Chemisty Compound Nomenclatures

Definition:
Oppositely changed
ions bonding to become stable

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

Example:
Clacium Chlorate = Ca(ClO3)2

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

Example:
Sodium Sulfide = Na2S

Definition:
Dissolves in water and
ends in (aq)

Oxyacid:
Hydrogen (first) +
polyatomic compound

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

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

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

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

Definition:
Two non-metal atoms sharing
electrons to stabilize

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

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

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

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)