Name: 
 

Chemistry 12: College Preparation Unit 1 Self Quiz



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 

Which of the following ions has the same number of electrons as an argon atom, Ar?
a.
S2+
c.
K-
b.
Mg2+
d.
P3-
 

 2. 

Which type of reaction does the following equation represent?
Zn(s) + H2SO4(aq) ® H2(g) + ZnSO4(aq)
a.
synthesis
c.
single displacement
b.
decomposition
d.
double displacement
 

 3. 

Which of the following bonds is the most polar?
a.
H—F
c.
H—Cl
b.
F—F
d.
Cl—Cl
 

 4. 

Who stated that electrons can only jump between fixed energy levels?
a.
Bohr
c.
Rutherford
b.
Chadwick
d.
Dalton
 

 5. 

Which of the following properties is typical of an ionic compound?
a.
It is colourless.
c.
It is a nonelectrolyte.
b.
It is insoluble in water.
d.
It has a high melting point.
 

 6. 

The methane molecule, CH4(g), consists of a carbon atom bonded to four hydrogen atoms. Its shape is
a.
linear
c.
pyramidal
b.
bent
d.
tetrahedral
 

 7. 

An atom can form a positive ion by
a.
losing electrons
c.
losing protons
b.
gaining electrons
d.
gaining protons
 

 8. 

Which of the following statements is not considered to be an observation?
a.
The colour of the cabinet is black.
b.
The height of the desk is 96 cm.
c.
The temperature of the solution is 26°C.
d.
The temperature of a substance is a measure of the average kinetic energy of the molecules that comprise it.
 

 9. 

Which of the following forms of electromagnetic energy has a higher frequency than UV energy?
a.
X-ray waves
c.
microwaves
b.
radio waves
d.
infrared waves
 

 10. 

Which of the following atoms is subjected to magnetic fields and radio waves during an MRI?
a.
carbon
c.
hydrogen
b.
oxygen
d.
potassium
 

 11. 

An electron in an excited state must have
a.
released energy in the form of light
b.
absorbed energy
c.
paired with another electron from another atom
d.
been ejected from an atom by absorbing light energy
 

 12. 

Which of the following is an example of qualitative analysis?
a.
determining if a block of concrete has been carbonated
b.
identifying a substance by the colour it emits during a flame test
c.
identifying a substance by its line spectra
d.
all of the above
 

 13. 

If aqueous silver nitrate, AgNO3(aq), is mixed with aqueous calcium chloride, CaCl2(aq),
a.
no precipitate will form
b.
a precipitate of calcium nitrate, Ca(NO3)2(s), will form
c.
a precipitate of silver chloride, AgCl(s), will form
d.
a single displacement reaction will occur
 

Short Answer
 

 14. 

Briefly outline J.J. Thomson’s contribution to modern atomic theory.
 

 15. 

Complete each of the following double displacement reaction equations by balancing it and adding states. Write the total ionic equation and net ionic equation for each reaction.
a. AgNO3 + NaCl ® AgCl + NaNO3
b. Na2CO3 + Zn(NO3)2 ® NaNO3 + ZnCO3
 

 16. 

Draw a Lewis structure for each of the following molecules:
a. SiI4
b. NH3
 

 17. 

The following flow chart outlines an experimental procedure for determining the presence of Pbimages/i0190000.jpg and/or Srimages/i0190001.jpg ions in a solution.

images/i0190002.jpg

a. Sodium chloride is added to the solution, and a precipitate forms. The precipitate indicates the presence of which ion?
b. What piece of equipment could be used to separate the precipitate from the supernate?
c. Using the solubility rules, explain why sodium chloride must be added to the solution before sodium sulfate in order to obtain conclusive results.
 

 18. 

Give three situations in which spectroscopy can be used to perform qualitative analysis.
 

 19. 

A solution is known to contain sulfate and/or bromide ions. Design an experiment to test for the presence of these two ions. Use the solubility rules to help you decide which ions you should use to test for the presence of sulfate and bromide ions.
 

 20. 

A solution conducts electricity, is basic, and forms a precipitate when sodium sulfate is added. When the solution is subjected to a flame test, the flame turns a yellow-green colour. Write the chemical formula for a solute that may be present in the solution. Give reasons for your choice.
 

 21. 

During an experiment, a technician notes the colour of each solution and conducts a flame test on each solution. Which ions are present in solutions A to E in Table 1?
Table 1 Solution and Flame Colours
Solution
Solution colour
Flame colour
A
colourless
violet
B
blue
green
C
colourless
yellow
D
colourless
yellow-red
E
colourless
bright red
A.
B.
C.
D.
E.
 

 22. 

Using what you have learned in this unit, write a paragraph that explains the chemistry behind a fireworks display. In your paragraph, include the following terms: ground state, excited state, Bohr model of the atom, flame test. Make sure that you comment, in general, on how the different colours in a fireworks display are produced.
 



 
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