Review
Chapter #1
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Chapter #2
Matter:
elements and compounds
Definitions etc
organization of elements Periodic table
Periodic Law
Modern Periodic Table, Families etc., group, period
Early theories of atomic structure, Dalton, Thomson, Rutherford etc
Gold Foil Experiment, what it showed, explanation for structure,
Atomic mass, Atomic number, electrons, neutrons and protons
Modern atomic theory Bohr, line spectrums, excited and ground states
Trends in Periodic table, Atomic radius, Ionic Radius, First and Second Ionization Energies, Electronegativities, Electron
Affinity
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Bonding
Classifying compounds
Ionic bonding
transfer of electrons stable octet
Properties of ionic compounds
Representing ionic bonds, electron dot diagram, Lewis diagrams
Covalent Bonding
sharing of electrons
Stable octet
Coordinate Covalent bonds
Electro negativity Polar bonds and Polar molecules
Intermolecular forces
Van der Waals forces ( dipole - dipole and London forces) hydrogen bonding
nomenclature, ionic , molecular, polyatomic compounds, acids
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Chemical Reactions.
Chemical and physical changes
Kinetic molecular theory and chemical changes, collision -reaction theory
Word, chemical equations,
Balanced chemical equations
Types of reactions, Combustion, Synthesis, Decomposition, Single/double displacement reactions
Solubility and double displacement reactions, Solute and solvent, Precipitates,
Predicting precipitates, solubility chart
Chapter #3
Chapter #4
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Chapter #5
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Chapter #6
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Chapter #7
Law of Definite Proportions
The mole and molar mass, Avogadro’s number.
Moles ( n) = m( mass) / M ( molar mass)
Percent Composition, Empirical and Molecular formulas
Quantities in Chemical Reactions
Balancing Equations, Mole ratios Stoichiometry,
Limiting and excess reactants, % yield
mass==> moles ==> Mole Ratio ==> moles ==> mass
Solutions
Defining solutions, homogeneous and heterogeneous mixtures
properties of solutions, intra molecular intermolecular forces
Ionic compounds in water, dissociation
Concentrations of solutions, c = n/v
Solution preparation, dilutions and prep from solid
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Solubility
Saturated solutions etc,, solubility
Solubility categories
Reactions in solution, net ionic equations
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Acids and bases
Properties., strong and weak acids and bases
pH of solutions, measuring pH
Acid base titrations,
Chapter #8
Chapter #9
Chapter #10
Gases
States of matter and KMT
Gas Laws, Charles, Boyles, Combined, Ideal Gas law
More Gas laws
Gas stoichiometry.
Review Worksheet #1
Chapter #1
Nature of matter
There are not many mathematical concepts within this chapter.
Work through the concepts for full understanding.
Matter, Atoms,Theories, periodic table, trends etc
Chapter #2
Classifying compounds, properties etc. Ionic and Covalent
Covalent and Ionic bonding. Basic concepts
Electro negativity and polar bonds and molecules
Nomenclature
Names:
KBrO3
SnO
Li2SO4
Ca3N2
HgCO3
Ag2S04
CoCl2
Al2(SO4)3
CuSO4*5H2O
NH4OH
KI
Ba(C2H3O2)2
H2S
HNO3
N2O4
CH4
NaOH
SbCl5
FeO
ZnCO3
H2O
H2O2
K2SO4
Sodium Iodate
Zinc oxide
Tin (IV) sulphate
ammonium hydroxide
Iron ( III) carbonate
carbon disulphide
magnesium nitrate
barium chlorate
ammonia
phosphoric acid
lead (II) acetate
phosphorous pentabromide
dinitrogen oxide
barium carbonate
Hydrochloric acid
Potassium hydroxide
vinegar
Tin (II ) oxide
Lithium chlorate
Aluminum sulphide
WORKSHEET #2
Chapter #3 Chemical Reactions
Mechanism for reactions and change, KMT and collision theory, evidence
Representing change, word and chemical formula equations
Balanced chemical equations
Balance the following equations:
Cu +
HNO3 ===>
MnO2
KClO3 ====>
SO2
KCl
H2SO4
Ca3(PO4)2
C4H10
+ HCl ===>
+ H2S ===>
NaCl +
+ SiO2
+ O2
Cu(NO3)2 + H2O
+
H2 O +
MnCl2
+ NO
+ H2O
+ Cl2
O2
S
+ MnO2 ===>
Na2SO4
+ MnSO4
+ C ====>
CaSiO3
+ CO
====>
CO2
+
+
H2 O
+ Cl2
+ P4
H2 O
Butane burns in the presence of oxygen to produce two well known compounds.
Write out balanced chemical equation for this reaction
Types of reactions.
Be able to examine various reactions and classify as to a name of type.
Solubility:
Silver nitrate and Sodium Chloride solutions were mixed together.
Write out the balanced chemical equation.
Write out the total ionic equation
Write out the net ionic equation for this reaction.
Indicate whether or not a precipitate was produced and its identity.
WORKSHEET #3
Chapter 4&5 & 9&10
Stoichiometry and gas laws
Law of definite proportions
The mole and molar mass Avagadros number
Conversions with moles and molar mass and mass. Percentage composition
Empirical and molecular formulas
Percent Yield.
Mole Ratios===> Mass==> moles===Mole Ratio==> Moles===> Mass
Limiting and excess reactants, conduct stoichiometric analysis to determine
#1
a)
b)
C)
Zn ( s)
+ HCl
===>
ZnCl2 ( aq) + H2 (g)
What mass of zinc is needed to produce 20.0 L of hydrogen gas at STP?
what mass of zinc is needed to produce 20.0 g of hydrogen?
what mass of zinc is needed to react with 100.0 g of hydrochloric acid?
#2
a)
b)
c)
d)
Cu(s) + 4HNO3 ( aq) ===>
Cu(NO3)2 (aq) + 2NO2( g) + 2H2O (l)
What mass of copper is required to produce 100 L of nitrogen dioxide at 25 degrees C and
105 kPa>
What mass of copper is required to produce 100 g of copper (II) nitrate?
what mass of nitric acid will react with 100 g of copper?
what mass of water is produced at the same time as 100 g of nitrogen dioxide?
#3
a)
b)
c)
2S(s) + 3 O2 ( g) + 2H2O ( l) ===> 2 H2SO4 (l)
What mass of sulphuric acid can be manufactured using 100 L of oxygen at STP?
what mass of sulphur is needed to produce 1.o Kg of sulphuric acid?
what volume of oxygen at 27 degrees c and 110 kPa will react with 64.o g of sulphur?
#4
If a 1.00 L balloon at 101.3 kPa is subjected to a new pressure of 225 kPa, what will its new
volume be?
To what temperature must 1.00 L of gas at 0degrees C be heated to increase its volume to
2.4 L
1.00L of a gas at 25 degrees Celsius and 110 kPa has a mass of 2.40 g. Calculate the molar
mass of this gas.
Calculate the volume of
a)
24g of CH4 at STP
b)
20.0 g of NH3 at 25 degrees C and 98 kPa
#5
#6
#7
#8
Calculate the mass of
a)
26.5L of CH4 at 25 degrees C and 200 kPa
b)
1.00 L of air ( molar mass = 28.8 g/mol) at STP
#9
3.5 L of a gas at 20 degrees C and 118.4 kPa has a mass of 6.0 g . What would be the mass
of 2.6 L of the same gas at 0 degrees C and 104 kPa
WORKSHEET #4
Chapters 6,7 & 8 Solutions, Solubility and Acids & Bases
Solutions, definitions, properties, types, Explaining mixtures, ionic compounds in water,
water the universal solvent, Concentrations, water quality, prep of solutions, dilutions
Solubility, effects of temp. precipitates more net ionic equations stoichiometry with
solutions. Acids and bases properties, strong and weak pH and calcs. Neutralizations
titration
#1a)
Stock nitric acid was analyzed and found to have a density of 1.41 g/mL.
molar concentration of this solution?
Convert g - moles
Convert mL ==> L
#1b)
how much of this stock solution is needed to produce 2.00 L of 0.25 mol/L nitric acid
solution?
#2
Write equations for the dissociation or ionization for the following compounds.
KCl
==>
H2SO4
==>
Ba(NO3)2
==>
Ca3(PO4)2
==>
#3
Write net ionic equations for the formation of precipitates produced when the following
pairs of solutions react.
sodium hydroxide and aluminum sulphate
calcium nitrate and potassium carbonate
lithium sulphide and iron (III) nitrate
a)
b)
c)
#4
A)
B)
C)
#5
What is the
In a titration experiment it is found that 25.00 mL of a base solution is neutralized by 15.6
ml of 0.10 mol/l HCl solution.
how many moles of acid are used?
how many moles of base are used?
if , in addition , it is known that the 25 ml sample of base contains 0.05 g of base , what is
the molar mass of the base?
a)
b)
Describe in reasonable detail showing your calculations, how you would prepare the
following solutions.
1.00L of 0.05 mol/L KOH starting with pure KOH solid
0.500 L of 0.25 mol/L HCl starting with 12.0 mol/l HCl
#6
a)
b)
c)
Complete the following neutralization equations
NaOH + HCl ==>
H2SO4 + KOH ===>
HNO3
+ Ba(OH)2 ===>
WORKSHEET #5
#7
Chapter 6-8 continued
What mass of KOH is needed to neutralize100 ml of 0.20 mol/L HCl?
#8
What volume of 0.25 mol/L HCl is needed to neutralize 30.0 ml of 0.1 mol/L Ca(OH)2
#9
a)
b)
c)
25 ml of 0.20 mol/L KOH was titrated against various acid solutions. The volumes of acid
solutions used are listed below. Find the molar concentrations of each acid solution
10.0 ml H2SO4
20.0 mL of H3PO4
15 mL of HCl
#10
A)
B)
C)
What is the molar concentration of each of the following?
20.0 g of KOH in 500 ml
25.0 g of NaCl in 300 ml
50 ml of 12 mol/L HCl added to 350 ml water
#11
A)
B)
How many grams of solute in :
50 mL of 0.20 mol/L KCl
100 ml of 0.002 mol/L CH3COOH
#12
An acid solution contains 0.50 g of acid in every 25 ml of solution. 120 ml of 0.25 mol/L
KOH is needed to neutralize 25 ml of the acid solution. Assume 1:1 ratio of acid to base
the molar concentration of the acid solution
the moles of acid in 25 ml of the acid solution
the molar mass of the acid
a)
b)
c)
#13
On day in hallowed halls of the Wood, a piece of evidence to a crime appeared. It was a
gigantic pellet of sodium hydroxide. The whole solution to the crime depended upon the
mass of the pellet. Sadly the fairy balance beam wasn’t working , but the fairy Godmother
remembered her chemistry and knew she could find the mass of the pellet by conducting
various laboratory experiments. She found that when she added 18356 mL of 0.100 mol
/L HCl to a solution made by dissolving the pellet in a sample of water, the indicator
phenolpthalein changed from pink to clear. What was the mass of the pellet?
Answers
KBrO3
SnO
Li2SO4
Ca3N2
HgCO3
Ag2S04
CoCl2
Al2(SO4)3
CuSO4*5H2O
Potassium Bromate
Tin (II) oxide
Lithium Sulphate
Calcium nitride
Mercury (II) carbonate
Silver Sulphate
Cobalt (II) chloride
Aluminum Sulphate
Copper (II) sulphate penta
hydrate
NH4OH
KI
Ba(C2H3O2)2
H2S
HNO3
N2O4
CH4
NaOH
SbCl5
FeO
ZnCO3
H2O
H2O2
K2SO4
Sodium Iodate
Zinc oxide
Tin (IV) sulphate
ammonium hydroxide
Iron ( III) carbonate
carbon disulphide
magnesium nitrate
barium chlorate
ammonia
phosphoric acid
lead (II) acetate
phosphorous pentabromide
dinitrogen oxide
barium carbonate
Hydrochloric acid
Potassium hydroxide
vinegar
Tin (II ) oxide
Lithium chlorate
Aluminum sulphide
Ammonium Hydroxide
Potassium Iodide
Barium Acetate
Hydrogen Sulphide
Nitric Acid
dinitrogen tetroxide
Methane
Sodium hydroxide
Antimony (V) chloride
Iron (II) oxide
Zinc Carbonate
dihydrogen oxide
dihydrogen dioxide or
Hydrogen peroxide
Potassium sulphate
Na IO3
ZnO
Sn(SO4)2
NH4OH
Fe2(CO3)3
CS2
Mg(NO3)2
Ba(CLO3)2
NH3
H3PO4
Pb(C2H3O2)2
PBr5
N2O
BaCO3
HCl
KOH
HC2H3O2
SnO
LiClO3
Al2S3
Worksheet #2 Chapter 3 chemical Reactions
3Cu + 8 HNO3 ===> 3 Cu(NO3)2 + 4H2O + 2NO
MnO2
+ 4HCl ===>
MnCl2 + 2 H2O + Cl2
2 KClO3 ====> 2 KCl
+ 3 O2
SO2 + 2 H2S ===> 2 H2O + 3 S
2 NaCl + 2 H2SO4 + MnO2 ===> Na2SO4 + MnSO4
+
2 H2O + Cl2
2 Ca3(PO4)2 + 6 SiO2 + 10 C ====> 6 CaSiO3 +
10CO
+ P4
AgNO3 + NaCl ==>
AgCl
+
Ag+ + NO3- + Na + + Cl- ===> AgCl
Ag+
+
Cl- ===> AgCl
Precipitate is Silver chloride.
NaNO3
+ Na + + NO3 -
Worksheet #3 chapters 4,59,10
#1a)
58.1 g
B) 646.5 g
C) 88.8 g
#2a) 134.62 g
B) 33.86 g
C) 396.9 g D) = 39.06g
#3a) 294g
B) 326.5 g
C) 67.9 L
#4 = 0.45 L
#5= 655.2 K or 928.2 C
#6
#7 a)
33.6 L
B)
29.82 L
#8a)
34.24 g
B) 1.29 g
#9 Molar mass = 35.3 g/mol
Mass = 4.24 g
#1a)
#2a)
Worksheet #4
16 mol/L
B)
K+
+ Cl-
Chapter 6,7,8
0.031 L
b)
2H+
+ SO4 -2
+2
c)
Ba
+
2 NO3 -1
d)
3 Ca+2
+ 2 PO4 -3
#3
Al +3 + 3OH-1 ==> Al(OH)3 (s)
Ca +2 + CO3 -2 ==> CaCO3 (s)
2Fe+3 + 3 S-2 ==> Fe2S3(s)
#4a) 0.00156
B) 0.00156
#6a)NaCl
+ H2O
b)H2O + K2SO4
c)H2O + Ba(NO3)2
C) 32.05 g/mol
WORKSHEET #5
#7=1.12 g
#8
=24 ml
#9a) 0.25 mol/L b) 0.08 mol/L c) 0.33 mol/L
#10a) 0.72 mol/L b) 1.4 mol/L c) 1.5 mol/L
#11a) = 0.745 g
B) 0.012g
#12a) 1.2 mol/L
b) n = 0.03
c) 16.7 g/mol