1. Matter, Atomic Structure-Periodic Table
ISCI 2002
Spring 2009

2. Matter Anything that has mass and occupies space
Matter – all substances
Properties of matter
1. macroscopic
2. microscopic

3. Classification of Matter
Heterogeneous Matter
mixture
Peanut butter
Pure substance
Ice floating in water
Homogeneous Matter
gasoline
Pure substances
Sugar

4. Atomic Structure 1. Size and general structure 2. Parts - Atom
Small; cannot be seen with visible light
2. Parts - Atom
Nucleus
Protons and neutrons
Energy levels / electron clouds
Electrons
3. Atoms are mostly empty space
Nucleus determines the mass of the atom

5. Subatomic Particles Atomic mass unit (amu) – hydrogen atom (1 amu)
Electron mass = 1/2000 amu

6. Nucleus of the Atom 1. Proton + Neutron 2. Electrons Mass of the atom
1/2000 of one amu
Not included in the mass

7. Atomic Number Atomic Number – Periodic Table
Number of protons in an atom
Protons = electrons
Using your periodic table determine the number of protons and electrons in the following atoms
Sodium
Chlorine
Nitrogen
Lithium

8. Number of neutrons and protons
Combined mass – Mass Number
Atomic Weight
Average of all the isotopes in an element.
Carbon = amu
Combination of three carbon isotopes

9. Isotopes
1. Elements are composed of several different types of the same atom
Same type of atoms with differing number of neutrons
2. Carbon
3 isotopes
Carbon 12, 13, and 14
Calculating neutrons

10. Using the mass number and atomic number to determine the subatomic particles
The atomic number equals the number of protons. Protons always equal the number of electrons!

11. Periodic Table 1. Symbol 2. Atomic Number
Number of protons
3. Atomic Mass-(Average Atomic Mass)
Mass of neutrons and protons
4. Group
Vertical
5. Period
Horizontal

12. Periodic Table

13. Periodic Table

14. Groups and Periods Alkaline Earth metals Noble Alkali Halogens
Transition Metals

15. Drawing Planetary Models of Atoms
Energy Level (Electron Shell)
Orbitals
Max Number of electrons
Valence Electrons 1 S 2
S and P 8 3
S, P, D 18 4
S, P,D 32 5
S, P,D,F 50
Orbital
Maximum Electrons S 2 P 6 D 10 F 14

16. Drawing Planetary Models
1. Look at the atomic number
2. Determine the total number of electrons
3. Draw each energy level with correct number of electrons
Next – Dot Diagrams
Draw only the ‘valence’ electrons
S and P - orbitals only

17. Chemical and Physical Properties
Appearance – hard or soft; dull or shiny; color
Density; melting point and boiling point
Chemical Properties- describes changes of composition the substance undergo’s during a chemical change
What is required to bring about the change
Temperature, heat, number of electrons, etc.

18. Chemical and Physical Properties
Extensive Property
Depends on the ‘quantity’ of matter in a sample
Cannot be used to characterize a type of matter
Volume, mass
Intensive Property
Property shared by all examples of a specific type of matter
Density (m/v); color; melting point; solubility; acidic or alkaline
The density of water is 1.0 g/cm3