Ionic, Covalent, and Metallic Bonding: Key Concepts and Properties

Ionic bonds

Metals lose electrons to nonmetals.

Elements that create ionic bonds

Metals and nonmetals.

Polyatomic ion

Groups of more than one atom that have a charge.

Properties of ionic compounds

High melting points, usually dissolve in water, and conduct electricity.

Metallic bonding

Nuclei are in a sea of electrons.

Malleability and ductility in metals

The sea of electrons allows the nuclei to move—flatten (malleable) or stretch into wire (ductile).

Melting points of metals

High melting points.

Covalent bond

Nonmetals share valence electrons.

Electronegativity

The ability of an atom to attract electrons in a covalent bond.

Most electronegative elements

F, O, N, Cl.

Elements that do NOT follow the octet rule

Boron and elements in Period 3.

Types of intermolecular forces (IMFs)

Dispersion forces, dipole interactions, and hydrogen bonding.

High boiling point of water

Because of strong hydrogen bonding.

Difference between ionic and covalent solids

Ionic solids are repeating ion patterns; covalent solids are held by intermolecular forces.

Example of ionic compound formula

Li₂S

Example of covalent compound name

Carbon tetrafluoride

Formula for Sodium chloride

NaCl

Name for Fe₂O₃

Iron (III) oxide

Formula for Potassium hydroxide

KOH