1. Chapter 3 Classification of Matter
Objectives:
Define and give examples of 3 states of matter (3.1 & 3.2)
Distinguish between substances and mixtures (3.3 & 3.12)
Understand what elements are ( )
Distinguish between metals, nonmetals and metalloids (3.8)
Define compounds and diatomic molecules (3.9 & 3.10)
Be able to write chemical formulas (3.11)

2. What is Matter? Anything that has mass and occupies space
Composed of atoms
Exists in three states on earth
Exists in fourth state in space

3. Solids Definite Particles tightly packed Crystalline –
Amorphous solids –

4. Liquids
Definite volume
Not a
Particles have
Particles can

5. Gases
Indefinite volume No
Particles have
Particles

7. Substances and Mixtures
Pure Substance: a particular kind of matter with a definite, fixed composition
Mixture:

8. Matter Pure substances (homogeneous composition)
Mixtures of two or more substances
Elements
Compounds
Solutions (homogeneous composition – one phase)
Heterogeneous mixtures (two or more phases)
Figure 3.2 (page 48)

9. Types of Mixtures Heterogeneous mixtures Homogeneous mixtures
Chocolate chip cookies; granite
Homogeneous mixtures

10. Separating Mixtures Do NOT cause chemical changes
Heterogeneous Mixtures

11. Separating Mixtures
Homogeneous Mixtures

12. Separating Mixtures
Homogeneous Mixtures

13. Separating Mixtures
Homogeneous Mixtures

14. Pure Substances
Elements
Compound

15. Elements ~111 presently known elements At room temperature:
Figure 3.3 – distribution of elements in the

16. Elements
Names of the elements
Greek
Latin
Location where discovered

17. Elements Arranged in the Periodic Table (inside front cover) Symbols
Some symbols are Latin/Greek name (Table 3.4)

18. Elements
Classification
Metal
Nonmetal
Metalloid
See Table 3.5

19. Elements Metals: Usually solid at room temperature High luster
Malleable
Usually don’t combine with each other

20. Elements Nonmetals: Solids ( ); Liquid ( ); Gases (all others)
Poor conductors
Low melting point;
Will combine
Some found uncombined in nature

21. Elements Metalloids Have properties of
Some used for semiconductors in electronics

22. Compounds Two or more elements New properties
Can be chemically separated

23. Compounds
Molecular
Held together with
Molecule:
Water is an example

24. Compounds
Ionic
Ion:
Cation –
Anion –
Held together by ionic bond –

25. Compounds
Diatomic Molecules
Always only 2 atoms
7 naturally occurring

26. Chemical Formulas
Abbreviations for compounds
Sodium Chloride (NaCl)

27. Chemical Formulas Subscript indicates # of atoms present
H2O has 2 Hydrogen atoms and 1 Oxygen atom
NaOH has

28. Chemical Formulas
Parentheses are used to show when a compound contains more than one group of atoms that occurs as a unit

29. Chemical Formulas Show only number and kind of atom
Do not show arrangement of the atoms or how chemically bonded