An Introduction to Chemistry

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. • 13 • 22 • 9 • 3 • The answer cannot be determined

9. An atom with an atomic number of 13 and a mass of 22 possesses ____ valence electrons. • 2 • 3 • 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. 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