I.
Binary Ionic Compounds. Give the correct name or formula:
CsBr2
1. Cesium bromide
sodium chloride
6. NaCl
BaO
2. Barium oxide
calcium fluoride
7. CaF2
SrI2
3. Strontium iodide
lithium sulfide
8. Li2S
AlCl3
4. Aluminum chloride
cesium nitride
9. Cs3N
Rb2O
5. Rubidium oxide
aluminum oxide
10. Al2O3
II.
Ternary Ionic Compounds. Give the correct name or formula:
NaNO3
1. Sodium nitrate
sodium hydroxide
Na3PO4
2. Sodium phosphate
ammonium carbonate 7. (NH4)2CO3
6. NaOH
Ca(NO3)2 3. Calcium nitrate
lithium sulfate
8. Li2SO4
MgSO4
4. Magnesium sulfate
cesium phosphate
9. Cs3PO4
Ba3(PO4)2 5. Barium phosphate
aluminum nitrate
10. Al(NO3)3
NAME
acetate
nitrate
hydroxide
phosphate
FORMULA
NAME
FORMULA
-1
C2H3O2
ammonium NH4+1
NO3-1
OH-1
sulfate
SO4-2
PO4-3
carbonate CO3-2
III.
Balance the following reactions, and name the reaction type. Circle the reactants:
Reaction Type
Double Replacement
1 Ca(NO3)2 + 1 Li2CO3 2 LiNO3 + 1 CaCO3
Double Replacement
Combustion
Single Replacement
Synthesis
Decomposition
Double Replacement
(Acid-Base Neutralization)
Combustion
Single Replacement
Decomposition
1 Al(NO3)3 + 3 LiOH 1 Al(OH)3 + 3 NaNO3
1 C3H8 + 5 O2 3 CO2 + 4 H2O
2 Na + 2 H2O 2 NaOH + 1 H2
16 Al + 3 S8 8 Al2S3
1 Na2CO3 1 Na2O + 1 CO2
2 HNO3 + 1 Mg(OH)2 1 Mg(NO3)2 + 2 H2O
2 C4H10 + 13 O2 8 CO2 + 10 H2O
3 Na + 1 FeCl3 3 NaCl + 1 Fe
2 KClO3 2 KCl + 3 O2
IV. Find the formula mass of the following:
78
1. Na2S
2(23) + 32
85 3. (NH4)3P
3(14) + 12 + 31
261
2. Ba(NO3)2
137 + 2(14) + 6(16)
159 or 160 4. CuSO4
63.5 + 32 + 4(16)
V. Basic Stoichiometry
1. What is the mass of 7.50 moles of sulfur dioxide (SO2) ?
7.50mol SO 2 ∗
64.1g SO 2
= 481g SO 2
1mol SO 2
2. If you have a 10.2 L container of helium (He) gas at STP, how many moles are in there?
10.2 L He ∗
1mol He
= 0.455mol He
22.4 L He
3. How many moles are there in 15.0g of sodium fluoride (NaF)?
15.0 g NaF ∗
1mol NaF
= 0.357 mol NaF
42 g NaF
4. What is the mass of 1.54 L of sulfur hexachloride (SCl6) ?
1.54 L SCl6 ∗
1mol SCl6 244.8 g SCl6
∗
= 16.8 g SCl6
22.4 L SCl6 1mol SCl6
5. What volume would 10.0 grams of carbon dioxide (CO2) gas occupy at STP?
10.0 g CO 2 ∗
1mol CO 2 22.4 L CO 2
∗
= 5.09 L CO 2
44 g CO 2 1mol CO 2
VI. Find the percent composition for the following:
1. Li2O
2(6.94) + 16 = 29.88
13.88 g
% Li =
x100% = 46.5%
29.88 g
16 g
%O =
x100% = 53.5%
29.88 g
2. N2O4
3. Fe2(CO3)3
2(14) + 4(16) = 92
28 g
%N =
x100% = 30.4%
92 g
64 g
%O =
x100% = 69.6%
92 g
2(55.8) + 3(12) + 9(16) = 292
112 g
% Fe =
x100% = 38%
292 g
36 g
%C =
x100% = 12%
292 g
144 g
%O =
x100% = 49%
292 g
4. A 0.63g sample of magnesium is heated to form 1.04g of magnesium oxide.
% Mg =
VII.
0.63 g
x100% = 60.6% → %O = 100.0 − 60.6 = 39.4%
1.04 g
Equation Stoichiometry
1) Answer the following questions using the following equation:
3 H2(g) + N2(g) 2 NH3(g)
a. How many moles of ammonia will be produced when you react 0.476 moles of hydrogen
2 NH 3
0
.
476
H
∗
= 0.317 mol NH 3
2
with excess nitrogen?
3 H2
b. At STP, what volume of hydrogen gas do you need to react with 3.81 L of nitrogen gas?
3.81L N 2 ∗
3 H2
= 11.4 L H 2
1 N2
c. If you want to produce 10.0 g of ammonia for your cleaning product, how many grams of
hydrogen do you need?
10.0 g NH 3 ∗
1mol NH 3 3 H 2
2g H2
∗
∗
= 1.78 g H 2
17 g NH 3 2 NH 3 1mol H 2
d. If you begin with 6.50 liters of nitrogen gas at STP, how many grams of ammonia will you
produce?
2 NH 3 17 g NH 3
1 N2
6.50 L N 2 ∗
∗
∗
= 9.87 g H 2
22.4 L N 2 1 N 2 1mol NH 3
e. If the reaction in (d) actually produced 8.79g of ammonia, what is the percent yield?
8.79 g
x100% = 89.1%
9.87 g
VIII. Solution Definitions
1. What is the relationship between a solute, solvent, and a solution?
A solute is added to a liquid solvent to form the solution.
2. Give an example of a(n):
a. gas solution - air
b. gas-in-liquid solution – CO2 in water (soda), O2 in water
c. liquid-in-liquid solution – antifreeze, food coloring in water, alcohol & water
d. solid-in-liquid solution – sugar in water, salt in water
e. solid solution – any alloy (brass, bronze, steel)
3. Describe how antifreeze works.
By mixing ethylene glycol and water, it raises the boiling point higher than 100oC and
lowers the freezing point below 0oC so that the mixture remains a liquid over a greater range of
temperatures.
4. Give 5 properties associated with solutions.
Solutions are homogenous, they can’t be filtered , they don’t settle, they are all in one
phase, and liquid solutions are clear and transparent.
5. Define the following:
a. saturated solution – holding as much solute as possible at that temperature
b. unsaturated solution – could hold more solute if needed at that temperature
c. supersaturated solution – is holding more solute than it should at that temperature.
Unstable and formed by heating and cooling a saturated solution.
6. Answer the following questions about the solubility of a solute:
a. Why won’t oil and water dissolve in each other?
“Like dissolves Like”. Water is polar, and oil is nonpolar in molecular structure, so
they are not able to mix with each other.
b. What happens to the solubility of sugar as temperature increases?
As the temperature of the solvent increases, sugar becomes more soluble. This is the
case for most solid solutes (see the graph on the next page) such as NaCl, KClO3, KNO3, etc.
c. What happens to the solubility of oxygen gas (O2) as temperature increases?
As the temperature of the solvent increases, oxygen becomes less soluble. This is the
case for all gas solutes (see the graph on the next page) such as NH3, HCl, SO2, etc.
d. What happens to the solubility of oxygen gas (O2) as pressure increases?
As pressure increases, gas solutes, such as oxygen, become more soluble. When soda
is bottled, it is done at high pressures to force more CO2 gas to dissolve. When the bottle is
opened, the pressure is released, and the CO2 comes out of solution as bubbles.
IX. Solution Problems
1. Use the solubility chart below to answer the following:
a. Put in order from least to most soluble at 10oC: NH3, KClO3, NaCl, KNO3
KClO3 , KNO3 , NaCl , NH3
b. Put the above compounds in order from least to most soluble at 90oC.
NH3 , NaCl , KClO3 , KNO3
c. What is the solubility of NH4Cl at 60oC?
55g NH4Cl / 10θg H2O
d. If you added 50.0g of NH4Cl to 10θ g of water at 60oC, would the solution be saturated,
unsaturated, or supersaturated? If it is saturated, how much is left over?
solubility: 55g NH4Cl / 10θg H2O unsaturated
(could add 5 more grams of solute)
2. What is the molarity of a solution in which you dissolve 0.430 moles of a solute
so
in 1.33 L of
water?
Molarity =
moles solute 0.430mol
=
= 0.323M
1
.
33
L
liters solution
3. What is the molarity of a solution in which you dissolve 10.0g of sodium bicarbonate (NaHCO3) in
0.600 L of water?
10.0 g NaHCO 3 ∗
1mol NaHCO 3 0.119mol NaHCO 3
=
= 0.198M
0.600L
84 g NaHCO 3
4.. If you begin with 100.0 mL of a 3.00 M HCl solution and yyou
ou dilute it with water to 50θ
50 mL, what
will the new concentration be?
(3.00 M )(100.0mL ) = ( M )(500 mL ) → M =
(3.00 M )(100.0mL )
= 0.600 M
500mL
5. What volume of concentrated (12 M) HCl do you need to make 50θ mL of a 1.00 M solution?
(1.00 M )(500mL) = (12 M )V → V =
(1.00 M )(500mL)
= 42mL
12 M
6. How many mL of water are needed to dilute 5.0 mL of concentrated HCl (12 M) into a 3.0 M
solution?
(12 M )(5.0mL) = (3.0 M )V → V =
(12 M )(5.0mL)
= 20mL
3 .0 M
7. How many grams of sodium chloride (NaCl) are needed to make 50θ mL of a 2.00 M solution?
500mL = 0.500 L ∗
2.00mol NaCl
58.5 g NaCl
= 1.00mol NaCl ∗
= 58.5 g NaCl
1L
1mol NaCl
8. How many grams of lead nitrate ( Pb(NO3)2 ) are needed to make 1.00 L of a 0.0100 M solution?
1.00 L ∗
0.0100mol Pb(NO 3 ) 2
331g Pb(NO 3 ) 2
= 0.0100mol Pb(NO 3 ) 2 ∗
= 3.31g Pb(NO 3 ) 2
1L
1mol Pb(NO 3 ) 2
X. Kinetics:
• collision theory: collision effectiveness and collision frequency
• 4 factors that affect reaction rates: nature of reactants, concentration, temperature, catalysts
• potential energy diagram (see CK I HW), activation energy, activated complex, enthalpy of
reaction
A. Energy Diagram. Use the diagram shown below:
Potential Energy
2
3
1
Reaction Coordinate
Points 1 & 3 1. The difference of what two points represents the enthalpy or heat of this
reaction?
Endothermic 2. Is the reaction endothermic or exothermic?
Points 1 & 2 3. The difference of what two points indicates the activation energy for the
forward reaction?
Number 3 4. Which number indicates the products?
Point 2 only 5. Which points would have their values change when a catalyst is added?
Activated Complex 6. What is the term for the “stuff” described at point #2?
B. For each of the following, circle whether the given factor will increase or decrease the rate of a
reaction. Then, using Kinetic Theory, explain why your answer is correct:
1. increasing the concentration of the reactants
Increase
Decrease
As concentration increases, the particles are closer together & collide more often
2. increasing the temperature
Increase
Decrease
As temperature increases, the particles are moving faster & collide more often
XI. Thermodynamics
• enthalpy (ΔH), heat of formation, exothermic, endothermic
1) For each of the following, calculate ∆H. Also state whether they are endothermic or exothermic
a)
C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(l)
∆H = 3(-394) + 4(-286) – (-103.8) – 5(0) = -2222 kJ, exothermic
b)
2 Al2O3(s) 4 Al(s) + 3 O2(g)
∆H = 4(0) + 3(0) – 2(-1676) = +3352 kJ, endothermic
c)
3 Al(s) + 3 NH4ClO4(s) Al2O3(s) + AlCl3(s) + 3 NO(g) + 6 H2O(g)
∆H = -1676 + -704 + 3(90.4) + 6(-242) – 3(0) – 3(-295) = -2676 kJ, exothermic
Substance
Al(s)
AlCl3(s)
Al2O3(s)
CH4(g)
C3H8(g)
C6H6(l)
C2H5OH(l)
CO(g)
CO2(g)
CuO(s)
∆Hfo (kJ/mol)
0
-704
-1676
-75.0
-103.8
+49.04
-277
-110
-394
-155
So (J/K)
28.3
111
51.0
186.2
259.9
124.5
161.0
197.9
213.6
43.5
Substance
H2O(g)
H2O(l)
NH3(g)
NH4ClO4(aq)
NO(g)
NO2(g)
N2O5(g)
O2(g)
SO2(g)
SiO2(s)
∆Hfo (kJ/mol)
-242
-286
-46.0
-295
+90.4
+33.1
+11.3
0
-297
-511
So (J/K)
188.7
69.9
192.5
186
210.6
240.5
356.0
205.0
248.5
41.8
XII. Acid and Bases
1. Define the following:
• Ionic Compound – a compound made of a metal and nonmetal
• Molecular Compound – a compound made of 2 nonmetals
• Acid – a molecular compound that starts with hydrogen (H-A)
• Base – an ionic compound that ends with hydroxide (MOH)
• Salt – an ionic compound that is not a base
• Electrolyte – a substance that dissolves in water to produce ions; conducts electricity
• Neutralization – a reaction in which an acid reacts with a base to make salt and water
• Indicator – a substance whose color is affected by the pH
• Buffer – a solution that can resist changes in pH
• Titration – the process of finding the concentration of an unknown using a known solution
o Standard Solution – the solution of known concentration
o Unknown Solution – the solution whose solution is being tested
2. What are the 5 properties of acids and bases?
Acids
Bases
1
Electrolytes that produce
Electrolytes that produce hydroxide ions
+
hydronium ions (H3O )
(OH-)
2
Neutralize bases
Neutralize acids
3
Turn indicators colors
Turn indicators colors
4
Taste sour
Taste bitter and are slippery
5
React with active metals to
produce hydrogen gas (H2)
Emulsify fats
3. Draw the Lewis Structures for the following substances. For each:
• Give the name of the substance
• Label it as an acid, base, salt, or neither
a. H2S
hydrosulfuric acid
acid
b. NaOH
sodium hydroxide
base
c. NaCl
sodium chloride
salt
d. SCl2
sulfur dichloride
neither
4. Rank the following acids from weakest to strongest:
H2SO4, HF, H3PO4, HCl
HF, H3PO4, H2SO4, HCl
5. Name the following compounds, and label as an acid (A), base (B), salt (S), or neither (N):
(S) calcium chloride
a. CaCl2
(B) lithium hydroxide
d. LiOH
(A) nitric acid
b. HNO3
(S) lithium oxide
e. Li2O
(B) magnesium hydroxide
c. Mg(OH)2
(N) carbon dioxide
f. CO2
6. Give the formulas for the following compounds, and label as an acid (A), base (B), salt (S), or
neither (N):
(S) BaBr2
a. barium bromide
(B) Al(OH)3
d. aluminum hydroxide
(A) HBr
b. hydrobromic acid
(N) N2O
e. dinitrogen monoxide
(B) NaOH
c. sodium hydroxide
(A) H2SO4
f. sulfuric acid
7. Give the products for the following neutralization reactions. Label the acid, base, salt, and
water.
a. _____ HBr(aq) + _____ NaOH(aq) NaBr + HOH
b.
2 HCl(aq) + _____ Mg(OH)2(aq) MgCl2 + 2 HOH
8. Given the information below, label the solutions as acidic, basic, or neutral. What color would
each show with pH paper?
pH
a) 3.8
b) 5.8
c) 7.8
acidic, basic,
neutral
Acidic
Acidic
Basic
color
pH
Red
Orange
Green
d) 7.0
e) 13.4
f) 7.1
acidic, basic,
neutral
Neutral
Basic
Acidic
color
Yellow/green
Blue
Yellow/green
9. Using the information in #8, answer the following questions:
a. Which is most acidic? (a)
b. Which is most basic? (e)
least acidic? (e)
least basic? (a)
c. (a) is 100 times less acidic than (b) and 10,000 times less
acidic than (c).
10. Look at the data in the table below and answer the questions:
Substance
initial pH
pH after 1 drop HCl
pH after 2 drops NaOH
A
10.7
10.2
11.2
B
4.4
4.3
4.5
C
7.0
1.9
12.4
a. Using your indicator table in the notes, give the color that each of the substances will show
before adding any acid or base:
Substance
initial pH
acid, base, or
neutral?
color in methyl
red
color in
phenolphthalein
A
10.7
Base
Yellow
Magenta
B
4.4
Acid
Red
Colorless
C
7.0
neutral
yellow
Colorless
b. Look at the 3rd column of the top table. What is the Lewis Structure for HCl? Is it an acid or a
base? When you add HCl, what happens to the pH?
Cl
H
Acid
The pH decreases
c. Look at the 4th column of the top table. What is the Lewis Structure for NaOH? Is it an acid or a
base? When you add NaOH, what happens to the pH?
+1
Na
O
H
Base
The pH increases
d. Which solution is the best buffer: A, B, or C? Explain your answer.
“B” is the best buffer because the pH changed very little when acid or base were added
11. If you titrate some vinegar (weak acid) of unknown concentration with a standard 0.800 M
solution of NaOH, what is the concentration of vinegar if the titration required:
a. 5.0 mL of vinegar and 7.6 mL of NaOH
(Ma)(5.0 mL) = (0.800M)(7.6 mL)
Ma = 1.2 M
d. exactly 5θ drops of vinegar and 31 drops of NaOH
(Ma)(50 drops) = (0.800M)(31 drops)
Ma = 0.50 M (0.496M)
XIII. Carbon Chemistry
Symbol
Atomic #
C
Carbon
Protons Electrons
6
6
Valence
Electrons
6
Lewis
Structure
4
C
How many bonds does carbon “like” to form? 4 bonds
Give the prefix for the following number of carbons:
MethEthPropBut-
One
Two
Three
Four
PentaHexaHeptaOcta-
Five
Six
Seven
Eight
Nine
Ten
NonaDeca-
Define the following:
• Allotrope (give examples for carbon) – different form of the same element; for carbon,
examples are amorphous, diamond, graphite, buckminsterfullerene
• Hydrocarbon – a compound which contains only the elements carbon and hydrogen
• Saturated hydrocarbon (example) – a hydrocarbon that has only single bonds: CH4
• Unsaturated hydrocarbon (example) – a hydrocarbon with at least one multiple bond: C2H4
• Alkane – a saturated hydrocarbon
• Alkene – an unsaturated hydrocarbon with a double bond
• Alkyne – an unsaturated hydrocarbon with a triple bond
• Isomer – a different compound with the same molecular formula
• Polymer (give some examples) – a long chain of hundreds or thousands of repeating units
held by covalent bonds (proteins, fats, plastics)
Draw 3 different isomers for C5H12
H
H
H
H
H
C
C
C
C
H
H
H
C
H
H
H
H
H
H
H
C
C
C
C
C
H
H
H
H
H
H
H
H
H
C H
H
H
H
H
H
C
C
H
H
C
H
C H
H
H
1. Give the formula for the hydrocarbon on d-f.
2. State if there are single, double or triple bonds.
3. State if it is an alkane, alkene, or alkyne.
4. State if the hydrocarbon is saturated or unsaturated
5. Name the compound.
a. C3H8
H
H
H
H
C
C
C
H
H
H
10 Singles
H
d.
0 Doubles 0 Triples
CH
C
C
C
H
H
H
H
H
Formula
0 Doubles 0 Triples
----------------------------------------------------------------------------------
CH3
CH2
H
H
H
H
H
H
C
C
C
C
C
H
H
H
H
H
H
1 Doubles 0 Triples
C5H12
pentene Product's Name
----------------------------------------------------------------------------------
c. C8H18
H
H
H
H
H
H
H
H
C
C
C
C
C
C
C
C
H
H
H
H
H
H
H
H
0 Doubles 0 Triples
Octane Product's Name
Formula
16 Singles
0 Doubles 0 Triples
Pentane Product's Name
----------------------------------------------------------------------------------
H
H
C
C
H
f.
C2 H 2
25 Singles
C
Butane Product's Name
e.
H
H
13 Singles
b. C5H10
13 Singles
H
C4H10
Propane Product's Name
CH
H
H
----------------------------------------------------------------------------------
CH3
H
Formula
2 Singles
0 Doubles 1 Triples
Ethyne Product's Name