Chemisty Compound Nomenclatures

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Chemcial/ionic bonding

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Chemisty Compound Nomenclatures

Covalent Compounds

Definition: Two non-metal atoms sharing electrons to stabilize

Memorize: O3 - Ozone H2O - Water CH4 - Methane NH3 - Ammonia H2O2 - Hydrogen Peroxide

HONC Rule: Tells us the combining capacity of atoms H - Hydrogen + Halogens (form 1) O - Oxygen + Sulfur (form 2) N - Nitrogen + Phosphorus (form 3) C - Carbon + Silicon (form 4)

Diatomic Gases: Bonds with themselves to follow the octet rule (The 7 to make 8)

The 7 gasses: Hydrogen - H2 Oxygen - O2 Nitrogen - N2 Fluorine - F2 Chlorine - Cl2 Bromine - Br2 iodie (sometimes) - I2

Prefixes: Used to create ratios for compounds that aren't ionic

Example: Dinitrogen dihydride = N2H2 Also: Mono Di Tri Tetra Penta Hexa

Acids

Definition: Dissolves in water and ends in (aq)

Binary Acid: Hydrogen (first) + Halogen (Non-metal)

Example: Binary + Classical Name Hydrochloric acid = HCl (aq) Binary + IUPAC Name Aqueous hydrogen chloride

Naming Acids:

Binary + Classical Name = Hydro "___" ic Acid Binary + IUPAC Name = Aqueous Hydrogen "__" ide

Oxyacid + Classical Name = "__" ic acid Oxyacid + IUPAC Name = Aqueous Hydrogen "__" ate

Oxyacid: Hydrogen (first) + polyatomic compound

Example: Oxyacid + Classical Name Sulfuric acid = H2SO4 (aq) Oxyacid + IUPAC Name Aqueous Hydrogen sulfate

Ionic Compounds

Definition: Oppositely changed ions bonding to become stable

Ionic: Metal (first) + Non-metal (ends with 'ide')

Example: Sodium Sulfide = Na2S

Polyatomic Ion: Metal (first) + Polyatomic ion compound (Back of periodic table)

Example: Clacium Chlorate = Ca(ClO3)2