1. Chapter 2
Matter and Change

2. Matter and Change 2.1 – Properties of Matter 2.2 – Mixtures
2.3 – Elements and Compounds
2.4 – Chemical Reactions

3. Objectives
Differentiate and give examples of extensive and intensive properties
Distinguish the three primary states of matter
Distinguish physical from chemical change.
Classify mixtures as homogeneous or heterogeneous.
Distinguish between elements and compounds.
Memorize the 24 most encountered elements names and symbols.
Distinguish chemical from physical properties

4. Extensive Properties Mass - amount of matter of an object.
Volume - the space occupied by an object.
Extensive Property - a property that depends on the amount of matter in a sample.

5. Intensive Properties
a property that depends on the type of matter, not the amount of matter.
Example:
Hardness of a rock
Boiling point

6. Substances
Matter that has a uniform and definite composition

7. Physical Properties
Can be observed or measured without changing the composition of a substance
Can be used to identify substances
Examples:
Hardness
Color
Malleability
Boiling Point

8. Identifying Substances

9. Physical Changes
Some properties of the material may change, but the composition stays the same
Can be reversible or irreversible
Examples:
Boil
Freeze
Break
Crush

10. States of Matter Solid Liquid Gas Definite shape and volume
Particles are highly organized and packed close together
Not easily compressed
Liquid
Definite volume; takes the shape of its container
Particles are tightly packed together, but arranged randomly
Gas
Takes the shape and volume of its container
Particles are spaced very far apart
Easily Compressed

11. States of Matter

12. Vapor
the gaseous state of a substance that is generally a liquid or solid at room temperature

13. Classification of Physical Changes
some properties of a material change
the composition of the material remains the same

15. 24 Common Elements Carbon C Aluminum Al Copper Cu (from cuprum)
Fluorine F
Bromine Br
Iron
Fe (from ferrum)
Hydrogen H
Calcium Ca
Lead
Pb (from plumbum)
Iodine I
Chlorine Cl
Mercury
Hg (from hydrargyrum)
Nitrogen N
Helium He
Potassium
K (from kalium)
Oxygen O
Lithium Li
Silver
Ag (from argentum)
Phosphorus P
Magnesium Mg
Sodium
Na (from hatrium)
Sulfur S
Silicon Si
Tin
Sn (from stannum)

17. Mixture physical blend of two or more components
heterogeneous mixture – composition is not uniform throughout (2 or more phases/part)
homogeneous mixture – the composition is uniform throughout is a (single phase/part)
Also known as a solution.

18. Separating Mixtures
Filtration - separates a solid from the liquid in a heterogeneous mixture
Distillation – a liquid is boiled to produce a vapor that is then condensed into a liquid.

19. Elements vs. Compounds
element – the simplest form of matter that has a unique set of properties.
compound – a substance that contains two or more elements chemically combined in a fixed proportion.
Properties of the individual components are different than the properties of the compound

20. Distinguishing Substances & Mixtures
The flow chart summarizes the process for classifying matter. Any sample of matter is either an element, a compound, or a mixture. Interpreting Diagrams What is the key difference between a substance and a solution?

22. Chemical Reactions Chemical Property
ability of a chemical to undergo a chemical change
Reactant – substances that undergo change
Products – New substances
Chemical Change – a substance changes composition and becomes something different

23. Chemical Changes Evidence of a change
produces matter with a different composition than the original matter
Evidence of a change
Energy Transfer
Color Change
Production of gas
Production of a precipitate
Energy Transfer – heat (gets hot or cold), light, sound
Precipitate – a solid that settles out of solution

24. Law of Conservation of Mass
Matter is neither created or destroyed; it is only changed
Mass of the products = Mass of the reactants