Unit 1: Matter and Qualitative Analysis

SCH4CName:______

Exam Review Assignment

due exam day

Unit 1: Matter and Qualitative Analysis

1. Using examples, explain the difference between:

1. Complete the subatomic particle chart

1. In each of the following reactions balance the equation and indicate if they are synthesis, decomposition, single displacement or double displacement.

a)H2O + SO3  H2SO4 ______

b)Mg(OH)2 + HNO3  Mg(NO3)2 + H2O______

c)FeCl3 + NaOH  Fe(OH)3 + NaCl______

d)Cl2 + ZnI2  ZnCl2 + I2______

e)H2SO4 + Mg  MgSO4 + H2 ______

f)K2O + H2O  KOH______

g)NaClO3  NaCl + O2______

h)BCl3 + H2S  B2S3 + HCl______

i)Pb(NO3)2  PbO + NO2 + O2 ______

j)NaOH + H3PO4  Na3PO4 + H2O______

1. Determine whether each of the following compounds is soluble in water: (aq) or (s) ?

a) CoOH (cobalt hydroxide) ______

b) NaNO3 (sodium nitrate) ______

c) NaOH (sodium hydroxide) ______

d) AgI (silver iodide) ______

1. Predict the products of the following reactions and BALANCE the equations.

a) Li(s) + NaCl(aq)

b) Cu(s) + AgNO3(aq)

c) F2(aq) + KI(aq)

d) Ag(NO3) (aq) + NaOH (aq) 

e) Mg(NO3)2(aq) + Ca(NO3)(aq) 

f) Fe(NO3)3(aq) + NaOH (aq) 

1. Write the total ionic equation, and net ionic equation for the chemical reaction below. Chemical Equation

Total Ionic Equation

Net Ionic Equation

1. How can you use the following qualitative properties to identify a gas sample?
2. line spectra

1. flame tests

1. Answer the following:
2. How is precipitation used in qualitative chemical analysis?

1. Is solution colour useful for identifying all metal ions? Explain.

1. You are given a mystery solution that may contain Cu+ and/or Sr2+. How could you use the solubility rules and flame tests to identify which, if any, of the ions are present? (Make a flow chart diagram).

Unit 2: Quantities in Chemistry

1. Calculate the molar mass of the following molecules or formula units:

a)C6H6b) Ba(NO3)2c) K3PO4d) NH3

1. Calculate the molar mass of

a)tin, if 1.010 mol has a mass of 119.88 g.

b)an element, if 26.66 g contains 2.220 mol. Identify the element.

1. Calculate the number of particles:

a)A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin?

b)How many molecules of water are in 55.6 mol?

c)In 2.5g of HCl.

1. Calculate the number of moles:

a)in a sample of Al2O3 that contains 7.71 x 1024 molecules.

b)in a sample of aluminum that contains 2.1 x 1024 atoms.

c)in 3.2 g of oxygen gas * remember HOFBrINCl

1. Calculate the mass:

a)0.10 mol of glucose, C6H12O6c) of 8.8 x 1024 molecules of NH3.

b)0.10 mol of carbon dioxided)of 6.02 x 1024 formula units of ZnCl2

1. Calculate the mass of oxygen that is needed to burn 15 g of propane. The balanced chemical equation is given below (although technically – you should be able to figure it out!)

C3H8 + 5O2 --> 3CO2 + 4H2O

1. How many molecules of oxygen are produced from the decomposition of 12 g of water into its elements? (REMEMBER TO BALANCE FIRST) H2O --> O2 + H2

1. Consider the following reaction: SO2 + O2 --> SO3

a)192.18 g of sulfur dioxide reacts excess oxygen to produce sulfur trioxide. What is the mass of sulfur trioxide produced? (balance the equation first!)

b)Sulfur trioxide is a gas. If a laboratory experiment is done with the above amounts and 145 g of gas are collected, what is the percentage yield of sulfur trioxide?

9. What is the difference between limiting and excess reactant?

10. If you dilute 20 mL of 6.0 mol/L HCl to 1.0L, what is the concentration of the final solution?

11. You need to make 500 mLof a 1.2 mol/L CuSO4 solution from solid CuSO4. Determine the mass of CuSO4 you will need to make this solution.

Unit 3: Organic Chemistry

1. Draw the structural formula for the following hydrocarbons

1. Name the following hydrocarbons

1. With respect to Fractional distillation and cracking:

a)Explain how the two technologies are both important for producing gasoline.

b)What are 3 other useful fuels that come from petroleum?

1. Which organic family has the highest boiling points? the lowest?

1. Using structures show the addition reaction of:

a)2-butene and hydrogen bromide (HBr)

b)2-pentyne and chlorine gas *

1. Write a balanced chemical equation for the complete combustion of the hydrocarbon:

a)ethane

b)propyne

1. Answer the following questions on organic solvents:

a)Why are organic solvent vapours so dangerous?

b)What are some precautions to consider with using organic solvents?

1. Use structural formulas to show the formation of an ester between 1-butanol and propanoic acid.

1. Put the following bonds in order of increasing electronegativity (least polar to most) O-H, C-H, H-H, F-H.

10. Use the Octet Rule to draw the Lewis Structures for the following:

11. Complete the chart and circle the functional group in the example.

12. Is the bond between Cl-O polar covalent or non-polar covalent? Show your calculation.

13. a) What is the difference between polar covalent bonds and non polar covalent bonds?

b) What do these bonds have in common?

Unit 4: Chemistry in the Environment

1. Complete the table:

1. Classify each of the following solutions as acid or base:

a)NaOHb) HC2H3O2c) Mg(OH)2d) HCl

1. a) What two metal ions are most responsible for the hardness of water?

b) How can hard water reduce the efficiency of appliances that are used to heat water?

1. What is acid rain? Name two pollutants that are major contributors to acid precipitation. What can be done to prevent acid rain?

1. A titration is done to determine the concentration of an unknown acid. 10 mL of acid is put in a flask with 3 drops of phenolpthalein. NaOH (a base) with a concentration of 2 mol/L is added drop by drop.

a)What is the function of the phenolpthalein?

b)When should the experimenter stop adding NaOH?

c)What has happened to the acid at this point? What is in the flask now?

d)If it only takes 5 mL of base to reach this point, what is the concentration of the acid? Show your calculations.

e)Draw the set up for a titration.

Unit 5: Electrochemistry

1. Identify the reactant oxidized and the reactant reduced in each of the following reactions:

a)Zn(s) + Cl2 (g) --> ZnCl2 (s)

b)Cu(NO 3)2 (aq) + Pb (s) --> Cu(s) + Pb(NO 3)2 (aq) *hint- find total ionic equation first

c) Zn(s) + Cu2+(aq) --> Zn(2+aq) + Cu (s)

1. Answer the following questions about galvanic cells:

a)What is a galvanic cell?

b)Describe the function of the salt bridge.

c)What happens to the cell potential if the salt bridge is removed? why?

d)Why are galvanic cells not a practical source of electricity?

1. Write the anode, cathode and overall cell reactions that occur when each pair of half cells is combined to form a galvanic cell.

a) a copper electrode in a solution of copper(II)nitrate and a tin strip in a solution of tin(II) chloride.

b) an aluminum strip in a solution of aluminum nitrate and a silver strip in an solution of silver nitrate.

1. a) draw a diagram of a galvanic cell for each of the cells described in the question above.

b) identify the anode and the cathode in each cell

c) indicate the direction of electron flow and ion flow in the cell

5. What is corrosion? What 4 factors affect the rate of corrosion? How does corrosion affect society?

Unit 2 Review Answers

1. a) 78.12 g b) 261.35 gc) 212.27 gd) 17.04 g

2. a) 118.7 g/molb) 12.01 g/mol, Carbon

1. a) 1.07 x1022 atoms of ironb) 3.35 x 1025 molecules.c) 4.1 x1022 molecules.
2. a) 12.8 molb) 3.5 molc) 0.10 mol
3. a) 18 g b) 4.4 gc) 250 gd) 1363 g or 14 kg
4. 54 g of oxygen
5. 2.0 x 1023 molecules.