PART B [4 marks] [6 marks] UNIT 1
: Short Answers & Calculations (45 marks)
: STRUCTURE OF MATTER
1. Write the electron configurations for each element:
2. Use VSEPR Theory to draw the 3D geometric structure of each molecule and provide the name of the resulting shape.
a) BrI5 b) IF3
UNIT 2: ORGANIC CHEMISTRY
3. Draw the structure for the following organic molecules:
a) 1-chloro-3-ethylcyclohexene b) 2-bromopentanal
c) 2,4-dimethylpentan-2-ol d) 1-chloropentan-3-one
4. Write the complete structural formula equation for each of the reactions below. Write the IUPAC name for each product.
a) Addition Reaction (Hydration): addition of water to pent-2-ene
b) Esterification Reaction: propan-1-ol and butanoic acid
UNIT 3: ENERGY CHANGES
5. Use Hess's Law to calculate the heat of formation of C2H4 from the following data.
Target Equation: C(s) + H2(g) → C2H4(g)
C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) ∆H = -1410 kJ/mol
C(s) + O2(g) → CO2(g) ∆H = -393 kJ/mol
H2(g) + 1/2 O2(g) → H2O(l) ∆H = -286 kJ/mol
6. Calculate the mass of carbon in C(s) + O2(g) → CO2(g) that would have to be burned to heat 30.0 mL of water from 20.0 °C to 65.0 °C. The ∆H for this reaction is -393 kJ/mol (Specific heat capacity of water is 4.18 J/g°C)
UNIT 4: EQUILIBRIUM
7. Consider the following reaction which has a K = 0.50
SO3(g) + NO(g) → NO2(g) + SO2(g)
If 0.60 mol of SO3 and 0.60 mol of NO were placed in a 3.0 L container and
allowed to react, what would be the equilibrium concentration of each gas?
8. Calculate the pH, pOH, [H+1], [OH-1] of a 0.02 mol/L NaOH solution.
UNIT 5: ELECTROCHEMISTRY
9. Determine the oxidation number of the underlined element in the compounds below. Show your work.
(a) HClO3 (b) KNO2 (c) SO4-2
10. Use oxidation numbers to determine whether the following are redox reactions or not.
(a) CaCO3 → CaO + CO2
(b) SO3 + H2O → H2SO4