Naming Compounds and Chemical Formulas

Bonding – Octet Rule

Ionic CovalentStarts with a metal Starts with a nonmetalTransfer of electrons Shares electronsFormula unit MoleculesStrong bond Weak bondHi melting/boiling points Lo melting/boiling

pointsHard, brittle solids Soft solids or gasesGood conductors Poor conductorsCrystal structures VSEPR shapesCations (+) and anions (-)

Polar or nonpolar bonds

Nomenclature

Roman numeral = charge

Metals always (+) Written 1st

Nonmetals (-) in ionic bonding Exception NH4

1+ (ammonium ion)

Endings

ide = original element (nonmetal)

ate and ite = polyatomic ions 2 exceptions: CN1- (cyanide) and OH1-

(hydroxide)

Don’t confuse valence # with charge. Valence # is the number of electrons in

the outer shellCharge is the transfer of electrons

Acid endings

Hydro --- ic acid Hydro --- ic becomes ide = original element

(nonmetal)

ous acid ous becomes ite polyatomic ion

ic acid ic beomes ate polyatomic ion

Examples of Acids

Hydrosulfuric acid H2S

Sulfurous acid H2SO3

H3P Hydrophosphoric

acid

H3PO4

Phosphoric acid

Examples of Covalent Compounds

Disulfur hexafluoride S2F6

Carbon monoxide CO

P3O Triphosphorus

monoxide

C3Cl8 Tricarbon

octachloride

Examples of ionic compounds Magnesium sulfide

MgS

Iron (III) sulfate Fe2(SO4)3

Na2O Sodium oxide

Cu(NO3)2

Copper (II) nitrate