DEFINITIONS SO FAR

The number of protons in the nucleus of the atom

The number of particles (protons and neutrons) in the nucleus

Atoms of the same element with the same number of neutrons but a different number of neutrons

An electrically charged particle formed by the loss or gain of one or more electrons from an atom or group of atoms

The mass of an atom of an isotope compared to 1/12th the mass of carbon 12

The weighted mean mass of an atom of an element compared to 1/12th the mass of carbon 12

The weighted mean mass of a molecule compared with 1/12th of the mass of an atom of carbon 12 (ONLY applies to simple covalent molecules e.g. O2 or CO2)

The weighted mean mass of a formula unit compared to 1/12th of the mass of an atom of carbon 12 (Can apply to ionic substances as they occur as giant lattices)

Volume per mole of gas. Units= dm^3 mol^-1 At RTP= 24.0dm^3 mol^-1 approx.

The amount of solute, in mol, dissolved per 1dm^3 (1000cm^3) of solution

The process of decreasing the concentration of a solute in solution. Adding more solvent without adding more solute will reduce the concentration.

Atoms chemically joined

2 or more atoms bonded with covalent bonds

Average energy required to break one mole of that type of bond

A shared pair of electrons

Attraction (electrostatic) between oppositely charged ions

Substance which contains only 1 type of atom

A region that can be occupied by up to 2 electrons with opposite spins

Both of the shared electrons originate from the same species

The ability of an atom to attract the bonding electrons in a covalent bond

How close to the true value a measurement is

Minimum energy required to start a reaction by breaking bonds in the reactants

The purpose of the investigation

The quantity whose unit is mole. Amount of substance=counting atoms