Unit 1 - Chemistry

Front 1

Orbitals

Back 1

Region where there is a 95% probability of locating an electron.An orbital can hold a maximum of two electrons.

Front 2

Electron configuration

Back 2

The distribution of electrons in an atom or molecule

Front 3

Spin

Back 3

Electrons have two possible states,'spin up' and 'spin down'. In an orbital , each electron will be in a different 'spin state'

Front 4

Ionic bonding

Back 4

Electrostatic attraction between two oppositely charged ions.

Front 5

Electrostatic attraction

Back 5

The force experienced by oppositely charged particles.It holds the particles strongly together.

Front 6

Giant ionic lattice

Back 6

A regular arrangement of positive ions and negative ions,for example in NaCl.

Front 7

Lone pair

Back 7

A non-binding pair of electrons.

Front 8

Organic compound

Back 8

A compound that contains one or more carbon in a carbon chain.

Front 9

Delocalised electrons

Back 9

Electrons that are free to move.They are present in metals and are not associated with a single atom or covalent bond.

Front 10

Non-polar molecule

Back 10

A molecule where the electrons are distributed evenly through out the molecule.

Front 11

Polar molecule

Back 11

A molecule with partial positive charge in one part of the molecule and similar negative charge in another part due to an uneven electron distribution.

Front 12

Intermolecular forces

Back 12

The attraction or repulsion between neighboring molecules

Front 13

Dipoles

Back 13

Separation of charges within a covalent molecule.

Front 14

Van der Waals forces

Back 14

All intermolecular attractions are van der Waals forces.

Front 15

Mole

Back 15

A unit of substance equivalent to the number of atoms in 12g of carbon-12.One mole of a compound has a mass equal to its relative atomic mass expressed in grams.

Front 16

Molar mass

Back 16

The mass of one mole of a substance.

Front 17

Titration

Back 17

A method of volumetric analysis used to calculate the concentration of a solution.

Front 18

Solution

Back 18

A liquid mixture where a solute is dissolved in a solvent.

Front 19

Standard solution

Back 19

A solution of known concentration used in volumetric analysis.

Front 20

Solute

Back 20

The substance dissolved in a solvent to form a solution.

Front 21

Solvent

Back 21

A liquid that dissolves another substance.

Front 22

Stoichiometry

Back 22

Involves using the relationship between the reactants and the products in a chemical reaction to work out how much product will be produced from give amounts of reactants.

Front 23

Theoretical mass

Back 23

The expected amount of product form a reaction calculated from the balanced equation.

Front 24

Reversible reaction

Back 24

A reaction where the reactants react to form products and the products simultaneously react to re form the reactant for example, in NaCl.

Front 25

Percentage yield

Back 25

The actual amount of mass worked out as a percentage of the theoretical mass.

Front 26

Atomic number

Back 26

The number of protons in a n atom.

Front 27

Cations

Back 27

Ions with a positive charge.

Front 28

Isoelectronic

Back 28

Having the same number of electrons.

Front 29

Anions

Back 29

Ions with a negative charge.

Front 30

First ionisation energy

Back 30

The energy needed for one mole of electrons to be removed from one mole of gaseous atom.

Front 31

Periodicity

Back 31

The repeating pattern seen by the elements in the period table.

Front 32

Electron affinity

Back 32

The change in energy when one mole of a gaseous atom gains one mole of electrons to form a mole of gaseous atom gains one mole of electrons to form a mole of negative ion.

Front 33

Malleble

Back 33

Can be hammered into shape without breaking.

Front 34

Ductile

Back 34

Can be hammered thin or stretched into wires without breaking.

Front 35

Alkaline solution

Back 35

A solution with a pH above 7.

Front 36

Oxidation

Back 36

Loss of electrons form an atom/ion.

Front 37

Allotropes

Back 37

Two or more different physical form that an element can exist in.

Front 38

Amphoteric

Back 38

Substance that can act as both an acid and base.

Front 39

Redox

Back 39

The transfer of electrons during chemical reactions.

Front 40

Reduction

Back 40

When an atom ion gains electrons.

Front 41

Half equation

Back 41

An equation that shows the loss or gain of electrons during a reaction.

Front 42

Oxidation state

Back 42

The number assigned to an element in a chemical compound.It is a positive or negative number depending on how many electrons the element has lost or gained.

Front 43

Redox reaction

Back 43

Reactions in which atoms have their oxidation state changed.

Front 44

Catalysts

Back 44

Substances that increase the rate of a chemical reaction but are unchanged at the end of the reaction.

Front 45

Oxidising agents

Back 45

Substances that withdraw electrons from other atoms or ions.