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在A-level考试中，A-level化学是大家喜爱的一个理科课程，它的学习以理论和实操为主，主要是一些化学实验的反应原理，还有一些化学元素的记忆，小编为大家总结了ALevel化学AS最全定义，一起来学习一下吧！
1Relative atomic mass
The weighted mean/average mass of an atom relative to 1/12 the mass of an atom of C-12
2Relative isotopic mass
Mean/average mass of an atom relative to 1/12 the mass of an atom of C-12
3Relative molecular mass
Mean/average mass of an molecule relative to 1/12 the mass of an atom of C-12
4Relative formula mass
Mean/average mass of an molecule relative to 1/12 the mass of an atom of C-12
5Isotope
Atoms with the same number of protons and different number of neutrons
6Atomic number
Proton number or number of protons
7Mass number
Nucleon number; total number of protons and neutrons
8First ionisation energy
The amount of energy required to remove one electron from each atom in one mole of atoms of the element in the gaseous state (to form gaseous 1+ ions).
9Ionic bonding
Attraction/attractive force between positively and negatively charged ions in an ionic lattice.
10Covalent bonding
Attraction between nucleus and shared pair of electrons.
11Dative covalent bonding
One atom provides both electrons in the formation of the covalent bond.
12Sigma bond (σ bond）
Sigma bonds are formed by end-on overlap of atomic orbitals.
13Pi bond (Π bond）
Pi bonds are formed by sideways overlap of p-type atomic orbitals.
14Standard conditions
100kPa and 298K
15Enthalpy change of formation
The enthalpy change when one mole of a compound is formed from its elements
16The standard enthalpy change of formation
The enthalpy change when one mole of a compound is formed from its elements under standard conditions.
17The standard enthalpy change of combustion
The enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions.
18The standard enthalpy change of atomisation
The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state under standard conditions.
19The standard enthalpy change of neutralisation
The enthalpy change when one mole of water is formed by the reaction of an acid with an alkali under standard conditions.
20The standard enthalpy change of solution
The enthalpy change when one mole of solute is dissoved in a solvent to form an infinitely dilute solution under standard conditions.
21The standard enthalpy change of hydration of an anhydrous salt
The enthalpy change when one mole of anhydrous salt is formed from one mole of the anhydrous salt under standard conditions.
22Hess's law
The total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same.
23Bond enthalpy
The total amount of energy required to break 1 mole of that chemical bond.
24Reduction
Reduction is gain of electrons
Reduction is a decrease in oxidation number
25Oxidation
Oxidation is an increase of oxidation number.
Oxidation is loss of electrons.
26Equilibrium
It is dynamic.
The forward and reverse reactions occur at the same rate (of reaction).
The concentrations of reactants and products remain constant at equilibrium
It requires a closed system
27Le Chatelier's principle
If one or more factors that affect an equilibrium is changed, the position of equilibrium shifts in the direction that reduces (opposes) the change.
28Bronsted-Lowry acid
A Bronsted-Lowry acid is a proton donor
29Bronsted-Lowry base
A Bronsted-Lowry base is a proton acceptor
30Strong acids
Acids that dissociate almose completely in solution are called strong acid.
31Weak acids
Acids that are only partially dissociated in solution are called weak acid.
32Strong base
Bases that dissociate almost completely in solution
33Weak base
Weak Bases which dissociate to only a small extent in solution
34Activation energy
The minimum energy that colliding particles must possess for a successful collision to take place.
35Catalyst
A substance that increases the rate of a reaction but remains chemically unchanged itself at the end of the reaction.
36Amphoteric
Compounds that can act as both acids and bases, such as aluminium oxide.
37Group 2 metal
The group 2 metals get more reactive going down the group
38Group 17 halogens
The halogens (Cl2,Br2,I2 molecules) get less reactive going down Group 17.
More reactive halogen can displace a less reactive halogen from a halide solution of the less reactive halogen.
39The hydrogen halides
(HF, HCl, HBr, HI)
The hydrogen halides get less thermally stable going down group 17
HF least thermally stable
HI most thermally stable
It gets easier to oxidise the hydrogen halides going down group 17.
40Halogenoalkane
(R-Cl; R-Br; R-I)
Halogenoalkane becomes more reactive down the group
Fluoroalkanes least reactive
Iodoalkanes most reactive
41Disproportionation
The element chlorine (Cl2) undergoes a type of redox reaction called disproportionation when it reacts with alkali.
self reduction and oxidation
the actual reaction that takes place depends on the temperature.(in cold/hot alkali)
42Structural isomers
Structural isomers have the same molecular formula but different structural formulae.
43Stereoisomerism
Molecules have the same atoms bonded to each other but with different arrangements of the atoms in space.
44Optical isomerism
If a molecule contains a carbon atom that is bonded to four different atoms or groups of atoms, it can form two optical isomers. The two different molecules are mirror images of each other and cannot be superimposed.
45Chiral centre
The carbon atom with the four different groups attached.
46Free radicals
Free radical has an unpaired electron.
It is very reactive andproduced when a bond breaks homolytically. (homolytic fission)
47Heterolytic fission
A bond breaks unevenly to form ions.
48Carbocation
Positive alkyl ion
49Nucleophile
A donator of a pair of electrons
50Electrophile
An acceptor of a pair of electrons
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