SCH4U
Unit 1 – Organic Chemistry
Unit Preparation
Name: _______________________________
Chemical Bonds
1. What is the difference (in terms of ∆EN) between ionic bonds, covalent bonds, and polar
covalent bonds?
2. Determine the ∆EN for the following:
a. HCl
b. NaF
c. MgO
Representing Molecules
1. Provide both the classical and stock names for the following compounds:
a.
b.
c.
d.
e.
f.
TiO2
Fe(OH)3
CuO
Pb3(PO4)4
SnCl2
CoCl2
2. Write the correct chemical formula for each of the following compounds:
a.
b.
c.
d.
e.
f.
Zinc perchlorate
Mercury (II) nitride
Stannous fluoride
Ferric hydroxide
Lead (IV) phosphate
Nickel (III) sulfite
Balancing Equations
1. Balance each of the following equations:
 ___ NaCl(aq )  ___ NaClO(aq)  ___ H 2O(l )
a. ___ NaOH(aq )  ___ Cl2(g ) 
 ___ Al2 (SO4 ) 3(aq )  ___ HNO3(aq)
b. ___ Al(NO3 ) 3(aq)  ___H 2SO4(aq) 


c.
___KI(aq)  ___ MnO2(s)  ___ H2SO4(aq) 
 ___K2SO4(aq)  ___ MnSO4(aq)  ___ H2O(l )  I2(s
 ___ CO2(g )  ___ H 2O(g )
d. ___ C6 H 6(l )  ___ O2(g ) 

Ionic Equations
1. Aqueous solutions of several pairs of ionic solids are prepared and then mixed together.
For each pair listed below, write the following:
i. The balanced, total ionic equation
ii. The net ionic reaction, if a precipitate forms
iii. Any spectator ions
a. Lead (II) nitrate and zinc iodide
b. Sodium hydroxide and iron (III) nitrate
Mole and Concentration Calculations
1. How many moles of lead (IV) carbonate have a mass of 2.56 x 105 g?
2. A 6.00g sample is 76.5% sodium hydroxide. How many atoms of sodium are in this
sample?
3. A salt solution has a concentration of 1.00mol/L. What volume of this solution is needed to
prepare 2.00L of a solution that has a concentration of 0.475mol/L?
4. A sample of lead (II) nitrate, with a mass of 0.00372g, is completely dissolved in 250.0mL
of water. Assume that no change in volume occurs. Calculate the following concentrations.
a. The concentration of the solution, expressed in mol/L.
b. The concentration of Pb2+, expressed in ppm.
c. The concentration of the solution, expressed as a m/m percent.
Stoichiometric Calculations
1. 40.00mL of 0.0256mol/L gold (III) chloride is treated with 85.00mL of 0.105 mol/L
potassium iodide.
AuCl3(aq)  3KI(aq ) 
 AuI(s)  3KCl(aq )  I2(aq)
a. What is the theoretical yield of AuI(s) produced?

2. When 15.0g of copper and 4.83g of sulfur are heated, a 13.7g mass of copper (I) sulfide is
produced.
2Cu(s)  S(g ) 
 Cu2 S(s)
a. What is the percentage yield of Cu2S?
