Bonding

all types of intra- and inter- molecular forces

Chemical Bond

the attractive force that holds atoms or ions together

Valence Electrons

Electrons in the outermost energy level of an atom that are typically involved in chemical reactions by being gained, lost, or shared in the formation of chemical bonds.

Intramolecular force

forces that hold atoms and ions together in molecules and compounds

Intermolecular force

a weak force of attraction between molecules, includes hydrogen bonds and van der Waals forces

Ionic Bond

Formed when one or more electrons are transferred from one atom to another

Cation

A positively charged ion, usually a metal atom

Anion

A negatively charged ion, usually a nonmetal

Covalent Bonds

Bonds created by sharing electrons with other atoms

Single covalent bond

a bond formed when two atoms share a pair of electrons

Double covalent bond

a bond in which two atoms share two pairs of electrons

Triple covalent bond

a bond in which two atoms share three pairs of electrons

Metallic Bond

a bond formed by the valence electrons moving freely through the metallic substance, often described as a 'sea of mobile electrons'.

Hydrogen bond

Attraction between a slightly positive hydrogen atom and a slightly negative atom, the strongest intermolecular force

Dipole

a molecule that has two poles, or regions, with opposite charges

dipole-dipole forces

attractions between oppositely charged regions of polar molecules

van der Waals forces

a slight attraction that develops between the temporary dipoles in nearby molecules, the weakest intermolecular force

Polyatomic ion

A charged group of covalently bonded atoms (see table E)

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

electronegativity difference

The difference in electronegativities between the atoms in a bond, a measure of bond polarity

Nonpolar covalent bond

a covalent bond in which the electrons are shared equally by the two atoms

Polar covalent bond

A covalent bond in which electrons are not shared equally between atoms

bond polarity

a measure of how equally or unequally the electrons in any covalent bond are shared

chemical formula

Symbols that show the elements in a compound and the ratio of atoms

empirical formula

a formula with the lowest whole-number ratio of elements in a compound

structural formula

a formula that shows the arrangement of atoms in the molecule of a compound.

symmetry

having the same shape, size, and position on both sides of a dividing line

covalent network solids

solids in which the units that make up the three-dimensional network are joined by covalent bonds, examples - diamond and graphite

boiling point

The temperature at which a liquid changes to a gas

melting point

the temperature at which a solid changes to a liquid

vapor pressure

a measure of the force exerted by a gas above a liquid

crystal

any solid material in which the component atoms or ions are arranged in a definite geometric pattern

octet rule

states that atoms tend to form compounds in ways that give them eight valence electrons and thus the electron configuration of a noble gas. 

electron dot diagram

A way of representing atoms or molecules by showing electrons as dots surrounding the element symbol

transition metals

various metallic elements in groups 3-12 (such as chromium, iron, and nickel) that have valence electrons in two shells instead of only one, often have more than one oxidation state

electrostatic force

the attraction between opposite charges

oxidation state

the hypothetical charge of an atom if all of its bonds to different atoms were fully ionic.