L7 - Ionic and Covalent Bonding

Flashcards covering key vocabulary and concepts related to ionic and covalent bonding from the lecture notes.

Ionic Bond

Formed through the transfer of electrons between two species, creating positive and negative ions (cations and anions) which then attract each other.

Metallic Bonding

Electrons are delocalized, meaning they can float around amongst the solid space of metal atoms, allowing all atoms to have sufficient electrons for stability.

Covalent Bonding

Involves the sharing of electrons between two non-metals to achieve a full valence shell and stability.

Ionization Energy

The amount of energy required to either lose or gain an electron. It substantially increases with each subsequent electron removed due to increasing net positive charge.

Lewis Diagram

A representation where the chemical symbol represents the atom, and dots represent valence electrons.

Octet Rule

The tendency of atoms to prefer to have eight electrons in their valence shell. A useful but not perfect guide for predicting bonding.

Internuclear Distance

The distance between the nuclei of two bonded atoms, which affects the energy and stability of the bond. Each bond has a differing internuclear distance and energy.

Bonding Pair

A pair of electrons shared between two atoms in a covalent bond, effectively contributing to the valence shell of both atoms.

Lone Pair

A pair of valence electrons that are not involved in bonding and remain associated with a single atom.

Valence Electrons

The number of electrons in the outermost shell of an atom, which participate in bonding.

Valence

The number of bonds an atom needs to form to reach a noble gas configuration or the size of the charge formed if it forms an ion.

Hydrocarbon

A compound made up of only carbon and hydrogen atoms.

Polyatomic Ion

An ion composed of multiple atoms covalently bonded together that carries an overall charge.

Double Bond

A covalent bond in which two atoms share two pairs of electrons (four electrons total).

Triple Bond

A covalent bond in which two atoms share three pairs of electrons (six electrons total).