1. Properties of Matter
Chapter 16

2. Properties
Extensive = Characteristic of matter in which the amount of the material affects the property
Intensive = Characteristic of matter in which the amount of the material does not affect the property

3. List examples of extensive and intensive properties

4. Measuring Matter Length Meter (m) Volume Mass Temperature density
Measurement
Unit
instrument
Length
Meter (m)
Meter stick, ruler, odometer
Volume
Liter (l) or cubic meter cm3
Ruler or graduated cylinder
Mass
Gram (g) or kilogram (kg)
Scale or balance
Temperature
Celsius (C0) or Kelvin (K)
Thermometer
density
g/cm3 or g/ml
Balance and ruler or graduated cylinder

5. Classifying Matter: matter can be classified into two main types
Mixture
contains more than one kind of matter that can be separated by physical means
Pure Substances
is matter that cannot be separated by physical means
sugar
Trail mix

6. Two Types of substances
Elements
has one kind type of atom
examples:
helium (He)
carbon (C)
hydrogen (H)
oxygen (O)
Compounds
a substance that contains more than one type of atom
examples:
H2O (pure water)
NaCl (sodium chloride)

7. Matter
Examples of elements:
mercury
gold
aluminum
iodine

9. Examples of pure substances that are compounds
NaCl = table salt
Water =H2O
Sugar = C6H12O6

10. Basic units of substances are always in motion
Atom
is the smallest possible particle of an element
Molecule
is the smallest particle of the compound that retains the properties of the compound

11. Types of mixtures Heterogeneous mixture
the composition is not uniform (different)
examples:
chicken noodle soup
mixed nuts
soil
Homogeneous Mixture
The composition is uniform (same)
examples:
salt water
tap water
brass

12. What type of mixture is it?
homogeneous
heterogeneous
Salt water

13. Solutions, Suspensions, and Colloids
It isn’t always easy to tell the difference between a homogeneous or heterogeneous mixture.
Based on the size of its largest particles, a mixture can be classified as a solution, a suspension, or a colloid.

14. Solutions
When substances dissolve and form a homogeneous mixture, the mixture that forms is called a solution.

15. All mixtures can be separated.
Methods to separate mixtures
1. Sorting
2. Filtering
3. Heating
4. Cooling
5. distillation

16. Matter Substances mixtures Compounds elements Heterogeneous mixture
Homogeneous mixture
elements

17. Two types of Properties of Matter
1. A physical property is any characteristic of a material that can be observed or measured without changing the composition of the substance in the material.
A chemical property can be observed only when the substances in a sample of matter are changing into different substances.

18. Physical Properties Viscosity= Resistance of a liquid to flowing
High viscosity

19. Physical Properties of matter
Conductivity = the ability of matter to transfer heat or electricity

20. Physical Properties
Malleability is the ability of a solid to be hammered without shattering.
diamond
Hardness is used to compare two materials. If a material can scratch another then it is harder.

21. Physical Properties
Melting point is the temperature at which a substance changes from a solid to a liquid (Water in the form of ice melts at 00C)
Boiling Point is the temperature at which a substance boils. (water boils at 1000C)

22. Physical Properties of Matter
Density is the ratio of the mass to volume of a substance.

23. Chemical Properties
A chemical property is any ability to produce a change in the composition of matter.
Chemical properties can be observed only when the substance in a sample of matter are changing into different substances.

24. Observing Chemical Properties
Flammability is a material’s ability to burn in the presence of oxygen.

25. Observing chemical properties
The property that describes how readily a substance combines chemically with other substances is reactivity.
Examples:
Rusting
Chemical reaction

26. Indentifying Chemical Change
Common types of evidence for a chemical change are
1. color
2. production of gas
3. formation of a precipitate
4. Thermal energy change

27. Identifying a chemical change

28. States of Matter Solid has a definite shape and definite volume
molecules vibrate slow but cannot switch places with other molecules

29. States of Matter Liquid has a definite volume but no definite shape
Molecules move faster and slip out of position

30. States of Matter Gas has no definite shape or volume
molecules move so fast that they bounce out of the liquid state and become a gas.

31. Temperature= the average energy of the molecules

32. Changing States of Matter
Melting point
temperature at which it changed from solid to liquid
Boiling point
temperature at which it changes from a liquid to a gas

33. Changing state of matter
Evaporation
fast-moving molecules in a liquid can escape to become a gas
cooling because it take the energy (heat) away from the substance
Condensation
molecules in a gas slow down and change into a liquid

34. Changes in State of Matter
Sublimation
when a solid changes directly from a solid to a gas