Ch U6b HO Name

(Keep as notes) Naming Chemical Cmpds Pd.

1. Ionic Compounds. -- this has already been discussed in great detail. Basically, you simply name the two ions involved. If the cation involved has more than one possible charge, you must indicate the oxidation # in the name by using the roman numeral Stock naming system, or the classical system with the latin name and ending.

2. Hydrates. ---Some ionic compounds will absorb water from the air to form loose bonds with the compound. These hydrates have different properties than the anhydous (without water) form.

Writing formulas: you simply put the formula of the ionic compound followed by a "" and xH₂O. "x" being the number of water molecules that bond per formula unit.

Naming hydrates: write the name of the ionic compound as normal, then add the correct numerical prefix in front of the word "hydrate" to indicate the number of water molecules bonded per formula unit.

anhydrous compound	formula of hydrate	hydrate name
CuSO₄	CuSO₄ 5H₂O	copper(II) sulfate pentahydrate
BaCl₂	BaCl₂ 2H₂O	barium chloride dihydrate
		calcium chloride dihydrate
	Li₂SO₄ H₂O
		sodium sulfide nonahydrate
	Ni(NO₃)₂ 6H₂O

Numerical Prefixes
1		6
2		7
3		8
4		9
5		10

3. Binary Molecular compounds -- these are compounds consisting of two elements covalently bonded together. (ex SO₂, CO, NH₃) The name consists of two words that reflect the elemts involved and the number of atoms.

First Word: numerical prefix + name of element * NOTE: for the first word, if only one atom is present DO NOT Use Prefix (see CO₂ below)

Second Word: numerical prefix + name of element with "ide" ending.

Molecular Formula	Name of Compound
N₂O	dinitrogen monoxide
CO₂	carbon dioxide
	dinitrogen tetrahydride
CCl₄
N₂O₅
	diarsenic pentasulfide
NO
	dihydrogen monoxide
SO₃