Chemical Bonding

Vocabulary flashcards for chemical bonding lecture review.

Ionic bond

The electrostatic attraction between oppositely charged ions (cations and anions)

Metallic bond

The electrostatic attraction between cations and delocalized electrons

Covalent bond

The electrostatic attraction between the nuclei of two atoms and a shared pair of electrons

Co-ordinate/dative covalent bond

The sharing of a pair of electrons between two atoms where both the electrons in the bond come from the same atom

Electronegativity

The power of an atom that is covalently bonded to another atom to attract the bonding pair of electrons to itself

Bond energy

The energy required to break one mole of that bond in a molecule that is in the gaseous state

Lone pair

Pairs of electrons in the outer shell of an atom that are not involved in bonding

Single covalent bond

One shared pair of electrons bonding two atoms together

Double covalent bond

Two shared pairs of electrons bonding two atoms together

Triple covalent bond

Three shared pairs of electrons bonding two atoms together

Molecular orbital

A combined orbital formed by two atomic orbitals overlapping to form a covalent bond

Sigma (σ) bonds

Covalent bonds involving the end-to-end overlapping of an atomic orbital from one atom to another end of an atomic orbital from another atom

Pi (π) bonds

Covalent bonds involving the side-by-side overlapping of two p orbitals

Instantaneous dipole-induced dipole forces

Attractive intermolecular forces caused by temporary instantaneous dipoles in molecules

Permanent dipole-permanent dipole forces

Attractive intermolecular forces caused by permanent dipoles in molecules

Hydrogen bonding

Observed for H bonded to F, O or N; strongest amongst the intermolecular forces

Bond length

The internuclear distance between two atoms in a covalent bond

Bond polarity

The partial separation of charge when two different atoms are joined by a covalent bond, resulting in an unequal sharing for the bonding pair of electrons