy level of an atom?
a)
cations
b)
anions
c)
orbital electrons
d)
valence electrons
34.
Are atoms more stable when they are bonded together or when they are apart?
a)
Bonded Together
b)
Apart
35.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons
c)
The transfer of electrons
d)
None Of the above
36.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
37.
What usually forms a positive ion?
a)
Metal
b)
Non Metals
c)
None
38.
What usually forms a negative ion?
a)
nonmetals
b)
metal
c)
none
39.
The charge of an atom represented on the periodic table is always:
a)
Positive
b)
Neutral
c)
Negative
40.
Nonmetals are most likely to _____________ valence electrons in order to have a stable arrangement.
a)
lose
b)
gain
c)
gain or share
d)
share
41.
What is the correct name for CO2?
a)
carbon oxygen
b)
carbon oxide
c)
carbon dioxide
d)
carbon oxate
42.
The atomic number tells you what about an atom?
a)
number of valence electrons
b)
number of protons and neutrons
c)
number of neutrons and electrons
d)
number of electrons and protons in an atom.
43.
Which element has 2 energy shells and 3 valence electrons?
a)
Si
b)
B
c)
Li
d)
He
44.
Which of the following is not a property of metals?
a)
brittle
b)
malleable
c)
lustrous
d)
conductive
45.
The most reactive nonmetals on the periodic table are
a)
metalloids
b)
alkaline earth
c)
halogens
d)
noble gases
46.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
47.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
48.
Which group of elements are the most reactive metals?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
49.
Which group of the periodic table is composed of inert (not reactive) gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
50.
Balance the problem:
Al + O2 --> Al2O3
Al + O2 --> Al2O3
a)
4, 3, 2
b)
2, 4, 2
c)
4, 4, 1
d)
1, 2, 3
51.
Solve the problem: Al + S --> Al2S3
a)
1, 2, 2
b)
2, 3, 1
c)
1, 2, 2
d)
2, 3, 2
52.
What are reactants?
a)
The chemical substances that begin the reaction.
b)
The ending result of a reaction.
c)
The arrow seperating both sides of an equation.
d)
What comes from the reaction.
53.
Is this equation balanced?:
CS2 + 202 --> CO2 +2SO2
CS2 + 202 --> CO2 +2SO2
a)
Yes
b)
No
54.
Solve the problem: N2 + O2 --> NO
a)
1, 1, 2
b)
2, 1, 2
c)
2, 2, 1
d)
1, 2, 1
55.
Which problem is balanced?
a)
PbO2 + 2H2
b)
So2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
56.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
57.
What type of chemical reaction is shown below?
Al(OH)3 --> Al2O3 + H2O
Al(OH)3 --> Al2O3 + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
58.
What type of chemical reaction is this one?
CuO + CO2 --> CuCO3
CuO + CO2 --> CuCO3
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
59.
What type of chemical reaction is this one?
Ca + MgCl2 --> CaCl2 + Mg
Ca + MgCl2 --> CaCl2 + Mg
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
60.
What type of chemical reaction is this one?
C2H2 + O2 --> CO2 + H2O
C2H2 + O2 --> CO2 + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
61.
A + BC = B + AC
a)
Single Replacement
b)
Combustion
c)
Double Replacement
d)
Synthesis
62.
AB + CD = AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
63.
This type of mixture contains two or more substances that are visibly distinguishable.
a)
homogeneous
b)
heterogeneous
c)
solution
d)
colloid
64.
Describe a solute.
a)
part of solution present in largest amount
b)
gets dissolved
c)
water
d)
surrounds and breaks apart
65.
Describe a solvent.
a)
part of solution present in smallest amount
b)
part of solution present in largest amount
c)
water
d)
gets dissolved
66.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it.
c)
dissolve more solute than you should be able to.
d)
dissolve a super amount of solvent in it.
67.
Solution where more solute can still be dissolved at the given temperature.
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
68.
A beaker containing 80 grams of lead(II) nitrate, Pb(NO3)2, in 100 grams of water has a temperature of 30 ºC. Approximately how many grams of the salt are undissolved, on the bottom of the beaker?
a)
20 grams
b)
80 grams
c)
66 grams
d)
14 grams
69.
Which salt is LEAST soluble at 0 ºC?
a)
K2Cr2O7
b)
KNO3
c)
KClO3
d)
Ce2(SO4)3
70.
How many grams of sodium nitrate, NaNO3, are soluble in 100 g of water at 10 ºC?
a)
80 grams
b)
100 grams
c)
40 grams
d)
10 grams
71.
When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
72.
Potting Soil is an example of
a)
mixture of solids
b)
solute
c)
element
73.
Instant coffee that is placed in hot water is an example of:
a)
element
b)
solute
c)
mixture of solids
74.
An aluminum pie plate is an example of:
a)
mixture of solids
b)
solute
c)
element
75.
Calcium carbonate is an example of:
a)
suspension
b)
compound
c)
alloy
d)
solute
76.
A steel crowbar is an example of:
a)
alloy
b)
suspension
c)
compound
d)
element
77.
Boiling point,melting point, and density are some of an element's
a)
pure properties
b)
physical properties
c)
chemical properties
d)
hidden properties
78.
Water is best described as an example of:
a)
compound
b)
element
c)
solution
d)
molecule
79.
Two or more different elements chemically combined:
a)
an atom
b)
a compound
c)
a mixture
d)
a pure substance
80.
A mixture that appears to be evenly mixed throughout:
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
81.
mixture that does NOT appear to be evenly mixed throughout:
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
82.
Which of these is not an example of a molecule?
a)
CH4
b)
C
c)
C6H12O6
d)
H2O
83.
Which of these is a pure substance?
a)
bread
b)
table salt
c)
garden soil
d)
sea water
84.
The food you eat provides your body with ______________energy.
a)
nuclear
b)
chemical
c)
heat
d)
radiant
85.
An object that has a greater mass and __________has a greater kinetic energy than an object that has less of each.
a)
mass
b)
motion
c)
speed
d)
heat
86.
Kinetic Energy is:
a)
Energy of motion
b)
always conserved
c)
Energy due to position
87.
The ultimate source of energy is:
a)
The sky
b)
The sun
c)
Plants
d)
Movement
88.
Look at the diagram. Which point does the ball have the maximum potential energy?
a)
A
b)
B
c)
C
d)
D
89.
Look at the diagram. At which point does the ball have the maximum kinetic energy?
a)
B
b)
C
c)
D
d)
E
90.
A cell phone battery dies. It gets plugged into an electrical outlet to recharge. Which of the following energy transformations occur during the charging?
a)
mechanical to chemical
b)
electrical to solar
c)
chemical to light
d)
chemical to electrical
91.
Mrs. Tolson's students are complaining that it is hot in the classroom. She plugs in the fan and turns it on, which energy transformation occurs?
a)
mechanical to electrical
b)
electrical to mechanical
c)
chemical to mechanical
d)
electromagnetic to mechanical
92.
The Law of Conservation of Energy states that...
a)
energy can be destroyed
b)
energy can not be created or destroyed
c)
energy can only be destroyed using the force
93.
Electrical -> Mechanical -> Sound
a)
A triple beam balance measuring an object’s mass
b)
A pencil sharpener plugged into a wall outlet
c)
A projector displaying a diagram on the screen
d)
A working flashlight used to light up a dark corner
94.
Which kind of energy change occurs when a candle is burning?
a)
Chemical to light
b)
Light to electrical
c)
Solar to heat
d)
Chemical to electrical
95.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
96.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
97.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
98.
Identify the element shown in this Bohr model
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
99.
Identify the Bohr model shown
a)
Helium
b)
Oxygen
c)
Sodium
d)
Phosphorous
100.
What does an atom's period tell us?
a)
Number of protons
b)
Number of electrons
c)
Number of valence electrons
d)
Number of shells
101.
What does an atom's group tell us?
a)
Number of protons
b)
Number of electrons
c)
Number of valence electrons
d)
Number of shells
102.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
103.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
104.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
105.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
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