1. Covalent Bond A chemical bond in which electrons are shared. Each atom has access to a full octet (8 electrons). No electrical charges.

2. Diatomic Molecule A molecule made up of two or more of the same atoms. Hydrogen-oxygen- Fluorine-Nitrogen- Bromine- Iodine- Chlorine-

4. Molecular Compounds Any combination of two or more nonmetals

5. Dot Structure for Molecules :Lewis Structures

6. Structural Formulas

7. Molecular Formula C 3 H 6 O 3 carbon atoms. 6 Hydrogen atoms. 1 oxygen atoms.

8. Octet Rule for Covalent Bonds In covalent bonds electrons are shared so that each atoms attain the electron configurations of noble gases. Each atom has access to 8 electrons. All energy levels become filled. The molecule is electrically neutral.

9. Octet Rule for Covalent Bonds

10. Single Bond

11. Multiple Bonds Double BondsTriple Bonds

12. Coordinate Covalent Bonds A covalent bond in which one atom contributes both bonding electrons.

13. Exceptions to Octet Rule

14. VSEPR Theory Valence shell electron pair repulsion. Repulsion between electron pairs causes molecular shapes to adjust so that valence electrons stay as far apart as possible.

15. Molecular Shapes Linear. Trigonal planar. Bent Pyramidal. Tetrahedral. Trigonal bi pyramidal. Octahedral Square planar. T-shaped.

17. Bond Polarity Nonpolar Molecules Electrons are shared equally. Polar Molecules Electrons are shared unequally. The more electronegative atom attracts electrons more strongly,

18. Dipole A molecule that has two oppositely charged ends.

19. Electronegativity Differences and Bond Types. 0.0 – 0.4 = nonpolar. 0.4 – 1.0 = slightly polar. 1.0 – 2.0 = very polar. Great than 2 = ionic bond (e- are completely transferred – no sharing).