Lecture notes: CHEM103– November 4, 2008

LECTURE OUTLINE:

1. nomenclature (naming) of ionic compounds

a. how to write a chemical formula for an ionic compound

b. how to name an ionic formula

c. polyatomic ions (made from non-metals) – the ones you NEED to remember

d. acids and bases: recognizing, identifying and naming

2. going from symbols to names of elements

a. metals

b. non-metals

3. going from names to symbols of elements

a. how to determine the charge of an ion from the name

b. periodic location OR Roman numerals

4. combining to form compounds (formulae)

a. metal always goes first

b. exceptions for HYDROGEN (non-metal but forms cation OR anion species)

c. balancing charge

Nomenclature examples:

aluminum oxide

calcium fluoride

potassium sulfide

FeBr₃

Mn₂O₃

Na₂HPO₄

tin (IV) chloride

potassium carbonate dihydrate

ammonium perchlorate

More examples:

barium sulfate; ammonium acetate, copper (I) chloride; zinc (II) perchlorate, sodium phosphate, calcium phosphate

copper (I) phosphide (s) Cu₃P, copper (II) chloride CuCl₂,

tin (II) chloride SnCl₂, tin (IV) hydride SnH₄,

lithium hydride LiH, hydrogen chloride (hydrochloric acid) HCl

RULES FOR NAMING ACIDS:

What’s an acid? A combination of a hydrogen (metal/non-metal?) with non-metal(s)

hydrohalides (acids)

HCl

HBr

HI