SNC2D Final Exam Review
Where should I start . . .
 Read through your notes.
 Redo all worksheets handed out during the 4 units.
 Study and then Re-do your unit tests/quizzes.
 Make study notes - especially the topics you are having trouble with.
 Complete the final exam review sheets. Here they are…! (note: not everything is included
in these example questions)
Chemistry Review
1. Definitions! Define each term below and also give and example.
Term
Definition
Physical
change
Chemical
change
Element
Example
Compound
2. a) Explain the characteristics of ionic and covalent compounds.
Characteristics
Ionic
Types of atoms involved: (Metals/non-metals)
Are the electrons shared or transferred?
Soluble (yes/no)
Conduct electricity (yes/no)
Melting point (high/low)
Appearance under a microscope
Covalent
b) Complete the chart below.
Lewis Dot diagram
(showing the bonding of the two
elements)
Magnesium and Chlorine
Sodium and Sulfur
Carbon and Fluorine (CF4)
Structural Diagram
Type of Bond
Formed
(ionic or
covalent)
Chemical Formula of
compound
Chemical name of
compound
Use the following words or numbers to complete questions 3-9. You may use words or numbers more than
once.
18
16
14
12
8
9
10
1
2
3
Neon
Argon
Helium
K+1
K-1
positively
negatively
not
neutrons
positrons electrons
protons
atomic mass atomic radius
3.
4.
5.
6.
7.
8.
9.
10.
The ion S2- would have ______ electrons surrounding its nucleus.
A neutral atom with 8 protons in its nucleus will also have ______ electrons. It will gain/lose (Circle
one)
______ electrons to match the electron population of _____, the nearest noble gas.
When element 19 has one electron taken away from it, its symbol is _______.
The atom is composed of an extremely small central nucleus containing protons (____________
charged, relative mass = 1) and ______________ (neutral, relative mass = 1 ) surrounded by
_______________ (negatively charged, relative mass = 0.0005).
The atomic number indicates the number of ___________ in an atom and is unique for each
element.
In a neutral atom, the number of ____________ must equal the number of ______________.
The number of neutrons in the nucleus is usually greater than or equal to the number of protons. The
sum of the numbers of protons and neutrons is called the ________________ .
Which of the following represent elements and which represent compounds? (circle the elements)
O2
11.
Co
CO
Fe
Al2(SO4)3
NO
Xe
P4
SO2
C8H18
Complete the following chart using a periodic table.
Symbol Atom or # of
# of
# of
Ion
protons electrons
neutrons
atom
0
1
1H
atom
19
20
23
11Na
atom
13
12
17
12.
13.
14.
15.
16
17.
10
12
35.453
Cl
The box above is from a typical periodic table.
List three pieces of information you can obtain
from this box.
What type of ion forms when a neutral atom gains an electron?
What type of ion forms when a neutral atom loses an electron?
What is a binary compound?
A white powder with a low melting point dissolves in water but does not conduct electricity in
solution. Is this an ionic or covalent substance? Explain your answer.
A yellow powder with a high melting point dissolves in water and conducts electricity in solution. Is
this an ionic or covalent substance? Explain your answer.
18. Give the correct name for each of the following compounds.
For compounds with a * , state how many of each type of atom make up one molecule.
XeF2
K3PO4
CS2
SnO2
BF3
Ba(OH)2
P2O5
SnF2
SO3
CuCl2
BrCl3
NiSO4
H2 S
*Fe2(SO4)3
AsF3
*Al(NO3)3
Na2O
CaBr2
Ca(PO4)2
NO
NaH
HF
H3PO4
MgH2
19. Provide the correct chemical formula for each of the following compounds.
carbon dioxide
barium phosphate
phosphorus pentasulfide
tin (II) bromide
dichlorine monoxide
nickel (II) sulfate
calcium sufate
sulfur hexafluoride
copper (II) sulfate
nitrogen monoxide
chromium (III) carbonate
carbon monoxide
cobalt (III) chlorate
iron (II) fluoride
sulfur dioxide
ammonium carbonate
boron trihydride
manganese (IV) oxide
iodine trichloride
beryllium sulfide
bromine monochloride
silver nitrate
dinitrogen trioxide
lithium nitride
tin (IV) oxide
zinc hydroxide
ammonium nitrate
calcium hydroxide
potassium oxide
lead (II) nitrate
sulfuric acid
hydrosulfuric acid
sulfurous acid
20. Explain why each of the following is wrong.
a) CaOH2
b) copper sulfate
c) magnesium dioxide
21. Use Lewis Dot diagrams to show how compounds would form between the following pairs of elements.
Show the chemical formula for each compound.
a) sodium and chlorine
b) calcium and fluorine
c) aluminum and nitrogen
d) lithium and nitrogen
22.
Balance the following and state the reaction type:
→
NH3(g)
a)
N2(g) + H2(g)
b)
K(s) + O2(g) →
c)
H2(g) + O2(g) → H2O(l)
c)
NaOH(s) + H3PO4(aq) →
d)
Pb3O4(s) →
23.
K2O(s)
Na3PO4(aq) + H2O(l)
PbO(s) + O2(g)
Write a balanced equation for each of the following word equations:
a)
phosphoric acid + sodium hydroxide → sodium phosphate + water
b)
magnesium + hydrochloric acid → (determine the products!)
c)
octane (C8H18) + oxygen gas → carbon dioxide gas + water vapour
24. Identify the reaction types in question # 22 as a single displacement, double displacement, synthesis,
decomposition, combustion or neutralization (or more than one of these)
25.
Complete the following word equations and then write a balanced chemical equation for each:
a)
A double displacement occurred between solutions of silver nitrate and calcium chloride.
b)
The single displacement between aluminum metal and aqueous lead(II)nitrate.
27.
Draw a sample pH scale. On the scale indicate the general locations of acidic substances, basic
substances or neutral substances.
28. Give the general formula for a neutralization reaction.
29. Define and explain the Law of Conservation of Mass
.30. Use the following table to answer the questions below:
Biology Review
1. State the function of each of the following parts of cells: nucleus, cell membrane, cell wall, mitochondria,
chloroplasts, vacuoles, E.R., ribosomes, lysosomes, centrioles
2. Animal cells are different from plant cells. List three differences.
3. How are osmosis and simple diffusion similar?
4. Review how to determine the size of a cell and how to make a scale diagram.
5. a) What is mitosis? b) What is the importance of mitosis to living organisms?
c) Draw a cell with 4 chromosomes going through the 4 phases of mitosis. (explain what is happening)
6. Complete the chart.
Eyepiece
Objective Lens
4X
15X
20X
Total Magnification
40X
150X
240X
7. Study your Digestion, Respiration, and Circulation diagrams
8. Give an example of mechanical digestion and an example of chemical digestion.
9. State the main function of each of the following digestive organs:
mouth, salivary glands, esophagus, stomach, small intestine, large intestine, liver, gall bladder, pancreas
10. Compare: arteries, veins, capillaries (size, type of blood carried, direction of blood flow)
11. What is the main function of each of the following?
a) red blood cells
b) white blood cells
c) platelets
12. Explain how having a large surface area in various locations
helps the digestive, respiratory, and circulatory systems.
Use the alveoli, capillaries, and small intestine as
specific examples.
13. Explain the following list: organelle, cell, tissue, organ,
system, individual
14. Why is the circulatory system important with regard to the
digestive system of a living organism?
15. Estimate the size of the cell in the drawing to the right.
Show all steps.
Optics Review
1. Be familiar with the following terms:
Visible light
Light Ray
Electromagnetic spectrum
Normal
Transparent
Translucent
Angle of incidence
Angle of Reflection
Real Image
Concave Mirror
Convex Mirror
SALT
Centre of Curvature
Principal Axis
Converge
Diverge
Plane mirror
Perpendicular
Incident Ray
Reflected Ray
Opaque
Virtual Image
Focus
Vertex
Refraction
Angle of Refraction
2. Using a diagram and object-image lines, show how the image of the following objects can be found in a
plane mirror . Describe each image in terms of SALT.
3.
4.
5.
6.
Explain the acronym SALT.
What would the angle of reflection be for an incident ray of 48˚ in a plane mirror?
State two laws of reflection.
How does the image of your face appear if you look into the following mirrors (use salt to describe):
a) a plane mirror
b) a convex mirror
c) a concave mirror (when your face is between F and the mirror)
7.
a) What is refraction? Why does it occur?
b) Explain any one piece of technology which employs the use of refraction.
8. Complete the following ray diagrams including SALT:
9. A concave mirror has a focal length of 10 cm. An object with a height of 3 cm is placed 12 cm from the
mirror. Draw the ray diagram including SALT to describe the image formed.
10. Complete the ray diagram for the image formed in the following lenses:
11. An object 5-cm tall is placed 8 cm from a converging lens with a focal length of 3 cm. Complete the ray
diagram and image characteristics.
12. Examine the indices of refraction in the following table.
a) calculate the speed of light through each media
Medium Index of Refraction
Material
A
1.00
Air
B
1.54
Crystal
C
1.46
Quartz
Speed of light
C = 3 x108 m/s
b) in which medium does light travel the fastest? __________________________
c) draw a ray of light with an angle of incidence of 45 degrees passing from air, through the
diamond, through the glass (note: exact angles through the media are not necessary)