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SNC2P
Chemical Reactions Unit Review
1. Draw Bohr-Rutherford diagrams for the following atoms and ions.
a) aluminum atom b) helium atom
c) oxygen ion d) beryllium ion
2. Draw Lewis Dot Diagrams of the following atoms and ions.
a) magnesium atom
b) nitrogen atom c) fluorine ion d) sodium ion
3. The figure below shows a Bohr diagram of a calcium atom.
a) How many electron shells are shown?
b) How many valence electrons are in the valence shell?
c) The charge on a calcium ion is 2+. Explain how this diagram might
have been used to predict this charge.
4. What is a molecule?
5. What is a valence shell?
6. What is a valence electron?
7. What kinds of elements combine to form ionic compounds?
8. What kinds of elements combine to form molecular compounds?
9. Use electron dot diagrams to show the bonding in the following ionic
compounds. (show electron transfer, draw stick diagrams, write formula)
a) Na + Br
b) Mg + F
c) Al + Cl
10. Use electron dot diagrams to show the bonding in the following covalent
compounds. (show electron sharing, draw ions with charges, write formula)
a) C + O (CO2)
b) F + F (F2)
c) O + Cl (OCl2)
11. Compare at least 3 physical properties of ionic and covalent compounds.
How would you design an experiment to decide if an unknown solid is ionic
or covalent?
12. State the law of conservation of mass.
13. Where are the reactants and the products located in a chemical equation?
14. What type of chemical reaction is the opposite of a synthesis reaction?
15. If the products of a chemical reaction are carbon dioxide and water.
What kind of chemical reaction occurred?
16. Balance the chemical reactions below. Classify each chemical reactions
into one of the 5 major groups
Type of Reaction:
a)
b)
c)
d)
e)
___ KClO3 ___ KCl + ___ O2
___ C3H6 + ___ O2  ___ CO2 + ___ H2O
___ Li4C + ___ Ca  ___ Li + ___ Ca2C
___ H2 + ___ O2  ___ H2O
___ CsF + ___ AlBr3  ___ CsBr + ___ AlF3
_______________
_______________
_______________
_______________
______________________
17. Write the names of the following ionic compounds
a) BeO
e) Ca3P2
b) KCl
f) MnCl2
c) MgBr2
g) K2SO4
d) Al2S3
h) Li3PO4
18. Write the formulas for the following ionic compounds.
a) sodium bromide
d) ammonium sulphate
b) beryllium phosphide
e) ammonium nitrate
c) copper (I) oxide
19. Write the names of the following molecular compounds
a) S2O3
d) N2O3
b) P2S5
e) CO2
c) OF2
20. Write the formulas for the following binary molecular compounds.
a) sulphur hexafluoride
d) carbon tetrachloride
b) carbon disulphide
e) carbon monoxide
c) dinitrogen monoxide
21. For each of the following word equations, identify the type of chemical
reaction it represents.
a) methane (CH4) + oxygen  carbon dioxide + water
b) barium + oxygen  barium oxide
c) aluminum bromide + fluorine  aluminum fluoride + bromine
d) magnesium chloride  magnesium + chloride
e) lithium sulphate + barium chloride  lithium chloride + barium
sulphate
22. Write the skeleton equation and balanced chemical equation for each of
the following chemical reactions.
a) lead(II) nitrate + sodium sulphate  lead (II) sulphate + sodium
nitrate
b) carbon disulphide + oxygen  carbon dioxide + sulphur dioxide
23. When calcium metal undergoes a chemical reaction with oxygen gas,
solid calcium oxide is produced. Identify the type of chemical reaction, and
then write the balanced chemical equation.
24. Compare the appearance of complete and incomplete combustion. How
will you decide if combustion is complete? What would cause combustion to
be incomplete?
35. Write out the balance chemical equation for the complete combustion of
propane (C3H8).