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WorksheetsChem B: Semester Review
Total questions: 69
Worksheet time: 2hrs 33mins
Name
Class
Date
1.
What type of chemical reaction is this one?
Al(OH)3 --> Al2O3 + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
2.
What type of chemical reaction is this one?
CuO + CO2 --> CuCO3
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
3.
What type of chemical reaction is this one?
Ca + MgCl2 --> CaCl2 + Mg
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement
4.
Solve the problem: Al + O2 --> Al2O3
a)
4Al + 3O2 --> 2Al2O3
b)
2Al + 4O2 --> Al2O3
5.
This equation violates which law of chemistry? 2H2O + O2 --> 4MgO + 3Fe
a)
Kinetic Molecular Theory
b)
Conservation of Mass
c)
Boyle's Law
d)
Avogadro's Law
6.
What is a reactant?
a)
The chemical substances that begin the reaction.
b)
What comes from the reaction.
7.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2+ H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
8.
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.
9.
Which of the following gases is NOT diatomic?
a)
oxygen
b)
iodine
c)
carbon dioxide
d)
fluorine
10.
Which of the following gases is LEAST reactive?
a)
Ne
b)
F2
c)
O2
d)
He
11.
What will happen if a balloon is in a hot outdoor environment?
a)
Particles will move less
b)
Gas will compress
c)
Gas will expand
12.
Why can you shape a balloon filled with gas?
a)
The gas is able to be compressed
b)
Magic
c)
The particles move around for space
d)
The gases move to the walls of the balloons
13.
What is the equation for Boyle's Law?
a)
P1*V1=P2*V2
b)
V1/T1 = V2/T2
c)
L*W
14.
At a constant volume, the pressure increases. What happens to the temperature?
a)
increases
b)
decreases
c)
stays the same
15.
At 25 degrees Celsius, a gas is approximately 3 L at standard pressure. What is the new volume if the pressure increases to 3 atm?
a)
9 L
b)
1 L
c)
9 atm
d)
1 atm
16.
A gas has a volume of 22.4 L at STP. What is the new volume if the pressure is increased to 2 atm and the temperature is decreased to 250 K?
a)
10.3 L
b)
24.5 L
c)
48.9 L
d)
20.6 L
17.
A sample of carbon dioxide at STP is 0.50 L. How many grams of carbon dioxide do we have?
a)
0.48 g
b)
0.49 g
c)
1.96 g
d)
0.98 g
18.
What is the mass of 1.2 x 1025 atoms of sulfur (S) =32 g/mol) ?
a)
1.2.x.1025 / 6 x 1023 x 32
b)
1.2 x 1025 x 32
c)
2 x 32
19.
How many moles of each atom are there in Al2O3?
a)
3 Al, 2 O
b)
2 Al, 3O
c)
6 Al, 6O
d)
1 Al 1 O
20.
What is the molar mass of H2O?
a)
16 g/mol
b)
17 g/mol
c)
18 g/mol
d)
19 g/mol
21.
How many grams is 1.2 moles of Neon?
a)
0.05 grams
b)
16.6 grams
c)
21.2 grams
d)
24 grams
22.
How do you calculate the molarity of a solution?
a)
By tasting it.
b)
Dividing the moles of solute by the L of solution
c)
Dividing the moles of solute by the kg of solvent
d)
By adding the sum of the molecular weight of the elements in the substance.
23.
A 3 M solution has how many moles per liter?
a)
1
b)
2.5
c)
4
d)
3
24.
What is the difference between concentration and saturation?
a)
concentration is a fixed % and saturation refers to amount of solute dissolved
b)
concentration refers to amount of solute dissolved and saturation is a fixed %.
c)
Nothing
d)
All of the above
25.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
26.
The ___ is the thing being dissolved in a solution.
a)
solute
b)
solvent
c)
substance
d)
stuff
27.
What is ionization?
a)
The process in which charged molecules lose or gain electrons
b)
Breaking the solute into small pieces and spreading throughout the solvent.
c)
The process in which an ionic compound separates into ions in a solution.
d)
The process in which neutral molecules lose or gain electrons
28.
What is the purpose of the pH scale?
a)
to describe solubility
b)
to describe concentration of hydroxide ions
c)
to describe the concentration of hydrogen ions
d)
to tell the color of something
29.
The "like dissolves like" rule is the reason why water cannot dissolve
a)
salt
b)
sugar
c)
vinegar
d)
oil
30.
Forms hydroxide ions in water
a)
Acids
b)
Bases
c)
All
31.
Forms hydronium ions in water.
a)
Acids
b)
Bases
c)
All
32.
The pH scale is based off of the concentration of _________ ions.
a)
Oxygen
b)
Hydronium
c)
Nitrogen
d)
None of the others
33.
This image represents
a)
Neutralization reaction
b)
synthesis
c)
decompostion
d)
single displacement
34.
Bleach is a strong base, what is the pH level of bleach?
a)
13
b)
14
c)
1
d)
2
35.
Which pH solution is 10 times acidic than solution has a pH=5?
a)
pH=50
b)
pH=.5
c)
pH=6
d)
pH=4
36.
What is NH3 acting as in the included equation?
a)
Acid
b)
Base
c)
Conjugate acid
d)
Conjugate base
37.
A solution of NaOH would most likely have a pH _____ 7
a)
less than
b)
more than
c)
equal to
38.
A solution has [H+] = 1.0 x 10-4. What is the pH?
a)
1
b)
2
c)
4
d)
10
39.
Water is special because it has a positive and negative part to its molecule. This makes it...
a)
magnetic
b)
hybrid
c)
polar
d)
electric
40.
Cohesion is when water sticks to...
a)
itself
b)
something else
41.
Adhesion is when water sticks to...
a)
itself
b)
something else
42.
What property of water helps to moderate earth's temperature?
a)
adhesion
b)
chohesion
c)
Specific heat capacity
d)
Latent heat of vaporization
43.
Attractions between water molecules is the result of
a)
Covalent bonds
b)
Ionic bonds
c)
Polar bonds
d)
Hydrogen bonds
44.
Why does water move from the roots to the leaves of plants?
a)
Water is pushed by solutes
b)
Capillary action pulls the water molecules like a chain
c)
Water is pulled by gravity
d)
Water’s cohesion causes it to “pull” towards the leaves
45.
Water is polar because...
a)
The unequal sharing of electrons gives the water molecule a slight negative charge near its oxygen atom and a slight positive charge near its hydrogen atoms.
b)
The molecule has two poles, at which the it is colder than other regions of the molecule.
c)
The unequal sharing of electrons gives the water molecule a slight negative charge near its hydrogen atoms and a slight positive charge near its oxygen atom.
d)
The water molecule is neutral.
46.
Acids produce _________ ions when they break down or dissocciate.
a)
Hydroxide (OH-)
b)
Water
c)
Chlorine (Cl-)
d)
Hydrogen (H+)
47.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
48.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
49.
What is the [H+] if the pH is 4.0?
a)
1.0 x 10-10 M
b)
1.0 x 10-4 M
c)
1.0 x 10-14 M
d)
1.0 x 10-7 M
50.
The greater the pOH, the smaller the concentration of
a)
OH-
b)
H+
51.
ammonium chloride
a)
NH3Cl2
b)
NH4Cl
c)
NH4ClO3
d)
NH4Cl2
52.
calcium phosphate
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
53.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
54.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
55.
copper(II) chloride
a)
CuCl2
b)
CuCl
c)
Cu2Cl
d)
Cu2Cl2
56.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
57.
Which has the greater EN:
N or C?
N or C?
a)
C
b)
N
58.
Which has the greater EN:
H or F?
H or F?
a)
H
b)
F
59.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends.
60.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
61.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6?
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L
c)
1 mol = 6.02x 1023 particles
d)
more than one
62.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
63.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
64.
Phase change from a solid to a gas.
a)
sublimation
b)
deposition
c)
condensation
d)
evaporation
65.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
66.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
67.
What can be determined by measuring the speed of molecules?
a)
volume
b)
density
c)
pressure
d)
temperature
68.
According to the phase diagram, water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
69.
What state of matter is X?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
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