DEFINITIONS Flashcards
(92 cards)
1
Q
Atom
A
The smallest particle of matter and is made up of protons, neutrons and electrons
2
Q
Element
A
Only made up of one sort of atom
3
Q
Molecule
A
Two or more atoms covalently bonded together. Atoms can be the same or different elements
4
Q
Compound
A
Two or more different types of atom bonded together. Boning can be ionic or covalent
5
Q
Mixture
A
Has two or more different elements and/or compounds in the same space.
They can be separated into individual components
6
Q
Sulfuric acid
A
H2SO4
7
Q
Nitric acid
A
HNO3
8
Q
Phosphoric acid
A
H3PO4
9
Q
Ammonium
A
NH4 +
10
Q
Nitrate
A
NO3 -
11
Q
Hydrogencarbonate
A
HCO3 -
12
Q
Carbonate ion
A
CO3 2-
13
Q
Sulfate ion
A
SO4 2-
14
Q
Phosphate ion
A
PO4 3-
15
Q
An acid
A
a substance that donates H+ Ions
16
Q
A base
A
Substace that accepts H+ ions
17
Q
An alkali
A
A base that releases hydroxide ions in aqueous solution
18
Q
A salt
A
Formed when hydrogen ions from an acid are replaced by a metal or ammonium ion
19
Q
Acid + Alkali
A
Salt + water
20
Q
Acid + Base
A
Salt + Water
21
Q
Acid + Metal
A
Salt + Hydrogen
22
Q
Acid + metal carbonate
A
Salt + water + CO2
23
Q
Acid + metal hydrocarbonate
A
Salt + water + CO2
24
Q
What to split for an ionic equation
A
Must be:
-Ionic
-(Acids)
-aqueous
25
Atomic number
Number of protons in the nucleus
26
Mass number
Number of protons and neutrons in the nucleus
27
Isotope
Atoms of the same element with a different number of neutrons
28
Why do isotopes have the same chemical properties
They have the same electron configuration
29
Isotopic mass
The mass of an isotope relative to 1/12th the mass of a C-12 atom
30
Relative atomic mass(Ar)
the weighted average mass of all the isotopes relative to 1/12th the mass of an atom of c-12
31
Relative molwecular mass
The mass of a molecule of the compound relative to 1/12th the mass of an atom of C-12.
32
Relative formular mass
Is the mass of one formula unit of an ionic compound relative to 1/12th of the mass of an atom of c-12
33
The mole
The amount of substance that contains as many particles as there are in exactly 12g of C-12
34
Empirical formula
The simplest whole number ratio of atoms of each element present in a molecule
35
Molecular formula
The actual number of atoms of each element present in a molecule
36
Metallic bond
The attratction between delocalised outer shell electrons and positive metal ions in a lattice
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Ionic bond
The electrostatic attraction between oppositley charged ions in a lattice
38
Covalent bond
A shared pair of e-
39
A lone pair
A pair of e- which is not bonded
40
Co-ordinate bond
A covalent bond in which both e- of the shared pair come from the same atom
41
Electronegativety
The power of an atom to attract the pair of e- in a covalent bond
42
Enthalpy change
The heat energy change at constant pressure
43
Activation energy
The minimum energy required to start a reaction by the breaking of bonds
44
Bond enthalpy
The energy required to break one mole of a given covalent bond in he molecules in the gaseous state
45
Mean bond enthalpy
The energy required to break a covalent bond, avergaed for the type of bond in a range of different compounds
46
Standard enthalpy of formation
The enthalpy change that occurs when one mole of a compound is formed from its constituent elements with all reactants and products in their standard states
47
Standard enthalpy of combustion
The enthalpy change tat occurs when one mole of a compound reacts completley in oxygen with all reactants and produucts
48
Hess's law
The enthalpy change for a chemicals reaction is independent of the route taken
49
Rate of reaction
The change in concentration of a substance in a given time
50
Le chataliiers principle
If a system in euqilibrium is subjected to a change, the postiotn of equilibrium will move in the direction which opposes that change
51
Oxidation
Loss of electrons
51
Reduction
Gain of electrons
51
Oxidation (OS)
Increase in oxidation state
51
Reduction (OS)
Decrease in oxidation state
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Oxidising agent
A species that accepts e-
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Reducing agent
Species that donates e-
54
Enthalpy of lattice dissociation
The enthalpy change to seperate one mole of solid ionic compound into its gaseous ions.
55
Enthalpy of lattice formation
The enthalpy change when one mole of solid ionic compound is formed from its gaseous ions
56
Standard enthalpy of formation
The enthalpy change that occurs when one mole of a compound is formed from its constituent elements with all reactants and products in their standard states
57
Standard enthalpy of of atomisation
The enthalpy change when one mole of gaseous atoms is formed from the elements in its standard states.
58
Bond ethalpy
The energy required to brea one mole of a given covalent bond in the molecules in the gaseous state.
59
First ionisation energy
The energy needed to remove one mole of elecrons from one mole of atoms in the gaseous state
60
Second ionisation nergy
The enthalpy hcnage when one mole of gaseous 2+ ions are formed from one mole of gaseous +1 ions.
61
First electron affinity
The enthalpy change when one mole of gaseous 1- ions are formed from one mole of gaseous atoms.
62
Second electron affinity
The enthalpy change when one mole of gaseous 2- ions are formed from one mole of gaseous 1- ions.
63
Perfect ionic model
Ions are perfect spheres with only electrostatic forces of atraction.
63
Enthalpy change of solution
The enthalpy change when one mole of an ionic substance dissolves in enough solvent to form an infinitely dilute solution
64
Rate determining step
The slowest step in a reaction mechansim
65
Standard electrode potentiel
The emf of a halfcell compared with the standard hydrogen half-cell. Measured at 298k, all solution have conc of 1moldm-3 and gases at 100kpa.
66
Bronsted-Lowry acid-base reaction
Proton transfer
67
Acid
Donates H+
68
Strong acid
Completley dissociates in siolution
69
Weak acid
Partially dissociates in solution
70
Base
Accpets H+
71
Alkali
A base that releases hydroxide ions in aqueous solutions
72
Buffer
A solution that maintains an approximatley constant pH on addition of small amounts of acid or base
73
Molecular formula
The actual number of atoms of each element present in a molecule
74
Emperical formula
Simplest whole number ratio of atoms of each element present in a molcule
74
Structural formula
Shows how the atoms in a molecule are arranged
75
Displayed formula
Shows all the atoms and bonds in a molecule
76
Skeletal formula
Shows the shape of the carbon skelenton
77
Homologous series
A famoly of compounds conatining the same functional group and having the same general formula but having a different carbon chain lenght
78
Functional group
An atom or group os atoms which gives an organic compound particular chemical properties
79
Structual isomers
Compounds with the same molecular formula but a different structural formula
80
Chain isomers
Same molecula formula but their structures have the hydrocarbon chain arranged differently
81
Position isomers
Have the functional group in a differetn position
82
Functional group isomers
Same molecular formular but different functional group
83
Free-radical
A species with an unpaired e-
84
An electrophile
An e- pair acceptor
85
Biofuel
A fuel derived or produced from renewable biological resources
86
Optical isomers
Non-superimposable mirror images
87
Racemic mixture
A mixture of equal amounts of the two enantiomers
