1. Covalent Bonding Sharing is caring

2. Types of Bonds Review Metallic Ionic Covalent Transfer Electrons Delocalized Electrons (sea of e - ) Share Electrons Molecule Unit Cell

3. Electronegativity and bond types Another way to usually tell whether a bond is ionic or covalent is with electronegativities Electronegativity (Page 194)– the tendency of an atom to gain electrons in a chemical bond. If the difference between the electronegativities is large, the bond tends to be ionic. If it is small, it tends to be covalent. Compounds can have both, but usually show one type more than the other chemically, usually ionic).

4. Naming Covalent Compound

5. Types of Covalent Compounds Diatomic molecules (twins): ________________________________ NEVER FOUND AS SINGLE ATOMS if “alone” Their names are just the name of the element H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 There are seven diatomic molecules

6. Binary Molecular Compounds ___________________________(no metals or ions) i.e. Does not start with an H. Steps to name compounds a._________ _________ - use entire name b._________ _________ - change ending to –ide c.Prefixes used to indicate _________ of atoms of each p. 832 Only time that no prefix is used is if the first is a one Examples: CCl 4 – As 2 O 3 – Non-metals with no H + Name first Namesecond number tridi tetrachloridecarbon arsenicoxide

7. The Prefixes Mono-monocle Tri-tricycle Penta-pentagon Octa- octopus Tetra-Tetris Di-Dialogue

8. Acids Always begin with ______ Two Types: _________ and ___________ H+H+ oxyacidbinary Remember: The number of hydrogen atoms in the acid equals the charge of the anion

9. Binary Acids Binary Acids - ______ but no _______ Steps to name compounds a.Use prefix - _________ b.Root of second element plus suffix - _________ followed by the word acid Example: HCl - H+H+ O hydro -ic hydrochloricacid

10. Oxyacids – has a ________________, so most have ___ Steps to name compounds Identify polyatomic ion p. 178 a.Use root of anion, change suffix ending and word acid a.Suffix rules: ends in ate  change to _________ b. ends in ite  change to _________ Example: HNO 3 - polyatomic ion -ic -ous nitricacid O

11. Hydrocarbons a compound containing carbon and hydrogen Named using prefixes that correspond to the number of carbons in the compound. 1 – meth 2 – eth 3 – prop 4 – but After this it used the “normal” prefixes

12. Hydrocarbons Ending refers to the type of functional group found in the compound. The simplest hydrocarbon ends in -ane which means that the hydrocarbon only has single bonds and the number of hydrogen atoms equal 2(Carbon atoms)+2.

13. Practice FormulaType of Covalent BondName PCl 5 HI N2N2 C2H6C2H6 H 3 PO 4 HClO 2 N2H4N2H4 Dinitrogen tetrahydride Phosphic acid Nitrogen Hydroiodic acid Binary Molecular Diatomic Binary Acid Phosphorous pentachloride Binary Molecular Oxyacid Chlorous acid Hydrocarbonethane