Unit 2: Molecular and Ionic Compound Structure and Properties

Bonding

Atoms engage in bonding to share electrons and achieve a stable, lower-energy state.

Ionic Bonds

Bonds between a nonmetal and metal held together in a lattice structure by electrostatic attraction.

Cation

A positively charged ion that gives up electron(s) to bond with an anion.

Anion

A negatively charged ion that accepts electron(s) from a cation.

Electrostatic Attraction

The force that holds ionic bonds together due to opposite charges.

Coulomb's Law

Describes how the strength of ionic bonds increases with greater charge and decreases with larger ion size.

Metallic Bonds

Bonds characterized by a 'sea of electrons' allowing for electrical conductivity, malleability, and ductility.

Interstitial Alloys

Alloys formed when two metals with vastly different atomic radii combine.

Substitutional Alloys

Alloys formed when metals of similar atomic radii combine.

Covalent Bonds

Bonds formed when two nonmetals share electrons in their valence shell.

Sigma Bond

The first covalent bond formed between two atoms, involving direct overlap of orbitals.

Pi Bond

A bond formed from the side-to-side overlap of p-orbitals, existing in double and triple bonds.

Internuclear Distance

The distance between two nuclei in a covalent bond determining bond stability.

Network Covalent Bonds

Strong bonds in a lattice structure, resulting in very hard materials with high melting and boiling points.

Conductivity

The ability of a substance to conduct electricity, influenced by the type of bonds it has.

Formal Charge

A calculation to determine the most likely structure of a molecule using assigned and valence electrons.

Lewis Dot Structures

Diagrams that represent the valence electrons of atoms within a molecule.

VSEPR Model

A model used to predict the geometric arrangement of electron pairs around a central atom.

Expanded Octets

The ability of certain elements to have more than eight valence electrons due to d-orbitals.

Incomplete Octets

Atoms, like Boron, that are stable with fewer than eight valence electrons.