Unit 4.1 Ionic & Covalent Bonding

Ionic Bonds

Bonds formed from the transfer of electrons from a metallic element to a non-metallic element.

Cation

A positively charged ion formed when a metal loses electrons from its valence shell.

Anion

A negatively charged ion formed when a non-metal gains electrons.

Electrostatic Attractions

Strong attractions formed between oppositely charged ions (cations and anions) to form ionic compounds.

Ionic Lattice

An evenly distributed crystalline structure formed by ions arranged in a regular repeating pattern due to electrostatic forces of attraction between cations and anions.

Properties of Ionic Compounds

Different physical properties (melting/boiling points, electrical conductivity, and solubility) due to their structure and bonding.

Covalent Bonds

Bonds formed between two non-metals through the sharing of electrons in their outer shells.

Dative Covalent Bond

A type of covalent bond where one atom donates a lone pair of electrons to an electron-deficient atom.

Multiple Bonds

Non-metals can share more than one pair of electrons to form different types of covalent bonds.

Bond Energy

The energy required to break one mole of a particular covalent bond in the gaseous state.

Bond Length

The internuclear distance between two covalently bonded atoms.

Bond Polarity

The polarity of a covalent bond determined by the difference in electronegativity between the atoms involved.

Lewis Structures

Simplified electron shell diagrams that show pairs of electrons around atoms.

Octet Rule

The tendency of atoms to gain a valence shell with a total of 8 electrons.

Incomplete Octets

Exceptions to the octet rule where elements below atomic number 20 can achieve stability with fewer than 8 electrons in their valence shells.