SCH4C-U1W4D2
Unit 1: Review
Topic Summary of unit 1
- What is matter?
o Chemical and physical properties
 Chemical (3)
 Physical (lots)
o Chemical and physical changes
 Evidence of a chemical change
o Classification of matter
o Observation vs inference
- Early Atomic Models
- Electromagnetic spectrum
- The periodic table – families, solids, liquids, gases
- Bohr – Rutherford model.
- Atoms
- Ions
- Lewis structures
- Ionic compounds
o Formation
o Properties
o Nomenclature
 Binary, Multivalent, Polyatomic
- Covalent bonds
o Formation
o Coordinate covalent
o Nomenclature
o Drawing Lewis structures of molecules
- Intramolecular and Intermolecular forces
o Electronegativity
o Polar bonds
- Balancing equations
- Types of reactions
o 5 types
o Aqueous solution reactions.
 Reactivity series
 Solubility table
Date:
SCH4C-U1W4D2
Unit 1 Practice Problems
Chemical and physical changes
1. An egg is cooked
2. Ice melts
3. Ice is smashed
4. Salt is dissolved in water
5. Alcohol is mixed with water
6. Banana’s start to rot
7. Methane is oxidized
8. Electricity is used to split H2O into H2 and O2
9. A diamond scratches glass
10. A candle burns
Classify the following examples as either a: Compound, element, homogenous solution,
heterogeneous solution.
1. A salad
2. Tea
3. Water
4. Plastic ruler
5. Oxygen gas
6. Carbon dioxide gas
7. Pizza
8. Wood
9. Salt water
10. Salt
Early atomic models
- Who redeveloped the raisin bun model
- Who said that all matter was made up of 4 elements
- What is the particle theory of matter?
Electromagnetic spectrum
- What is the difference between line spectra and a continuous spectrum?
- How can spectroscopy be used to identify elements?
- How does the Bohr model explain line spectra?
Bohr – Rutherford diagrams – Draw the following ions and atoms.
- Na
- Br
- B
- Cl- Li+
- P2-
-
FC
He
Lewis structures –Draw the following ions and atoms
- Cu2+
- P
- Zn
- Cl- Al
- P2-
-
FC
I-
Ionic Compounds
1. Draw the Lewis structures of the reactants and the products of the following compounds.
Zinc + Phosphorus  Zinc phosphide
Copper + Sulfate  copper (II) sulfate
Al + P  AlP
Fe + O  Fe2O3
Rb + Se  Rb2Se
Co + Cl  CoCl2
2. Write the chemical formulas for the following chemicals
Sodium hydrogen sulfate
Potassium nitrate
Sodium hydroxide
Aluminum oxide
Carbon dioxide
Potassium hydroxide
Sodium thoisulfate
Mercury (II) nitrite
Sodium hypochlorite
Aluminum perchlorate
Mercury (II) nitrite
Copper (I) sulfate
Lithium hydroxide
Nickel (III) phosphate
Silver carbonate
Magnesium oxide
3.
Write the name for the following formulas
NaCl
Pb(C2H3O2)2
NH4OCl
Sn(BrO3)4
Sb2O3
Zn(IO3)2
Fe(NO4)2
Ca(OH)2
Ba(C2H3O2)2
AuCl3
MgS
NiSO4
AgBrO3
LiClO4
CaHPO4
KI
Covalent bonding
1. Draw Lewis structures of the following molecules and indicate polar bonds, polar
molecules and coordinate covalent bonds. (Hint, use the have need rule)
NH4+
CO2
H2O
N2O2
O3
O2
C2H6
NO3NaOH
HCO3-
Balancing and types of reactions
1. Classify each of the following reactions as combustion, synthesis, decomposition, single
displacement or double displacement. Balance each equation.
a. S8 + O2  SO2
b. HBr + NaOH  NaBr + H2O
c. N2 + H2  NH3
d. PtCl4  Pt + Cl2
e. MgO + Si  Mg + SiO2
f. Na2S + HCl  NaCl + H2S
2. Classify the type of reaction, balance the equation, predict the products and the states of
the products.
a. Al(s) + AgNO3(aq) 
b. Cl2(g) + NaBr(aq)
c. Zn(s) + H2SO4(aq)
d. Aqueous silver nitrate + aqueous magnesium chloride
e. Na2C2O4(aq) + CaCl2(aq)
f. Sodium + water
g. Potassium hydroxide + iron (III) chloride
3. Indicate which of the following reactions will proceed. For each reaction that proceeds,
predict the products and write a balanced equation. Write NR for reactions that do not
proceed.
a. Li(s) + H2O(l) 
b. K(s) + H2O(l) 
c. Cu(s) + AgNO3(aq) 
d. Fe(s) + NaCl(aq) 
e. Mg(s) + Ca(NO3)2(aq) 
f. Al(s) + HCl(aq) 
g. Al(s) + H2O(aq) 
h. Ni(s) + HCl(aq) 
i. (NH4)2CO3(s) + CaCl2(aq) 
j. Ca(NO3)2(aq) + Na2SO4(aq) 
k. I2(s) + HCl(aq) 
l. Sn(s) + H2O(aq) 
For more practice
Page 71 # 1, 4, 5, 6, 10 – 20, 26, 27.