Chemistry Terms 🔬

Electron dot structures

Diagrams that show valence electrons as dots

Lone pairs

Electrons unused in bonding bonding

Alloy

Mixtures composed of two or more elements, at least one of which is a metal.

Dipole interactions

Occur when polar molecules are attracted to one another

Polar molecule

One end of the molecule is slightly negative and the other end is slightly positive

Chemical formula

Shows the kinds and numbers of atoms in the smallest representative unit of a substance

Resonance structure

A structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion

Polyatomic ion

A tightly bound group of atoms that has a positive or negative charge and behaves as a unit

Octet rule

An octet is a group of eight electrons; in forming compounds atoms want to achieve the electron configuration of a noble gas.

Hydrogen bonds

Attractive forces in which hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.

Single bond

Two atoms held together by sharing a pair of electrons

No polar covalent bonds

When the atoms in the bond pull equally, the bonding electrons are shared unequally.

Molecule

A neutral group of atoms joined together by covalent bonds

Coordinate covalent bond

A covalent bond in which one atom contributes both bonding electrons

Duet rule

A duet is a pair of electrons; this rule is followed by hydrogen, which only needs on more electron to be content.

Diatomic molecule

A molecule consisting of two atoms

Dipole

A molecule that has two poles

Ionic compounds

Compounds composed cations and anions

Metallic bonds

Consists of attraction of the free floating valence electrons for the positively charged metal ions.

Triple bond

Formed by the sharing of three pairs of electrons

Double bond

Involves two shared pairs of electrons

Covalent bond

The atoms held together by sharing electrons

Valence electrons

The electrons in the highest occupied energy level of an element's atoms

Ionic bond

The electrostatic forces that hold ions together in ionic compounds

VSPER theory

The idea that the repulsion between electron pairs causes molecular shapes to adjust so that the valence electron pairs stay far apart

Formula unit

The lowest whole number ratio of ions in an ionic compound

Coordination number

The number of ions of opposing charge that surround the ion in a crystal.

Dispersion forces

The weakest of all molecular interactions, are caused by the motion of electrons