Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
39 Cards in this Set
- Front
- Back
|
Acid |
A species that is a proton donor |
|
|
Alkali |
A type of base that dissolves in water forming hydroxide ions, OH-(aq) ions |
|
|
Amount of substance |
The quantity whose unit of the mole. Chemists use 'amount of substance' as a means of counting atoms |
|
|
Anion |
A negatively charged ion |
|
|
Atomic orbital |
A region within an atom that can hold up to two electrons, with opposite spins |
|
|
Avogadro constant, NA |
The number of atoms per mole of the carbon-12 isotopes (6.02 x 10^23 mole^-1) |
|
|
Base |
A species that is a proton acceptor |
|
|
Catalyst |
A substance that increases the rate of a chemical reaction without being used up in the process |
|
|
Cation |
A positively charged ion |
|
|
Dative covalent |
A shared pair of electrons which has been provided by one of the bonding atoms only; also called a coordinate bond |
|
|
Delocalised electrons |
Electrons that are shared between more than two atoms |
|
|
Disproportionation |
The oxidation and reduction of the same element in a redox reaction |
|
|
Electronegativity |
A measure of the attraction f a bonded atom for the pair of electrons in a covalent bond |
|
|
Electron shielding |
The repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer-shell electrons |
|
|
Empirical formula |
The simplest whole-number ratio of atoms of each element present in a compound |
|
|
Hydrolysis |
A reaction with water or aqueous hydroxide ions that breaks a chemical compound into two compounds |
|
|
First ionisation energy |
The energy requires to remove one electron from each atom in one mole of atoms in the gaseous sate |
|
|
Isotopes |
Atoms of the same element with different numbers of neutrons and different masses |
|
|
Lone pair |
An outer-shell pair of electrons that is not involved in chemical bonding |
|
|
Molar mass, M |
The mass mole of a substance. The units of molar mass are g mol^-1 |
|
|
Mole |
The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotopes |
|
|
Molecular formula |
The number of atoms of each element in a molecule |
|
|
Monomer |
A small molecule that combines with many other monomers to form a polymer |
|
|
Oxidation |
Loss of electrons or an increase in oxidation number |
|
|
Oxidation number |
A measure of the number of electrons that an atom uses to bond with atoms of another element. Oxidation numbers are derived from a set of rules |
|
|
Polymer |
A long molecular chain built up from monomer units |
|
|
Principal quantum number, n |
A number representing the relative overall energy of each orbital, which increases with distance from the nucleus. The sets of orbitals with the same n value are referred to as electron shells or energy levels |
|
|
Redox reaction |
A reaction in which both reduction and oxidation take place |
|
|
Reduction |
Gain of electrons or a decrease in oxidation number |
|
|
Relative atom imass, Ar |
The weighted mean mass of an atom of an element compared with one-twelfth of the mass ofa n atom of carbon-12 |
|
|
relative formula mass |
The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-2 |
|
|
Relative isotopic mass |
The mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12 |
|
|
Relative molecular Mass, Mr |
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12 |
|
|
Saturated hydrocarbon |
A hydrocarbon with single bonds only |
|
|
Stoichiometry |
The molar relationship between the relative quantaties of substances taking part in a reaction |
|
|
Structural formula |
A formula showing the minimal detail for the arrangement of atoms in a molecule |
|
|
Sub-shell |
A group of the same type of atomic orbitals (s, p, d or f) within a shell |
|
|
van der Walls' forces |
Very weak attractive forces between induced dipoles in neighbouring molecules |
|
|
Water of crystallisation |
Water molecules that form an essential part of the crystalline structure of a compound |
