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Date: _____________
Chemistry – Final Exam Review packet
Lab Equipment, Reports and Safety:
1.
Identify the following equipment. What is it used for?
a.
Beaker
b.
Graduated cylinder
c.
Balance
d.
Goggles
Could you identify it from a picture?
e.
Erlenmeyer flask
f.
Beaker and Crucible Tongs
g.
Striker
2.
Concepts & lab reports: Define the following. What are they used for?
a.
precipitate
e.
purpose
b.
reference material (reference
f.
hypothesis
solution)
g.
data
c.
control
h.
conclusion
d.
variable
Water Unit:
1.
Define the following mixtures. Give two real-life examples of each. How could you
experimentally test for each? How would you separate the components?
a.
Solution
b.
Colloid
2.
What is the Tyndall test? When would you use it?
3.
Do the following conversions. Show your work.
Indicate the type of measurement (distance, volume or mass)
c.
Suspension
a. Convert 150 km to meters
b. Convert 45 cL to mL
c. Convert 0.053 grams to mg
d. Convert 60 mL to cm3
e. Convert 15 kg to mg
4.
Calculate the density of an object that has a mass of 38.45 g and occupies 24.7 cm3.
5.
What types of substances are removed from mixtures using filtration? Adsorption? Distillation?
Think about the foul water lab!
6.
Identify the following as physical or chemical property by writing P or C next to each.
Page 1 of 13
Name: ___________________________________________
a.
b.
c.
d.
e.
density
surface tension
liquid at room temperature
boiling point
reacts with an acid to produce H2 gas
f.
g.
h.
i.
j.
Date: _____________
electrically conductive
dissolves ionic compounds
breaks down into H2 (g) and O2 (g)
color
inert
7.
Draw and label a picture of a water molecule. Explain it in terms of being polar.
Show hydrogen bonds between different water molecules.
8.
Why does table salt (NaCl) dissolve in water but not cooking oil?
9.
Define the following: solute, solvent and solution.
10.
35 g of ethanol is dissolved in 115 g of water. What is the % concentration of ethanol?
11.
12.
How many grams of salt would be found in 15 grams of a 25% NaCl solution?
What is hard water? What does it mean to soften hard water?
Use the following two graphs to answer questions 13 – 19
13.
What mass of KNO3 will dissolve in 100 g of water at 50°C?
________________
14.
What mass of KBr will dissolve in 100 g water at this temperature?
________________
15.
25 g of KNO3 is dissolved in 100 g of water at 30°C. Is this
solution saturated, unsaturated or supersaturated?
16.
In order to make this solution saturated, how much more KNO3 must be added?
17.
What is the minimum mass of water to dissolve 30 g KNO3 at 30°C?
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Name: ___________________________________________
Date: _____________
18.
What mass of oxygen can be dissolved in 1000 g of water at 30°C? At 20°C?
19.
What mass of oxygen can be dissolved in 100 g of water at 20 °C?
20.
Fill in the following table indicating if the substance would be soluble or insoluble.
Polar Solute
Non-polar Solute
Ionic solute
Polar Solvent
Non Polar Solvent
21.
Identify each as an acid, base or neutral substance when dissolved in water. Indicate the pH
(less than, greater than, or equal to 7) of the solution formed from this substance.
a.
b.
c.
d.
NaBr
HBr
HNO3
NaOH
22. If the concentration of H3O+ in a solution is 1 x 10-5, what is the pH? ______
Resources Unit:
1.
An element is found that is a good conductor of electricity, is ductile, brittle and doesn’t react
with an acid. This element is best classified as a (metal / nonmetal / metalloid).
2.
The current periodic table is arranged according to increasing _____________ ______________.
3.
Elements in the same vertical column are in the same ____________ or ___________ and have similar
physical and chemical properties due to similar _____________ ___________.
4.
Estimate the boiling point of krypton if the bp of Ar is -186 °C and that of Xe is -112 °C.
5.
Define:
a.
element
b.
cation
c.
anion
6.
d.
e.
Fill in the following table:
Name
Symbol
Atomic
Number
#
protons
#
neutrons
in most
common
isotope
ionic compound
covalent compound
Electron configuration
Atomic Mass
Hydrogen
Cu
7
197
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Name: ___________________________________________
7.
Date: _____________
Of the following elements: Na Mg Li K
a.
Which element is in the fourth energy level?
b.
Which are in the same family/group?
c.
Which are in the same period?
8. Label the blank PT with
 s, p, d block locations
 metals/nonmetals/metalloids **where’s
the “stairstep”?
 valence electrons of elements within
Groups I – VIII.
 Predicted ion charges of elements within
Groups I – VIII.
9.
Calculate the molar masses of each substance below. Round atomic masses to 1 decimal place.
Particle name? (molecule or
Chemical
Molar Mass
formula unit?)
SrCl2
OF2
Co(NO3)2
CO2
10. Complete the following table:
Element or
compound?
If a compound,
ionic or covalent?
Particle name?
(atom, molecule or
formula unit)
NaF
Cl2
H2O
LiCl
Al
CBr4
NH3
Ca(NO3)2
He
C3H8
11.
Complete the following mole conversions. Show all your dimensional analysis work.
a.
How many moles are in 72.9 g of HCl?
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Name: ___________________________________________
12.
b.
How many moles are in 11.2 L of CO2 gas at STP?
c.
d.
How many molecules are in 720 g of C6H12O6?
How many grams are in 3.5 mol of Ca3(PO4)2?
e.
What is the volume of 1.35 mol of Cl2 gas at STP?
f.
How many formula units are in 85 g of AgNO3?
g.
Convert 86.84 g of LiBr to moles.
h.
Convert 2.5 g of CuCl2 to moles.
i.
How many grams of lithium are there in 3.45 moles?
j.
How many moles of nitrogen are there in 4.3 × 1023 molecules?
k.
How many cadmium atoms are there in 6.57 × 103 moles?
l.
How many grams of SO2 are 4.5 × 1024 molecules?
Percent Composition. Calculate the percent composition (by mass) of each element in the
following:
a.
C in CH4
c.
Ba in BaCO3
b.
13.
Date: _____________
H in H2O
d.
N in Cu(NO3)2
Redox Reactions. Indicate the substance being oxidized, the substance being reduced, and
the oxidizing and reducing agents in the following equations:
a. 3 AgNO3 + Al  Al(NO3)3 + 3 Ag
b. 2 Li + CuCl2  2 LiCl + Cu
c. 2 NaCl + MgO  Na2O + MgCl2
d. Discuss the redox process that occurs when a metal is refined from its ore.
Page 5 of 13
Name: ___________________________________________
14.
Date: _____________
Indicate the oxidation number (charge) of each element in the following equations:
Write the charges above the symbol of each element.
a.
2 Li + CuCl2 → 2 LiCl + Cu
b.
2 NaCl + MgO → Na2O + MgCl2
15. Write half-reaction equations for each reaction in question 13. Remember that both equations
have to have the same number of electrons!
a.
oxidation:
reduction:
b.
oxidation:
reduction:
16.
Use the metal activity series to predict whether the following reactions will occur. If they do,
write the products and then balance the equation.
a.
___ CuCl2 + ___ Al
→
b.
___ NaNO3 + ___ Zn
→
c.
___ LiCl + Ag ___
→
d.
___ K + ___ Al2(SO4)3 →
17.
Explain why this reaction is NOT an example of a Redox reaction.
2 NaNO3 + BaI2 → Ba(NO3)2 + 2 NaI
18.
Complete the table below.
cation, anion or neutral
atom?
Number of electrons in substance
Li+1
S-2
Na0
bromide ion
magnesium ion
19.
Which have a full octet? Choose all that apply.
20.
Complete the table below.
Name of
element
Metal, nonmetal
or metalloid?
How many
valence
electrons?
Na
Xe
F
Na+1
Electron configuration
Ca
Se
Page 6 of 13
Name: ___________________________________________
Date: _____________
Zn
F
K
Si
Petroleum Unit:
1.
Draw the electron-dot structure for the following compounds:
a) C2H6
b) C2H4
c.) CH4
d) C2H4Cl2 (draw both isomers of this)
2.
Draw two isomers of C6H14.
3.
Draw and name the alkane, alkene and alkyne with three carbons.
4.
Which is saturated: C2H4 or C2H6 ? Why?
5.
Using the molar heats of combustion table, write thermochemical equations for the combustion
of:
a.
methane
b.
butane
c.
octane
6. Using the molar heats of combustion table, calculate the energy released from the burning of:
a.
3 mol C2H6
7.
b.
24 grams methane
c.
5.4 x 1025 molecules C4H10
The specific heat of water is 4.2 J/g°C. How many joules are absorbed if 10 g of water is heated
from 25 °C to 37 °C?
Page 7 of 13
Name: ___________________________________________
Date: _____________
8.
Which of the following: CH4
C3H8
a.
has the highest boiling point
b.
is the most viscous (define viscous, also)
c.
has the greatest intermolecular forces
C12H26
9.
In a fractionating tower, CH4 and C9H20 would be separated because they have different
__________________. Methane would be collected (higher / lower) on the tower.
10.
Identify the functional group(s) present in each molecule by circling the group(s). Classify the
group as an alcohol, acid or ester functional group.
Air Unit:
1.
Which gas is in greatest abundance in the atmosphere?
2.
Describe the relationship between altitude, air pressure, temperature, and number of molecules.
3.
If a balloon changes its volume from 2 L to 12 L, how would the Kelvin temperature of the gas in
the balloon change? Give a numerical answer. What gas law applies here?
4.
What are the conditions of temperature and pressure that scientists call STP conditions?
5.
6.
Write the equations for Boyle’s Law, Charles’ Law, Gay-Lussac’s law, and the Combined gas law.
A gas has a volume of 350 mL at 23 C. What is the new volume of the gas, if the temperature is
dropped to 5 C?
Which gas law applies here? ______________________
7.
A balloon contains argon gas at a pressure of 202.6 kPa and 29 C. Calculate the new
temperature of the gas, if the volume is held constant, but the pressure is reduced to 99.4 kPa.
Which gas law applies here? ______________________
Page 8 of 13
Name: ___________________________________________
Date: _____________
8.
A bicycle tire is filled with 425 mL of air, until the pressure is 1.35 atm. If 200 mL of air is added
to the tire, what will be the new pressure?
Which gas law applies here? ______________________
9.
A weather balloon has a volume of 18 L at STP conditions. Soon after, the pressure changes to
0.75 atm and the volume increases to 25 L. What is the new Kelvin temperature of the gas?
Which gas law applies here? ______________________
10.
A container of nitrogen gas is at 150 °C, and a pressure of 101.3 kPa. Without changing the
volume of the gas, what will the Celsius temperature of the gas be if the pressure is changed to
25.4 kPa?
Which gas law applies here? ______________________
11.
A sample of helium gas with an unknown volume is at 300 K and 101.6 kPa. When the gas is
placed in a container with a volume of 6.5 mL and a temperature of 125 K, , the pressure is
measured as 103.4 kPa. What was the original volume of the gas sample?
Which gas law applies here? ______________________
12.
Whenever you use a temperature value in a gas law equation, what unit must the temperature
be in? How do you convert between Celsius and this temperature unit?
13.
Convert 25 °C to Kelvin.
15.
What is room temperature in Celsius? __________ In Kelvin? _______________
16.
17.
What is the volume of one mole of any gas at STP conditions?
How many moles are in 18.6 L of CO gas at STP?
18.
Describe the greenhouse effect. What causes it? How can we effect change to reduce the
damaging effects of global warming?
14.
Convert -120 °C to Kelvin
________________________
19.
Explain what the different areas of this graph
mean, and what the role of O3, CO2 and water vapor are in
our atmosphere.
Page 9 of 13
Name: ___________________________________________
20.
Date: _____________
Graph interpretation.
A temperature “anomaly” indicates the difference from the average temperature.
Explain in a couple of sentences what this graph indicates about global temperature anomalies.
Base your discussion on the dark line – the 5-year average. The year 1980 is significant!
Page 10 of 13
Name: ___________________________________________
Date: _____________
Chemical Reactions Unit:
1.
List three ways that coefficients can be interpreted in a chemical reaction.
2.
What are the seven diatomic elements? How can you remember them?
3.
Identify products, reactants, coefficients, and subscripts in the following equation:
a.
4.
Ca (s) + 2 H2O (l) → Ca(OH)2 (aq) + H2 (g)
Write the formulas for the compounds formed between the element or ion pairs listed below:
Remember…balance the charges!
magnesium and sulfide
barium and iodide
aluminum and carbonate ion
lead(IV) and sulfate
sodium and chloride
lithium and hydroxide
beryllium and hydroxide
iron(III) and nitride
ammonium and phosphate ions
5.
6.
Balance the following equations.
a.
_____ S8 + _____ O2 → _____ SO3
b.
_____ N2 + _____ O2 → _____ N2O
c.
_____ HgO → _____ Hg + _____ O2
d.
_____ CO2 + _____ H2O → _____ C6H12O6 + _____ O2
e.
_____ SiCl4 + _____ H2O → _____ H4SiO4 + _____ HCl
f.
_____ Na2CO3 + _____ HCl → _____ NaCl + _____ H2O + _____ CO2
g.
_____ Na + _____ H2O → _____ NaOH + _____ H2
Transform these word equations into balanced chemical equations.
a.
Aluminum sulfate + Calcium hydroxide  Aluminum hydroxide + Calcium sulfate
b.
Aluminum + Hydrogen chloride  Aluminum chloride + Hydrogen gas
c.
Lead(II) nitrate  Lead(II) oxide + Nitrogen dioxide + Oxygen gas
Page 11 of 13
Name: ___________________________________________
Date: _____________
Stoichiometry Problems. Show all the dimensional analysis work!
7.
Consider the reaction:
4 NH3 (g) + 5 O2 (g) → 6 H2O (g) + 4 NO (g)
a.
How many moles of NO (g) are produced from 2.00 mol of NH3 (g)?
b.
How many grams of H2O (g) is produced from 4.00 mol of O2 (g) ?
c.
How many liters of NH3 (g) is required to react with 3.00 liters of O2 (g)?
8.
How many grams of silver chloride can be produced from 34.0 grams of silver nitrate according
to the reaction below?
__ AgNO3 + ___ CuCl2 → ___ AgCl + ___ Cu(NO3)2
9.
Chlorine gas reacts with sodium metal to produce sodium chloride. What mass of Chlorine will
be needed to react with 12.3 g of sodium?
___ Cl2 +___ Na → ___ NaCl
10.
Aluminum metal reacts with a solution of copper(II) nitrate. If you want to produce
5.4 x 1024 atoms of copper, how many moles of aluminum metal are needed?
___ Al + ___ Cu(NO3)2 → ___ Cu + ___ Al(NO3)3
11.
Limiting Reactants
a.
How do limiting reactant problems “look” different from regular stoichiometry problems?
b.
Our bodies burn sugar, forming water and carbon dioxide as follows:
1 C6H12O6 + 6 O2 → 6 H2O + 6 CO2
If your body takes in 20 moles of O2 from the air, and you eat 45 moles of sugar,
which is the limiting reactant?
c.
Using the same reaction equation, how many grams of CO2 can be produced from the
reaction of 15 grams of sugar and 25 grams of oxygen?
Page 12 of 13
Name: ___________________________________________
Date: _____________
Rates of Reactions Unit:
1.
Explain why raising the temperature speeds up a reaction.
2.
Explain why a catalyst speeds up a reaction.
3.
Is the following reaction endothermic or exothermic?
Determine the numerical values of EA and ΔH.
4. If the products have less energy than the reactants, then the reaction is (exothermic/endothermic).
5. Is the following reaction endothermic or exothermic?
N2 + 3 H2 → 2 NH3 + energy
Page 13 of 13