1. Unit 5 Properties of Matter
Section 10.1 and 12.1
The Nature of Matter

2. Level 3
Can identify chemical and physical properties of matter. And give examples of each.
Can identify whether a change is either a chemical or physical change.
Can distinguish between pure substances and mixtures.
Can identify mixtures as either Homogeneous or Heterogeneous.
Can, based on chem. formulas, identify a pure substance as either an element, compound or molecule.
Can state whether a material has high or low values of the below properties: TERMS
Lab: when given an object can determine its volume.
Can determine the density of an object from the slope of a mass vs. volume graph.
Can identify which term (accuracy, precision and resolution) applies to a given lab/measurement situation or example.
Can give examples of objects that have a mass of 1gm, a volume of 1ml and a length of 1cm.

3. Density (D = m/v) Malleability Elasticity Hardness Odor Conductivity Tensile Strength Thermal Expansion Brittleness Viscosity Color

4. Matter – anything that has mass and volume
Matter is made of tiny particles called atoms.
Democritus and Leucippus– Greek Philosophers – 1st to use term atomos.
Brownian Motion – all atoms move in a jerky motion

5. Matter Substance Mixture Compound Element
Can NOT be broken down by physical means.
Compound
Element

6. SUBSTANCE Element Compound Composed of elements joined chemically
Composed of atoms
Can NOT be broken down
Periodic Table
One capital letter
Compound
Composed of elements joined chemically
Two or more capital letters
Exception: Molecules
O2, H2

7. Matter Substance Mixture Homogeneous mixture Heterogeneous mixture
CAN be broken down by physical means.
Homogeneous mixture
Heterogeneous mixture

8. MIXTURES Homogeneous Heterogeneous
A mixture that is the same throughout
Each sample is the same
Examples:
Salt water
Rubbing alcohol
Closed can of pop
Air
Heterogeneous
A mixture in which the samples are not the same throughout.
Different proportions
Examples:
Cup of sandy water
Water with ice cubes
Open can of pop

9. Ways of Separating Mixtures
Physical Means
Sorting
Filtering
Heating / Evaporation
Cooling
Chromatography
Magnetism
Chemical Means
Electrolysis
Chemical reactions
Distillation

10. Chemical and physical properties

11. Matter Every element/compound is unique in some way from all others.
If you know enough about a substance, you can figure out what it is.
If you know what a substance is, you can know all types of things about it.

12. Matter All matter has 2 types of properties: Physical properties
chemical properties.

13. Physical properties
A physical property is a characteristic of a substance that can be observed without changing the substance into another substance.
(You can see it without changing what you’re looking at into something else.)

14. Physical Properties Physical properties can be extensive or intensive:
Extensive properties depend on the amount of a substance that you have.
Intensive properties don’t depend on how much you have.

15. Physical Properties - Examples
Examples of extensive physical properties include:
Volume
Mass
Weight
Size

16. Physical Properties - Examples
Examples of intensive physical properties include:
Density
Melting point
Boiling point

17. Physical Properties - Examples
Other physical properties include:
Color
Hardness
Odor
Taste
State of matter
Texture
Luster (shine)
Flexibility
Heat conductivity
Electrical conductivity
Solubility (ability to dissolve in water.)
Shape
Viscosity
Ductility
Malleability

18. Chemical properties
A Chemical property is a characteristic of a substance that can only be observed by changing it into a different substance.

19. Chemical properties - Examples
Examples of chemical properties include:
The ability to burn
Ability to tarnish
Ability to rust
Ability to decompose
Ability to react with other chemicals
Instability
Ability to do acid/base reactions

20. Element abundance
The most common element in the universe is Hydrogen (about 75%), and Helium (about 25%).
The most common element on Earth is Oxygen (46.6%), and Silicon (27.7%).
The most common element in your body is Oxygen (65%), and Carbon (18%)

21. Chemical and physical changes

22. Physical Change
A Physical change is a change in a substance that does not change what the substance is.

23. Physical Change - examples
Examples of physical change include:
Change in shape
Change in size
Change in phase
Melting (solid to liquid)
Boiling (liquid to gas)
Evaporation (liquid to gas)
Condensation (gas to liquid)
Freezing (liquid to solid)
Sublimation (solid to gas)
Deposition (gas to solid)

24. Physical Change Physical changes might be caused by: Grinding Cutting
Crushing
Bending
Breaking
Heating/cooling
(change in phase)
squishing

25. Physical Change
Evidence that a physical change has occurred might include:
Change in shape
Change in form
Change in size
Change in phase (This is always a physical change!)
Physical changes are usually reversible

26. Physical change
What could you do to these items to cause a physical change to occur?

27. Chemical change
A chemical change is a change in which a substance is changed into a different substance. (You’ve changed what it is.)

28. Chemical change Examples of chemical changes include: Burning Rusting
Tarnishing
Decomposing
Polymerization

29. Chemical change
Chemical changes occur when a chemical reaction causes bonds between atoms to break or to form.

30. Chemical Change: Evidence
Evidence that a chemical change has occurred might include:
A color change
An odor change
Formation of a precipitate (you mix two liquids and make a solid)
Gas is formed (bubbles)
Changes in physical properties.

31. Physical and Chemical change
During a chemical change energy can be released in the form of:
Heat
Light

32. Chemical change – Chemical reactions
When a chemical change occurs, energy is either released or absorbed.

33. Physical and Chemical change - heat
A chemical reaction that releases energy in the form of heat is called exothermic.
Heat comes OUT
Exo = out
Thermic = heat
It will feel HOT.

34. Physical and Chemical change - heat
A chemical reaction that absorbs energy in the form of heat is called endothermic.
Heat goes IN
Endo = in
Thermic = heat
It will feel COLD