Chemical Nomenclature

Ionic compounds

AKA formula units

Composed of cations and anions

Binary ionic compounds

Composed of two monoatomic ions

Polyatomic ionic compounds

Polyatomic ions act as a group and are held together by covalent bonds

Hydrates

Ionic compounds with water as part of the crystal

Formula ⋅ # H2O

6 ionic compound naming rules

1. Overall charge is 0

2. No prefixes in ionic compounds except naming hydrates

3. Written in the simplest ratios

4. Cation is written first

5. Parenthesis are used only when more than one polyatomic ion are present

6. Use roman numerals only when needed

Binary molecular compounds

Composed of two nonmetals

Represented by molecule particles (includes organic molecules & acids)

Held together by covalent bonds (sharing electrons)

Prefix system used to indicate # of atoms

Formulas identify the number of each atoms present (do not reduce)

Ammonia

NH3

Water

H2O

Hydrogen peroxide

H2O2

Diatomic elements

Have No Fear Of Ice Cold Beer

Organic molecules

Alkanes and alcohol

Molecules that contain carbon

Use hydrocarbon names (not prefixes)

4

A carbon atom contains __ valence electrons and forms __ covalent bonds with other atoms

Alkane formula

R-H

C(n)H(2n+2)

Alcohol formula

R-OH

C(n)H(2n+1)OH

Hydrocarbon names 1-4

Meth, eth, pro, bu

Methane

CH4

Methanol

CH3OH

Acids

Represented by covalent molecule that produces H3O+ in water

Acid naming rules

1. Anion ends in -ide: "Hydro" as prefix and -ic as suffix followed by "acid" (e.g. Hydrochloric acid).

2. Ends in -ite: -ous as suffix followed by "acid" (e.g. Phosphorous acid).

3. Ends in -ate: -ic as suffix followed by "acid" (e.g. Nitric acid).

Mono-

1

Di-

2

Tri-

3

Tetra-

4

Penta-

5

Hexa-

6

Hepta-

7

Octa-

8

Nona-

9

Deca-

10