Introduction to Ionic Bonds and Compounds

Ionic Bonds

Form when a substance that loses electrons easily (Metal) reacts with a substance that has a higher level of electron affinity (non metal).

Ion

Charged Atom.

Cation

What we call the PAWsitive atom in the Ionic Compound.

Anion

What we call the NEGATIVE atom in the Ionic compound.

Noble Gas Configuration

Each reaches a NOBLE GAS CONFIGURATION (8 Valence electrons).

Ionic Compounds

Structured so that each charge attracts an opposite charge to form a LATTICE shape.

Ionic Properties

Ionic Bonds are VERY difficult to break due to magnetic pull on atoms/ions.

Ionic Compounds at Room Temperature

Ionic Compounds are solid at room temperature.

Conductivity of Ionic Compounds

Do not conduct electricity as solids, but they will in an aqueous solution (dissolved in water).

Monatomic Ions

Made up from only a single atom.

Polyatomic Ions

Made up from 2+ atoms that bond and then remain together as a unit.

Type I Compounds

Group 1 and 2 on the periodic table will ALWAYS be Type I Compounds.

Type II Compounds

Transition metals are ALWAYS Type II Compounds.

Zero Rule

ALL Charges in an Ionic Compound must be equal and opposite each other out to make the molecule neutral.

Naming Ionic Compounds (Type I)

The metal (cation) is listed before the nonmetal (anion).

Naming Ionic Compounds (Type II)

We add roman numerals after the name of the compound to represent the charge it has.

Binary Compounds

Names are given as: The cation needs a roman numeral if it is a transition metal (Type II Compound) to mention its charge.

Example of Cation Naming

Exp: chlorine→Chloride.

Example of Ionic Compounds

1) SnI4 2) K3N 3) HgO 4) RbF 5) NaH 6) CrF2 7) MgBr2 8) MnI2.

Answers to Binary Compounds

1) tin (IV) iodide 2) potassium nitride 3) Mercury (II) oxide 4) Rubidium Flouride 5) sodium hydride 6) chromium (II) fluoride 7) magnesium bromide 8) manganese (II) iodide.