Chemistry: Grade 9 Academic Quiz Review
Key Words: Metals, Non-metals, Metalloids, Chemical Families, Alkali Metals,
Alkaline Earth Metals, Halogens, Noble Gases, Valence Electrons, Particle Theory,
Pure Substances, Mixtures, Mechanical (Heterogeneous) Mixtures, Solutions
(Homogeneous), Alloys, Physical Properties, Chemical Properties, Physical Change,
Chemical Change
Metals, Non-metals, & Metalloids [LAB] (Pages 212-214, 220-222)
See in class note on “Metals, Non-metals, & Metalloids” & “Metals vs. Non-Metals
Lab”
1.
Which group on the periodic table do each of the following chemical families
belong to:
a. Alkali Metals
1
c. Halogens
17
b. Alkaline Earth Metals 2
d. Noble Gases
18
2.
How many valence electrons do each of the following chemical families have:
a. Alkali Metals
1
c. Halogens 7
b. Alkaline Earth Metals 2
d. Noble Gases
8
3.
How does the number of valence electrons impact the reactivity of an
element?
The fewer electrons the more likely the atom will lose it, the
more valence electrons the more likely it will take an electron. When an atom
loses or gains an electron easily it means it is very reactive. The further the
electrons are from the nucleus the more likely it will lose the electrons, the
lower the electronegativity.
4.
Create a table as shown below and compare the properties of Metals to NonMetals:
Physical Properties
Metals
Non-Metals
Metalloids
Lustre
Conductivity
Shiny
Very good
conductors
Solid
Not Shiny
Poor conductors
Shiny
Semi
conductors
solid
Most common state at
room temperature
Liquid or gas
Malleability or
Brittleness
Ductility
Malleable
brittle
Can be coiled
into a wire
Cannot be coiled
into a wire
brittle
Cannot be
coiled into a
wire
Hardness
Hard
Soft
hard
a. What properties might you expect of metalloids? Explain why semi-conductors
are useful for electronics. Metalloids have characteristics of a non-metal and
metal. Semi-conductors are useful because they can conduct electricity but will
not over heat.
Matter (Pages 175-178)
See note on “The Particle Theory” and Worksheet on “Pure Substance vs Mixture”
1. Did Magnesium or Sulfur react with acid? Magnesium reacted with acid
forming bubbles. No reaction with sulfur.
2. What is a conductivity apparatus made of? Copper wires, battery,
electrodes or alligator clips, switch, load (light bulb)
3. List the 5 key points outlined in the Particle Theory. Explain how water can
move from a liquid state to a gas state using each of the points outlined in
the Particle Theory.
a. All matter contains tiny particles called atoms
b. Substances like a desk has different atoms then an eraser.
c. You can’t see but particles are always in motion even when the
object is a solid or the water is still.
d. The higher the temperature the faster the particles move.
e. The closer particles are together the more they are attracted to each
other.
Water can move from a liquid state to gas state because its atoms move
more frequently than normal. The faster they move the further apart
they are and the less attraction they have for one another. Therefore
the water can no longer be in liquid form because the water molecules
are moving too fast to be in liquid form it then becomes a gas.
Which of the following sentences best explains why water evaporates at
its boiling point:
f. Water molecule become attracted to the air
g. Water molecules move rapidly when heated causing them to break
through the surface tension
h. Water molecules become less attracted to one another when they
are heated to high temperatures
i. Water becomes too hot and needs to escape in order to cool off
4. List 5 examples of pure substances and mixtures we have discussed in class
or have done in a worksheet in class.
Pure Substances
Pure water
Salt
Sugar
Mixtures
Tap Water
Fruit Salad
Air
5. Are alloys considered mixtures or pure substances? Can you find alloys on
the periodic table? Name 3 examples of alloys (research if you need to).
Mixtures, no you cannot find an alloy on the periodic table.
Examples:
Cast Iron – contains Iron some carbon and very little silicon
Solder – mostly tin and very little copper.
Steel – mostly Iron and small amounts of carbon and other metals
Sterling silver – Mostly Silver with some copper.
6. Is CaCO3 considered a pure substance or a mixture? Explain. It is a pure
substance because its atoms combine to form a single molecule.
7. Create a chart with 5 examples of a mechanical mixture (heterogeneous)
and a solution (homogeneous).
Mechanical Mixture
Solution
Fruit Salad
Apple Juice
Peanut butter and jam sandwich
Tap water
Chilli
milk
Lucky Charms
Tomato Sauce
Cookie and Crème milk shake
solder
Properties of Matter (Pages 179-186)
See note on “Properties of Matter” and Worksheet on “Chemical and Physical
Properties of Matter”
1. Describe yourself using a chart of quantitative and qualitative
descriptions.
Qualitative
Quantitative
Nice
Brown hair
Caucasian
Athletic build
6’10 tall
300 lbs
30 inch waist
Size 11 shoe size
2. Create 5 examples of chemical change and physical change discussed in
class.
Physical Change
Chemical change
Melting ice
Burning the wick on the candle
Cutting paper
Colour change in a reaction
Crumpling aluminum sheet
Bubbling from a reaction
Evaporation of boiling water
Heat given off from a reaction
Condensation of water on the
Loud pop
windshield in the morning
3. Underline all of the evidence of chemical change in the statement
below.
a. “ When liquid lead nitrate and potassium iodide react the mixture
produces a yellow colour and a solid substance”
i. Yellow colour and precipitate at the bottom (solid
substance)
b. What evidence is there that a chemical change occurred?
new colour and a new substance is formed.