Covalent Bonding

Electronegativity

Measure of an atom's electron-attracting ability.

Covalent Bonding

Sharing of electron pairs between two atoms.

Octet Rule

Atoms share electrons to achieve full outer shell.

Diatomic Molecules

Molecules formed from two identical atoms.

Molecular Compounds

Neutral groups of atoms held by covalent bonds.

Bonding Pair

Electrons shared between two atoms.

Lone Pair

Electrons not shared between atoms.

Single Bond

One pair of electrons shared between atoms.

Double Bond

Two pairs of electrons shared between atoms.

Triple Bond

Three pairs of electrons shared between atoms.

Structural Formulas

Diagrams showing shared electron pairs with dashes.

Polyatomic Ions

Groups of covalently bonded atoms with a charge.

Lewis Dot Structure

Diagram representing valence electrons around atoms.

Binary Molecular Compounds

Compounds made of two different nonmetals.

Greek Prefixes

Used to indicate number of atoms in compounds.

Bond Polarity

Describes electron sharing in covalent bonds.

Nonpolar Covalent Bond

Electrons shared equally between atoms.

Polar Covalent Bond

Electrons shared unequally, creating partial charges.

Dipole

Molecule with two poles of opposite charge.

Flammability

Covalent compounds are more flammable than ionic.

Melting and Boiling Points

Covalent compounds generally have low melting/boiling points.

Conductivity

Covalent compounds do not conduct electricity.

Solubility

Covalent compounds do not dissolve well in water.

Central Atom

Least electronegative atom in a molecule.

Hydrogen's Duet Rule

Hydrogen requires two electrons for stability.

Octet Rule Exceptions

Hydrogen and some elements do not follow octet rule.