Science 10 Final Exam Chemistry Review KEY
Part 1: Definition – Compare and contrast THREE of the following terms: (9marks)
1. Ionic compound and molecular compound
a. Ionic – A compound consisting of a metal and nonmetal, metal and polyatomic ion, or
nonmetal and polyatomic ion.
b. Molecular – A compound consisting of 2 nonmetals
c. Both are created when ions combine with each other
2. Alkyl halide and Halogen
a. Alkyl Halide - Group 1 in the periodic table (ex/ Sodium)
b. Halogen - Group 17 in the Periodic Table (ex/ Fluorine)
c. Both are groups within the Periodic Table
3. Reactants and products
a. Reactant – Chemicals before any mixing has occurred
b. Product – Chemicals that are created after mixing has occurred
c. Both are involved in chemical formulae
4. Metals and nonmetals
a. Metals – Left side of the periodic table
b. Nonmetals – Right side of the periodic table
c. Both are found in the Periodic table and are separated by the metalloids
Part 2: Multiple Choice – Choose the best response for the following. (10 marks)
1. In class we watched a video about a group of chemicals that reacted explosively with water.
These were:
a. Halogens
b. Alkyl Halides
c. Noble Gases
d. Earth Alkaline Metals
2. Fluorine is a(n):
a. Alkyl halide
b. Halogen
c. Noble gas
d. Transition metal
3. Combining Neon with Beryllium would create a:
a. Ionic Compound
b. Molecular compound
c. Neon wouldn’t combine with Beryllium
d. Inorganic compound
4. The third shell can hold a maximum of:
a. 2 protons
b. 2 electrons
c. 8 protons
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d. 8 electrons
Science 10 Final Exam Chemistry Review KEY
5. The outermost shell of an atom is called:
a. Noble
b. Valence
c. Exergonic
d. Bohr
c. -1
d. -1
6. All halogens form a charge of:
a. +1
b. +2
7. In a chemical reaction, when a substance is dissolved in water, or is in solution form it is labeled
behind the compound with a(n): OMIT  Not covered in class
a. (s)
b. (g)
c. (aq)
d. (l)
8. NACL is the chemical formula for:
a. Sodium chloride
b. Monosodium monochloride
9. Cobalt always has:
a. 32 neutrons
c. Sodium monochloride
d. There is no such thing as NACL
b. 27 protons
c. Atomic mass of 59
d. 27 neutrons
10. When drawing a Bohr diagram always write the:
a. Number of protons in the nucleus
b. Number of neutrons in the nucleus
c. Atomic mass in the nucleus
d. Both a and b
Part 3: Fill in the Blanks – The following sentences are taken directly from
handouts(10 marks)
1. LABORATORY SAFETY HANDOUT
a. Students should know the proper _fire drill______________ procedure.
2. THE PERIODIC TABLE
a. A Russian chemist, _Dmitri Mendeleev_____________, made the first periodic table.
Later, Henry Mosley_______________ improved the table by rearranging it based on
the atomic number.
b. _Metalloids______________ generally have the properties of both metals and
nonmetals
3. ATOMIC STABILITY
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Science 10 Final Exam Chemistry Review KEY
a. The charge indicating the number of electrons gained or lost is written as a
_superscript______________
b. A positive ion is called a(n) _cation______________ and a negative ion is called a(n)
_anion______________.
4. They (valence electrons) represent the number of electrons that will be
_transferred______________, _accepted______________ or _shared______________ between
atoms when forming stable compounds.
Part 4: Short Answer – Complete the following questions (34 marks)
1. Draw the Bohr diagram for Sulfur as an element (3 marks)
2. Draw the shell diagram for Barium as an ion (3 marks)
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Science 10 Final Exam Chemistry Review KEY
3. Complete the following table (8 marks)
Symbol
Al
Al3+
Mg
Cl-
Te2-
Atomic #
13
13
12
17
52
Protons
13
13
12
17
52
Neutrons
14
14
12
18
76
Electrons
13
10
12
18
54
Atomic Mass
27
27
24
35
128
Charge
0
3+
0
-1
2-
4. Complete the following table: (8 marks)
Elements or Polyatomic ions
Molecule
Name
Sodium + chlorine
NaCl
Sodium chloride
Magnesium + phosphorus
Mg3P2
Magnesium phosphide
Ammonium + phosphate
(NH4) 3PO4
Ammonium phosphate
Sulfur + Oxygen
SO3
Sulfur trioxide
Ammonium + Hydroxide
NH4OH
Ammonium hydroxide
5. Balance the following chemical reactions: (11 marks)

a.
S8
+
8 O2
8 SO2
b.
1 C2H6
+
3.5 O2 
3 H 2O +
1 C O2
c.
3 KOH
+
1 H3PO4 
1 K3PO4 +
3 H 2O
6. What types of reactions were occurring in each part of question 4? (3 marks)
a. Synthesis
b. Combustion
c. Double Replacement
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