1. Naming Rules Review

2. Ionic Compounds A combination between: A metal and a non- metal Metals are on the left side of the “staircase” starting at Boron Electrons are donated and accepted

3. Ionic Compounds Which ion goes first? Cation comes first ◦ Metal ◦ Electron donor ◦ Positive ion forms Anion ◦ Non-metal ◦ Electron acceptor ◦ Negative ion forms E.g. Ca +2 (cation) and Br -1 (anion) makes CaBr 2

4. Ionic Compounds How to figure out their formulas OR What ratios elements will combine in? Valence shell electrons ◦ Stable octet desires ◦ Lose or gain electrons ◦ Overall neutral charge required Ca +2 (loses 2 electrons) and Br -1 (gains 1 electron EACH) makes CaBr 2 Ionic charge reflects electron:proton ratio

5. Ionic Compounds How to write their names: Use Periodic Table to find out names from symbols Drop the usual ending from the anion and add “-ide” E.g. NaBr is sodium bromide (not bromine)

6. Ionic Compounds When to use Roman numerals: For cations (metals) that have multiple combining capacities E.g. Iron can donate two or three electrons, so we name them: ◦ Iron (II) ◦ Iron (III)

7. Ionic Compounds Where do Roman numerals go in the name? AFTER the cation (metal) E.g. Iron (II) phosphide

8. Ionic Compounds What is a polyatomic ion? A group of atoms that behave as an anion or cation unit E.g. OH -

9. Ionic Compounds How do polyatomic ions change naming rules? The ending may not be “-ide”, but will be the name of the ACTUAL polyatomic ion E.g. beryllium nitrite is Be(NO 2 ) 2

10. Ionic Compounds The only polyatomic ion to end in “ide”: Hydroxide, OH - E.g. beryllium hydroxide is Be(OH) 2

11. Covalent Compounds A combination between: A non-metal and a non-metal Electron sharing

12. Covalent Compounds How are the naming rules different than ionic compounds? Names use prefixes to indicate the formula subscripts ◦ Mono- (1) ◦ Di- (2) ◦ Tri- (3) ◦ Tetra- (4) ◦ Penta- (5) ◦ Hexa -(6) ◦ Etc.

13. Covalent Compounds E.g. Carbon tetraflouride is CF 4 The prefix “mono-” not always used (see above example), but can be useful for differentiating between two compounds. ◦ E.g. Carbon monoxide and carbon dioxide