1. Naming and Writing Compounds Pg. 65

2. Ionic Compounds • 1. Cation goes first, then anion • Ex. NaCl • 2. The charges on each element are switched and become the subscript of the other element. • Na+1 + Cl-1 • 3. Ionic compounds must have an overall charge of 0. • 4. If the charges are the same, they cancel out. • NaCl • 5. Naming- the cation is written the same. The first syllable of the anion is kept and –ide is added to the end. • Ex. Sodium Chlorine = Sodium Chloride

3. Transition Metals • Charges of transition metals are shown in paranthesis. • Ex. Fe2O3 = Iron (III) oxide

4. Determining Charge • To determine the charge of an element, look at the subscript of the other element. • Ex. FeO • You know that oxygen has an oxidation state of -2. • Since there are no subscripts shown, the charges have been canceled out. Therefore, Fe must have a charge of __________.

5. Naming Covalent Compounds • Numerical prefixes are used in covalent compounds to tell how many atoms of each there are. • Ex. Carbon dioxide (di=2) CO