Nomenclature and Bonding

Chem 10 H

Octet Rule

The rule that states that atoms tend to gain, lose, or share electrons in order to achieve a full outer electron shell of eight electrons.

Ionic Bond

A type of chemical bond formed between atoms with a large electronegativity difference, resulting in the transfer of electrons from one atom to another.

Covalent Bond

A type of chemical bond formed between atoms with a small electronegativity difference, resulting in the sharing of electrons between atoms.

Diatomic Elements

Elements that naturally exist as molecules composed of two atoms bonded together.

Molecular Formula

The chemical formula that shows the type and number of atoms in a molecule of a compound.

Compound

A substance that contains two or more elements chemically combined in a fixed proportion.

Empirical Formula

The formula that shows the elements in a compound in their lowest whole-number ratio.

Binary Ionic Compounds

Compounds composed of a monatomic metal cation and a monatomic nonmetal anion.

Criss Cross Method

A method used to determine the subscripts in the formula of an ionic compound by crossing the charges of the ions.

Stock Name System

A naming system used for ionic compounds involving transition metal cations, where roman numerals indicate the charge of the cation.

Polyatomic Ions

Ions composed of more than one atom that are tightly bonded together and behave as a single unit.

Ternary Ionic Compounds

Ionic compounds composed of three or more elements, where one or both of the ions are polyatomic ions.

Binary Molecular Compounds

Molecular compounds composed of two nonmetal atoms.

Chemical Bond

The attractive force between atoms or ions that forms when they share or transfer valence electrons.

Metallic Bond

The force of attraction between a positive metal ion and the valence electrons surrounding it.

Ionic Solids

Solids composed of ions arranged in a lattice structure, with high melting points and poor conductivity.

Molecular Compounds

Compounds composed of discrete molecules joined by covalent bonds, with low boiling points and poor conductivity.

Multiple Covalent Bonds

Covalent bonds formed by atoms sharing two or three pairs of electrons.

Network Solids

Large samples of atoms covalently bonded together, resulting in very hard substances with high melting points.

Intermolecular Forces

Forces or attractions between molecules that hold a sample together.

London Dispersion Forces

The weakest type of intermolecular force, caused by the interaction of electron clouds between molecules.

Dipole-Dipole Attraction

The attraction between the oppositely charged ends (dipoles) of polar covalent molecules.

Hydrogen Bonding

A special type of dipole-dipole attraction between the hydrogen end of a polar covalent molecule and the electronegative end of a neighboring molecule.