Download Lab Stuff:

Name: ___________________________________________
Date: _____________
Chemistry – Final Exam Review packet 2015
Lab Equipment, Reports and Safety:
Big Ideas:
1. Laboratory equipment has specific uses, and also limitations on their uses.
2. Each piece of equipment provides data with specific units.
3. Safety rules and procedures are designed to protect you from contact with chemicals and
broken glass. Cuts from broken glass is one of the most common injuries in the chemistry lab.
4. Your eyes must always be protected with safety goggles.
1.
2.
Identify the following equipment. What is it used for? Could you identify it from a picture?
a.
Beaker
b.
Graduated cylinder
c.
Balance
d.
Goggles
e.
Erlenmeyer flask
f.
Beaker and Crucible Tongs
g.
Striker
Concepts & lab reports: Define the following. What are they used for?
a.
precipitate
b.
reference material (reference solution)
c.
control
d.
variable
e.
purpose
f.
hypothesis
g.
data
h.
conclusion
Page 1 of 20
Name: ___________________________________________
Date: _____________
Water Unit:
Big Ideas:
1. Chemists use the metric system when recording their measurements.
2. Dimensional analysis must be used to convert between measurement units.
3. Chemicals have both physical and chemical properties that can be used to tell them apart, and also
to separate components of a mixture.
4. Water’s polarity makes it an excellent solvent.
5. When it comes to evaluating a solute/solvent relationship, remember the phrase
“like dissolves like.”
6. Solubility can be quantified with a solubility curve, and by calculating the % concentration of a
solution.
7. An imbalance of H3O+ and OH- ions causes solutions to be either acidic or basic.
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
c.
Suspension
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)
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
Page 2 of 20
Name: ___________________________________________
Date: _____________
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.
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
density
surface tension
liquid at room temperature
boiling point
reacts with an acid to produce H2 gas
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.
How many grams of salt would be found in 15 grams of a 25% NaCl solution?
Page 3 of 20
Name: ___________________________________________
Date: _____________
Use the following two graphs to answer questions 12 – 18
12.
What mass of KNO3 will dissolve in 100 g of water at 50°C?
13.
What mass of KBr will dissolve in 100 g water at this temperature?
14.
25 g of KNO3 is dissolved in 100 g of water at 30°C. Is this solution saturated, unsaturated or
supersaturated?
15.
In order to make this solution saturated, how much more KNO3 must be added?
16.
What is the minimum mass of water to dissolve 30 g KNO3 at 30°C?
17.
What mass of oxygen can be dissolved in 1000 g of water at 30°C? At 20°C?
18.
What mass of oxygen can be dissolved in 100 g of water at 20 °C?
19.
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
Page 4 of 20
Name: ___________________________________________
20.
Date: _____________
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
21. If the concentration of H3O+ in a solution is 1 x 10-5, what is the pH? ______
Resources Unit:
Big Ideas:
1. Ionic compounds form when atoms gain or lose electrons. Metals lose electrons, nonmetals gain them.
2. The number of electrons gained or lost can be predicted with an understanding of the octet rule and the
number of valence electrons an atom contains.
3. The periodic table is organized by electron configuration, and elements are classified as metals,
nonmetals or metalloids based on physical and chemical properties.
4. Atoms have a central nucleus that contains the protons and neutrons, and electrons are found in
orbitals located outside the nucleus.
5. Electron configurations are used to describe locations of electrons within levels, sublevels and orbitals.
6. Metal reactivity is summarized in the Metal Activity Series.
7. The quantity 6.02 x 1023 is called a mole, and the periodic table lists the mass of 1 mole of each
element’s atoms, called the molar mass of the element.
8. Conversions between moles, particles, and mass are widely used in chemistry.
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.
Page 5 of 20
Name: ___________________________________________
5.
6.
Date: _____________
Define:
a.
element
b.
cation
c.
anion
d.
ionic compound
e.
covalent compound
Fill in the following table:
Name
Symbol
Atomic
Number
#
protons
#
neutrons
in most
common
isotope
Electron configuration
Atomic Mass
Hydrogen
Cu
7
197
7.
Of the following elements:
a.
b.
c.
8.
Na Mg Li K
Which element is in the fourth energy level?
Which are in the same family/group?
Which are in the same period?
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.
Page 6 of 20
Name: ___________________________________________
9.
Date: _____________
Calculate the molar masses of each substance below. Round atomic masses to 1 decimal place.
Chemical
Molar Mass
Particle name?
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?
b.
How many moles are in 11.2 L of CO2 gas at STP?
c.
How many molecules are in 720 g of C6H12O6?
d.
How many grams are in 3.5 mol of Ca3(PO4)2?
Page 7 of 20
Name: ___________________________________________
12.
Date: _____________
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
b.
H in H2O
c.
Ba in BaCO3
d.
N in Cu(NO3)2
Page 8 of 20
Name: ___________________________________________
13.
Date: _____________
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.
14.
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 →
Page 9 of 20
Name: ___________________________________________
17.
Date: _____________
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
Zn
F
K
Si
Page 10 of 20
Name: ___________________________________________
Date: _____________
Petroleum Unit:
Big Ideas:
1. Carbon atoms make 4 bonds, and can arrange these bonds by using single, double, or triple
bonds to other atoms.
2. Electron-dot and structural formulas describe the bonds between atoms in alkanes, alkenes
and alkynes.
3. Petroleum is a nonrenewable resource, and many everyday materials are produced from
petrochemical starting materials. Fractional distillation is used to separates the fractions
(components) of petroleum.
4. Compounds can be isomers if they have the same molecular formula, but different
structural formulas.
5. Hydrocarbons can be evaluated as possible fuel sources by examining their heats of
combustion.
6. Energy values can be inserted into a balanced chemical equation.
7. The specific heat of a substance is a measure of its resistance to temperature change.
Energy gained or lost = (mass) (specific heat constant) (change in temperature)
8. Functional groups are the reactivity centers of hydrocarbon molecules.
1.
9. Intermolecular forces are attractions between molecules, and help explain why a molecule
sample has a particular state of matter. Viscosity is one way we “see” IMA’s at work.
Draw the electron-dot structure for the following compounds:
a.
C2H6
b.
C2H4
c.
CH4
d.
C2H4Cl2 (there are two isomers of this – try to draw both!)
2.
Draw two isomers of C6H14.
3.
Draw and name the alkane, alkene and alkyne with three carbons.
Page 11 of 20
Name: ___________________________________________
Date: _____________
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
b.
24 grams methane
c.
5.4 x 1025 molecules C4H10
7.
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?
8.
Which of the following:
a.
b.
c.
9.
CH4
C3H8
C12H26
has the highest boiling point
is the most viscous (define viscous, also)
has the greatest intermolecular forces
In a fractionating tower, CH4 and C9H20 would be separated because they have different
__________________. Methane would be collected (higher / lower) on the tower.
Page 12 of 20
Name: ___________________________________________
10.
Date: _____________
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.
Chemical Reactions Unit:
Big Ideas:
1. Chemical reactions must be balanced with coefficients to obey the law of conservation of
mass/atoms.
2. Coefficients are interpreted as either particle, mole, or (if everything is a gas) liter ratios.
3. Stoichiometry is the name given to the process of using coefficients as mole ratios to convert
between chemicals in a reaction equation. How much is used? How much is made? These
questions can be answered with a stoichiometric calculation.
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 equations:
a.
Ca (s) + 2 H2O (l) → Ca(OH)2 (aq) + H2 (g)
b.
6 H2O + 4 NO → 4 NH3 + 5 O2
Page 13 of 20
Name: ___________________________________________
4.
Date: _____________
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 14 of 20
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)
8.
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)?
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
Page 15 of 20
Name: ___________________________________________
11.
Date: _____________
Limiting Reactants
a.
b.
How do limiting reactant problems “look” different from regular stoichiometry problems?
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?
Rates of Reactions Unit:
Big Ideas:
1. Kinetics is the study of reaction speed.
2. Reaction speed is controlled by 4 factors: concentration of reactants, temperature, surface area of
reacting molecules, and use of a catalyst.
3. Speeding up a reaction does not produce more product – it produces the same amount of product in
a shorter amount of time.
4. Enthalpy diagrams can be used to indicate ΔH, EA, and whether a reaction is exothermic or
endothermic.
Page 16 of 20
Name: ___________________________________________
Date: _____________
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
Air Unit:
Big Ideas:
1. The atmosphere is divided into 3 regions according to temperature variation: the troposphere,
the stratosphere, and the mesosphere.
2. 4 variables describe a gas’ behavior: P, V, n and T.
3. Boyle, Charles and Gay-Lussac developed mathematical gas laws that are used to predict and
calculate changes in gas properties.
4. At STP, one mole of any gas occupies a volume of 22.4 L. This is called the molar volume of a
gas.
5. The greenhouse effect the name given to the trapping of infrared radiation within Earth’s
atmosphere. Water vapor, carbon dioxide and methane are significant greenhouse gases.
6. Climate scientists agree that the amount of CO2 in our atmosphere has increased within the last
150 years, and that the primary cause of this increase is from anthropogenic (human) sources,
including the burning of fossil fuels.
Page 17 of 20
Name: ___________________________________________
Date: _____________
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.
Write the equations for Boyle’s Law, Charles’ Law, Gay-Lussac’s law, and the Combined gas law.
6.
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 18 of 20
Name: ___________________________________________
8.
Date: _____________
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?
Page 19 of 20
Name: ___________________________________________
Date: _____________
13.
Convert 25 °C to Kelvin.
14.
Convert -120 °C to Kelvin
15.
What is room temperature in Celsius? In Kelvin?
16.
What is the volume of one mole of any gas at STP conditions?
17.
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?
19.
Explain what the different areas of this graph mean, and what
the role of O3, CO2 and water vapor are in our atmosphere.
20.
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 20 of 20