This is a PowerPoint from when I was teaching chemistry. I taught chemistry for 5 years at a local private high school here in Erie, Pa.

1. Chapter 6: Chemical Bonding 6.2 – Covalent Bonding and Molecular Compounds

2. Molecule – neutral group of atoms that are held together by covalent bonds Molecular Compound – chemical compound whose simplest units are molecules

3. Chemical Formula – indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical scripts Molecular Formula – shows the types and numbers of atoms combined in a single molecule of a molecular compound.

4. Diatomic Molecules – molecules containing only two atoms. Br2 Cl2 F2 H2 I2 N2 O2

5. Octet Rule -> Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level. Electron-Dot Notation – notation in which only the valence electrons of an atom of a particular element are shown. Dots are placed around the elements symbol.

6. One Valence Electron X

7. Two Valence Electrons X

8. Three Valence Electrons X

9. Four Valence Electrons X

10. Five Valence Electrons X

11. Six Valence Electrons X

12. Seven Valence Electrons X

13. Eight Valence Electrons X

14. Lewis Structure – formulas in which atomic symbols represent nuclei and inner shell electrons — covalent bonds : unshared pair of electrons Lone pair (unshared pair) – pair of electrons that is not involved in bonding and that belongs exclusively to one atom.