An Introduction to Chemistry

• Important biological elements– Carbon– Oxygen– Nitrogen– Hydrogen– Sulfur– Na– K

II. Atomic Structure

• A. Definition• B. Analogy of

structure• C. Subatomic

particles– 1. Protons– 2. Neutrons– 3. Electrons

III. Electron orbitals

• A. Location• B. Maximum

number of electrons in an orbital

• C. Orbital filling• D. Examples

– 1. H– 2. C– 3. Na– 4. Si

III. Electron orbitals

• E. Valence electrons– 1. Definition– 2. Involved in chemical bond formation– 3. Determines chemical properties of the

atom– 4. Elements with the same number of

valence electrons have similar chemical properties

III. Electron orbitals

• E. Valence electrons– 5. gaining and

losing energy

IV. Periodic table

An atom with an atomic number of 13 and a mass of 22 possesses ____ electrons.

79%

0% 0%0%

21%

1. 13

2. 22

3. 9

4. 3

5. The answer cannot be determined

An atom with an atomic number of 13 and a mass of 22 possesses ____ valence electrons.

5%11%

16%

68%

1. 2

2. 3

3. 8

4. 13

V. Chemical Bonding

• A. Octet Rule– 1. Definition– 2. Noble Gases

V. Chemical Bonding

• B. Ionic Bonding– 1. Example

• 11Na

• 17Cl

V. Chemical Bonding

• B. Ionic Bonding– 2. Definition

Ionic bonding

What is the equation of the compound formed when 20Ca and 17Cl combine by ionic bonding?

19%

0%

63%

19%

1. Ca2Cl

2. CaCl

3. CaCl24. The answer

cannot be determined

V. Chemical Bonding

• C. Covalent bonding– 1. Definition– 2. Example of nonpolar covalent– 3. Example of polar covalent bonding

Nonpolar Covalent

Polar Covalent Bond