1. 1.2 Investigating Matter Matter is anything that has mass and volume.
Mass is the amount of matter in a substance or object.
Mass is often measured in grams or kilograms.
Volume is the amount of space a substance or an object occupies.
Volume is often measured in litres.

2. Mass Versus Volume
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3. Chemical Change A chemical change is a change in matter
that occurs when substances combine to form new substances.
(c) McGraw Hill Ryerson 2007
See page 17

4. CHEMICAL CHANGE
Sodium Na (solid)
Chlorine
Cl2 (gas)
Salt
NaCl

5. (c) McGraw Hill Ryerson 2007

6. Physical Change and Changes of State
When a physical change occurs, there may be a change in appearance, but no new substances are formed.
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See page 18

7. Physical Change and Changes of State
For example, when ice or snow melts to water, this physical change is a change of state. No new substances are formed. VS
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8. Physical Changes

9. The Particle Model of Matter
Describes the behaviour of matter.
Matter is made of small particles.
There are spaces between the particles.
Gases have more space than liquids. Liquids have more space than solids.
(c) McGraw Hill Ryerson 2007
See page 18

10. (c) McGraw Hill Ryerson 2007

11. The Particle Model of Matter
Particles are always moving.
Particles are attracted to each other. The strength of attraction depends on the type of particle.
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12. The Particle Model of Matter
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13. The Kinetic Molecular Theory
Describes what happens to matter when
the kinetic energy of particles changes.
The main points in the theory are:
Matter is made of small particles.
There is empty space between particles.
Particles are constantly moving.
Energy makes particles move.
(c) McGraw Hill Ryerson 2007
See page 19

14. The Kinetic Molecular Theory
Solid particles are packed together and
cannot move freely. They can only vibrate.
Liquid particles are farther apart and can slide past each other.
Gas particles are far apart and move around quickly.
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15. The Kinetic Molecular Theory and Changes of State
Solid Particles are close together, fixed in position and vibrating. Melting As temperature increases, particles’ kinetic energy increases. Liquid Particles are still close, but slide past one another. Boiling continues to increase, creating more space. Gas Particles are highly energetic and moving freely.
See page 20

16. TEMPERATURE AND CHANGE OF STATE
When heat is added to a substance, it’s particles gain kinetic energy and vibrate faster. This causes them to move farther apart.

17. TEMPERATURE AND CHANGE OF STATE
MELTING is the change of state from a SOLID to a LIQUID (popsicle melting )
SOLIDIFICATION (freezing) is the change of state from a LIQUID to a SOLID (pond freezing)

18. TEMPERATURE AND CHANGE OF STATE
EVAPORATION is the change
of state from a LIQUID to a GAS
( sweating )
CONDENSATION is the change of state from a
GAS to a LIQUID
( dew forming on lawn)

19. TEMPERATURE AND CHANGE OF STATE
SUBLIMATION is the change of state from a SOLID to a GAS (dry ice)
DEPOSITION is the change of state from a GAS to a SOLID (frost forming)

20. Temperature and Changes of State
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See page 21

21. Describing Matter Physical Properties Qualitative – non-numerical
state, colour, malleability
Quantitative – numerical
conductivity, viscosity, density
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22. (c) McGraw Hill Ryerson 2007

23. QUALITATIVE PROPERTIES
1. STATE is the physical state the matter is in: SOLID, LIQUID or GAS
2. COLOUR refers to the COLOUR of the matter

24. QUALITATIVE PROPERTIES
3. FORM refers to the SHAPE and STRUCTURE
(soft, hard, rough, smooth)
4. CLARITY refers to the ability for light to pass through matter
(opaque, translucent, transparent)

25. QUALITATIVE PROPERTIES
5. CRYSTALINITY refers to the
SHAPE or APPEARANCE of CRYSTALS
6. MALLEABILITY refers to the ability of the matter to be BEATEN into SHEETS

26. QUALITATIVE PROPERTIES
7. DUCTILITY refers to the
ability to be DRAWN into WIRES
8. LUSTRE refers to the
REFLECTIVENESS of an object
9. MAGNETISM refers to the tendency of matter to be ATTRACTED to a MAGNET

27. QUANTITATIVE PROPERTIES
1. SOLUBILITY refers to the ability
to DISSOLVE in WATER
2. CONDUCTIVITY refers to the ability to CONDUCT ELECTRICITY or HEAT

28. QUANTITATIVE PROPERTIES
3. VISCOSITY refers to the RESISTANCE of FLOW 4. DENSITY is the RATIO of the object’s MASS to its VOLUME

29. QUANTITATIVE PROPERTIES
5. MELTING/FREEZING POINT
is the TEMPERATURE at which
melting/freezing will occur
6. BOILING/CONDENSATION POINT is the TEMPERATURE at which boiling/condensing
will occur

30. TWO CATEGORIES OF MATTER
PURE SUBSTANCES are substances that are made up of only ONE type of matter. Eg. oxygen, water, gold MIXTURES are substances that are made up of TWO or more types of matter which are mixed but not combined chemically. Eg. breakfast cereal, sugar-water

31. MATTER Mixtures Pure Substances Compounds Solutions Elements
Mechanical
Suspensions

32. PURE SUBSTANCES
There are TWO types of Pure Substances: 1. ELEMENTS are pure substances that CANNOT be separated into simpler substances. Eg. carbon, nitrogen 2. COMPOUNDS are composed of TWO or more elements that are combined chemically. Eg. water, ethanol

33. MIXTURES There are THREE types of Mixtures:
1. SOLUTIONS are when one substance is dissolved in another substance.
Eg. sugar-water, salt-water
2. SUSPENSIONS are when a fluid contains solid particles that will settle out.
Eg. milk, orange juice

34. MIXTURES
3. MECHANICAL MIXTURES are when the parts of the substance can be easily separated out again.
Eg. Raisin Bran, Munchie Mix
Section 1.2 Quiz