As Chemistry Module 1 Definitions And Equations

Front 1

Isotopes

Back 1

Atoms of the same element with different neutron numbers

Hint 1

To do with neutrons

Front 2

Atomic number

Back 2

The number of protons in an atom

Front 3

Mass number

Back 3

The number of particles, protons and neutrons, in the nucleus

Front 4

Ion

Back 4

A positively or negatively charged atom or group of atoms

Front 5

Relative Isotopic Mass

Back 5

The mass of an atom of an isotope compared with 1/12 of the mass of an atom of Carbon-12

Front 6

Relative Atomic Mass

Back 6

The weighted mean mass of an atom of an element compared with 1/12 the mass of an atom of Carbon-12

Front 7

Relative Molecular Mass

Back 7

The weighted mean mass of a molecule compared with 1/12 the mass of an atom of Carbon-12

Front 8

Relative Formula Mass

Back 8

The weighted mean mass of a formula unit cleared with 1/12 the mass of an atom of Carbon-12

Front 9

Amount of Substance

Back 9

The quantity whose unit is a mole

Front 10

Avogadro Constant

Back 10

The nuber of atoms per mole of the carbon-12 isotope. (6.02 x 10^23 mol^-1)

Front 11

A mole

Back 11

The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope

Front 12

Molar Mass, M

Back 12

The mass per mole of a substance. Units: g mol^-1

Front 13

Empirical Formula

Back 13

The simplest whole number ratio of atoms of each element present in a compound

Front 14

Mole equation

Back 14

n = m ÷ M. N is Moles, m is mass, M is molar mass

Front 15

A molecule

Back 15

A small group of atoms held together by covalent bonds

Front 16

Molecular formula

Back 16

The actual number of atoms of each element in a molecule

Front 17

Molar volume

Back 17

The volume per mole of a gas. Units: dm^3 mol^-1. At RTP molar volume is 24.0 dm^3 mol^-1

Front 18

Work out moles of gas

Back 18

n = V(in dm^3) ÷ 24

Front 19

Concentration of solution

Back 19

The amount of solute, in mol, dissolved per 1 dm^3 of solution

Front 20

Concentration equation

Back 20

n = c x V (in dm^3)

Front 21

Standard Solution

Back 21

A solution of know concentration

Front 22

A Species

Back 22

Any type of particle that takes part in a chemical reaction

Front 23

Stoichiometry

Back 23

The molar relationship between the relative quantities of substances taking part in a reaction

Front 24

Acid

Back 24

A species that is a proton donor

Front 25

Base

Back 25

A species that is a proton acceptor

Front 26

An Alkali

Back 26

A base that dissolves in water forming aqueous hydroxide ions, OH-

Front 27

Common Acids

Back 27

HCL, H2SO4, HNO3

Front 28

Common Bases

Back 28

NaOH, Mg(OH)2, MgO, CuO, NH3, CH3NH2

Front 29

Common Alkalis

Back 29

NaOH, KOH, NH3

Front 30

A Salt

Back 30

Any chemical compound that is formed from an acid when a H+ ion from the acid is replaced by a metal ion or another positive ion such as NH4+

Front 31

Cation

Back 31

Positively charged ion

Front 32

Anion

Back 32

A negatively charged ion

Front 33

Hydrated

Back 33

A crystalline compound containing water molecules

Front 34

Anhydrous

Back 34

A substance that contains no water molecules

Front 35

Water of Crystallisation

Back 35

Water molecules that form an essential part of the crystalline structure of a compound

Front 36

Oxidation Number

Back 36

A measure of the number of electrons that an atom uses to bond with atoms of another element

Front 37

Oxidation

Back 37

Loss of electrons; increase in oxidation number

Front 38

Reduction

Back 38

Gain of electrons; decrease in oxidation number

Front 39

Redox Reaction

Back 39

Reaction in which both reduction and oxidation take place. OILRIG