Name: ___________________________________
Date: __________________________
Exam Review Questions
CHEMISTRY
1. Use Lewis dot diagrams to illustrate the formation of an ionic bond between the following atoms:
a) cesium and iodine
b) strontium and sulfur
c) aluminum and oxygen
2. What are valence electrons? Why are they important?
3. What is a “stable octet”?
4. a)What are ions?
b) Explain the difference between a cation and an anion? Provide an example of each.
5. Explain why we have to balance the number of atoms between the reactants and the products in a
chemical equation.
6. What is the difference between an ionic bond and a molecular bond?
7. When rubidium is dropped into a bathtub full of water, a hole is blasted through the tub.
a. Is this a physical or chemical change?
b. Describe either a physical or chemical property:
8. Balance the following equations
a. ______N2 + ______O2 => _____N2O5
i. State the type of reaction: ______________________
b. ______H3PO4 + ______ KOH =>______K3PO4 + ______H2O
i. State the type of reaction: _______________________
9. A solution contains 0.008 hydrogen ions
a. Calculate the pH.
b. Is the solution acidic or basic?
10. For the following reactants, predict the products and write the balanced equation:
a. Aluminum sulfide
b. Calcium nitride and potassium
11. Name the following compound
o Li3N:
_______________________
o FeI2:
_______________________
o MgSO4:
_______________________
o S 2O
_______________________
o H2CO3
_______________________
o NiPO4
_____________________________________
12. Write the formulas for the following compounds:
a. Strontium phosphide:
b. Chromium (III) chloride:
_______________________
_______________________
c. Beryllium sulfate:
_______________________
d. Trinitrogen pentafluoride
_______________________
e. Nitric acid:
_______________________
f. Mercuric chlorate:
_______________________
13. As a newly hired chemist, you have been given the task of creating magnesium iodide. The
reactants you have been given are magnesium (a long ribbon, the length and width of a shoelace)
and iodide (a dark blue liquid). Unfortunately, the reaction happens too fast and the production line
cannot keep up with the product produced. Describe 4 methods to slow down the reaction.
14. Copper has 2 isotopes: Cu-63 (62.93u) and Cu-65 (64.93u). These isotopes have an isotopic
abundance of 69.1% and 30.9% respectively. Calculate the average atomic mass of copper.
15. A piece of iron contains 0.0718 mol of iron. How many atoms of iron are in the piece?
16. A new cleaning solution contains 8.03 x 1023 molecules of ammonia. How many moles of ammonia
are in the solution?
17. What is the molar mass of one mole of Ca3(PO4)2?
18. A glass of water contains 55.6mol of water. What is the mass of water?
19. How many moles are in 7.34g of HNO2?
20. A sample contains 7.38 x 1021 molecules of Pb3(PO4)2. Determine the mass
21. Determine the number of molecules of 23.5g of S2Cl2. (5 marks)
22. Consider a 1 mol sample of CH4
a) How many molecules of CH4 are in the sample? _______________
b) How many atoms are in the sample? ________________
c) How many hydrogen atoms are in the sample? ______________
d) What is the mass of the sample? ____________
e) What is the molar mass of the sample? ______________
23. Determine the percent composition of each compound
a) CCl2F2
b) Pb4OH
c) MgCl2  2H2O
24. While exploring the Amazon for new animals, you stumble across a never seen before compound. After
returning the compound to the lab, you find that the 85 g sample is made up of 14 g Boron and the rest
Fluorine. Your goal is to find the molecular formula of the compound.
a)
b)
c)
d)
Calculate the percentage composition of this compound
Calculate the empirical formula of the compound
Calculate the molar mass of the empirical formula for the compound
A second tests shows that the molar mass of the molecular formula is 135.62g/mol, calculate the
molecular formula for the compound.
25. What is the empirical formula of a compound that is 15.9% boron and 84.1% fluorine?
26. A brand new compound was formed in a lab in Brampton. The compound contains only carbon and
hydrogen, and it was placed into a carbon-hydrogen combustion analyzer. After the combustion,
1.64g of carbon dioxide and 0.807g of water was produced. Calculate the empirical formula of the
new compound.
27. A new pharmaceutical drug has an empirical formula of C18H21NO3. If its molar mass is 897g/mol,
what is the molecular formula? (4 marks)
28. Ammonium sulfate is used as a source of nitrogen in some fertilizers. It reacts with sodium
hydroxide to produce sodium sulfate, ammonia, and water.
(NH4)2SO4(s) + 2NaOH(aq)  Na2SO4(aq) + 2NH3(g) + 2H2O(l
a) What mass of sodium hydroxide is required to react completely with 15.4 g of (NH 4)2SO4?
b) How many molecules of water are produced if 15.4 g of (NH4)2SO4 reacts?
29. Powdered zinc and sulfur react in an extremely rapid, exothermic reaction. The zinc sulfide that is
formed can be used to coat the inside of a television tube.
Zn(s) + S(s)  ZnS(s)
A 6.00 g sample of Zn is allowed to react with 3.35 g of S.
a) Determine the limiting reactant.
b) If you had 47 g of the limiting reactant, what would the mass of the product obtained be?
30. a) Explain the difference between actual yield and theoretical yield.
b) Discuss two reasons why these quantities are usually different.
31. Lithium hydroxide, LiOH, is used in spacecraft to recondition the air by absorbing the carbon dioxide
exhaled by astronauts. The reaction is shown below.
2 LiOH(s) + CO2(g)  Li2CO3(s) + H2O(l)
An astronaut produces an average of 1.00 x 103 g of carbon dioxide each day. What mass of lithium
hydroxide should engineers put on board a spacecraft if there are 4 astronauts going on a 5 day mission
32. For the following reaction, which of the given reactants do you think would be the limiting reactant?
Provide support for your hypothesis.
C6H12O6(s) + 6O2(g)  6CO2(g) + 6H2O(l)
PHYSICS
1. At what angle of incidence does no refraction occur?
2. Light is travelling from air into a more optically dense medium. Draw the refracted and reflected
ray. Also, calculate the angle of incidence and angle of reflection. (2 marks)
3.
4.
5.
6.
When does total internal reflection occur?
If I want to create an image bigger than my object, using a lens, where do I place my object?
What is myopia? How do you treat it?
If I want an image smaller than my object, using a converging mirror, where would I place my
object? (1 mark)
7. Calculate the index of refraction if the speed of light in a material is 0.5 x 10 8 m/s (speed of light is 3
x 108 m/s
8. A lens has a focal point of 2.5 cm. The object is 1cm in height and placed 5 cm from the optic
center. Draw the image
Describe 4 image characteristics:
9. A mirror has a focal point of 4cm. The object is 1 cm in height and place 7cm from the vertex. Draw
the image
Describe 3 image characteristics:
10. Draw the image created by the object on the plane mirror.
11. A 1cm object is placed in front of a lens, which produces an inverted image 6cm high. If the object is
place 31cm from the lens, what is the focal length of the lens?
12. Describe how the eye is able to see an image
13. Describe the necessary changes to camera to capture a magnified image
14. Standing on an angle from a glass cup, a penny is placed underneath in plain view. When the glass is
filled with water, the penny disappears. How does this illusion work? (3 marks)
15. Calculate the index of refraction if the speed of light in a material is 5 x 10 8 m/s.
16. Calculate the image distance when an image is magnified by a factor of -40 and the object distance
is 15m.
17. Calculate the magnification of an object that has an image distance of 1.5m and object distance 0.2
m.
18. Determine the image distance and image height for a 5 cm tall object placed 59 cm from a
converging lens having a focal length of 18 cm.
19. An object is placed 3.4m from the lens of a camera. If the focal length of the camera is 80mm, what
is the image distance?