1. In the following table, explain the charge, mass, and location of the three subatomic
particles we learned about. (6)
particle name
mass
charge
location
2. What is the number of electrons on the valence shell of strontium? arsenic? (2)
4. a) What is the number of protons, neutrons and electrons are in
209
80
Hg ? (3)
235
238
b) What is the difference between 92U and 92U ? What are these different versions of
uranium called? What is the same about them?(3)
5. Draw a Bohr diagram and a Lewis Dot diagram for sulfur and neon. (6)
7. Each element in a chemical family has similar chemical properties. Each element in a
chemical family has the same number of electrons in its valence shell. How does the second
statement explain the first statement? (2)
9. Why can you draw the Lewis Dot diagram for bismuth, even though the Bohr diagram is
ridiculously complicated? (2)
10. How does Bohr’s idea of orbits for electrons help explain the line spectra we saw
during the flame tests? (2)
11. a) Why do some lights produce line spectra, and others produce continuous spectra?
(2)
b) Which one are absorption spectra related to? How are they related?(2)
12. Why did Mendeleev leave gaps in his periodic table, and how did they end up
supporting his method of organization? (2)
14. On the periodic table below, indicate where the following are: transition metals, noble
gases, alkaline earth metals, halogens.
(4)
a) write correct chemical formulas for the following compounds (28 marks)
1. cesium iodide _________________
2. cobalt(III) phosphide _________________
3. iron(II) oxide _________________
4. iron(III) oxide _________________
5. calcium phosphate _________________
6. dinitrogen tetroxide _________________
7. mercury(I) nitrate _________________
8. mercury(I) nitride _________________
9. iodine _________________
10. ammonium sulfite _________________
11. nitrogen trihydride _________________
12. sodium hydroxide _________________
13. diphosphorous pentoxide _________________
14. magnesium oxide _________________
b) write the correct names for the following compounds (20 marks)
1. HBr _____________________________
2. NiO _____________________________
3. NH4NO3_____________________________
4. NO2 _____________________________
5. Mg(OH)2 _____________________________
6. NO _____________________________
7. Ag2SO4 _____________________________
8. SnO2 _____________________________
9. CBr4 _____________________________
10. NaHCO3 _____________________________
SHORT ANSWER
1. Write the dissociation reaction for: (6 marks)
a) AlBr3(aq) →
b) H2SO4(aq) →
c) NH4I(aq) →
2. Explain the difference between a covalent and ionic bond. Explain the difference
between a covalent and ionic compound. (4 marks)
3. Why do atoms give/receive/share electrons at all? (1 mark)
5. Explain what defines an acid and a base. Give an example of each from earlier in the
test. (4 marks)
6. How do acids and bases neutralize each other? (2 marks)
2. Classify and balance the following reactions. All formulas are correct. (10 marks)
a) Al + HCl → AlCl3 + H2
b) Sr + O2 → SrO
c) C6H12O6 + O2 →
CaCl2 →
d) Al2(SO4)3 +
e) ZnCO3 →
CO2 + H2O
ZnO +
CaSO4 + AlCl3
CO2
3. Write out the following reaction, balance and classify it. (3 marks)
lead(II) nitrate + potassium iodide → lead(II) iodide + potassium nitrate
4. Complete and balance the following neutralization reactions: (4 marks)
HCl + Ca(OH)2 →
H2SO4 + NaOH →
8. Predict the products, and balance the following reactions: (14 marks)
HCl →
a) SD:
Zn +
b) DD:
MgI2 + AgNO3 →
c) SD:
NaI + F2 →
d) DD:
CaI2 +
e) SYN:
Na2SO4 →
Na + N2 →
f) DEC: NaCl →