2. An Introduction to Chemistry
Important biological elements
Carbon
Oxygen
Nitrogen
Hydrogen
Sulfur Na K

3. II. Atomic Structure A. Definition B. Analogy of structure
C. Subatomic particles
1. Protons
2. Neutrons
3. Electrons

4. 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

5. 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

6. III. Electron orbitals E. Valence electrons
5. gaining and losing energy

7. IV. Periodic table

8. An atom with an atomic number of 13 and a mass of 22 possesses ____ electrons.9 3
The answer cannot be determined

9. An atom with an atomic number of 13 and a mass of 22 possesses ____ valence electrons.8 13

10. Chemical Bonding
A. Octet Rule
1. Definition
2. Noble Gases

11. V. Chemical Bonding
B. Ionic Bonding
1. Example
11Na
17Cl

12. V. Chemical Bonding
B. Ionic Bonding
2. Definition

13. Ionic bonding

14. The answer cannot be determined
What is the equation of the compound formed when 20Ca and 17Cl combine by ionic bonding?
Ca2Cl
CaCl
CaCl2
The answer cannot be determined

15. V. Chemical Bonding C. Covalent bonding 1. Definition
2. Example of nonpolar covalent
3. Example of polar covalent bonding

16. Nonpolar Covalent

17. Polar Covalent Bond