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definitions Flashcards

1
Q

atomisation

A

1 mole of gaseous atoms formed

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2
Q

combustion

A

1 mole of substance burned with excess oxygen

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3
Q

hydration

A

1 mole of gaseous ions dissolved sufficient water to form a very dilute solution

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4
Q

neutralisation

A

1 mole of water formed from alkali and acid

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5
Q

solution

A

1 mole of ionic solid dissolved sufficient water to form a very dilute solution

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6
Q

lattice energy

A

energy change of 1 mole of an ionic compound formed from its gaseous ions

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7
Q

SEP

A

voltage produced when a standard half-cell (1.00 moldm-3 298K) is connected to standard hydrogen electrode
under sc

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8
Q

SCP

A

diff between the 2 sep between two specified half cells

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9
Q

kw

A

equ constant of ionisation of water

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10
Q

ka

A

the equilibrium constant for the dissociation of a weak acid

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11
Q

adsorption

A

1st stage in heterogenous catalysis, when reactant molecules make bonds with atoms on the catalyst surface

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12
Q

bidentate ligand

A

a ligand that forms two coordinate bonds to the central transition metal ion in a complex

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13
Q

bond energy

A

the energy required to break one mole of a particular covalent bond in the gaseous state
units : kJmol-1

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14
Q

buffer solution

A

a solution that minimises significant changes in the pH when small amounts of acids and alkalis are added

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15
Q

carbocation

A

an alkyl group with a single positive charge on one of its carbon atoms, CH3+

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16
Q

catalysis

A

the increase in rate of a chemical reaction brought about by the addition of particular substance which is not used up by the reaction

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17
Q

desorption

A

last stage in heterogeneous catalysis
bonds holding the molecular of product to the surface of the catalyst are broken, and the product molecules diffuse away from the surface of the catalyst

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18
Q

diazotisation

A

the reaction between phenylamine and nitrous acid(HNO2) to give a diazonium salt in the first step in preparing azo dye

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19
Q

electronegativity

A

the power of a particular atom that is covalently bonded to another atom to attract the bonding pair of electrons towards itself

20
Q

electrophilic sub

A

the replacement of an atom by another atom or group of atoms after initial attack by an electron-deficient species

21
Q

electrophoresis

A

the separation of ions placed in an electric field between a positive and a negative electron

22
Q

enantiomers

A

a pair of optically active molecules whose mirror images cannot be superimposed

23
Q

enthalpy change

A

the heat energy transferred during a chemical reaction

24
Q

entropy

A

the no. of possible arrangements of the particles an their energy in a given system

25
Gibbs full name
Gibbs free energy change
26
ligand
a species with one or more lone pairs of electron that form dative covalent bonds to a central transition metal atom or ion
27
mobile phase
the solvent used in chromatography, which moves along the paper, thin layer of aluminum oxide or column containing liquid supported on a solid
28
2nd EA
the enthalpy change when 1 mole of electrons is added to 1 mole gaseous 1- ions to form 1 mole of gaseous 2- ions under sc
29
ion polarisation
the distortion of the electron cloud of an anion by a neighbouring cation. distortion greates when cation is small and highly charged
30
polarising power
the ability of a cation to attract the electron cloud of an anion and distort it
31
ion-dipole bond
the bond formed between an ion and a polar compound such as water. The negative end of the dipole with positive ion positive end of dipole with negative ion
32
electrolysis
the decomposition of an ionic compound when molten or in aqueous solution by an electric current
33
nerst formula
E (under non sc) = E (under sc) + 0.059/z log[oxidised/reduced] at ROOM TEMP 25 if not, then E (under non sc) = E (under sc) + RT/zF log[oxidised/reduced] oxidised Fe3+ reduced Fe2+ oxidised is the one thats ALREADY been oxidised for metal/metal ion electrode reduced is Metal, conc of metal does not change so E (under non sc) = E (under sc) + 0.059/z log[oxidised]
34
conjugate pair
an acid-base pair on each side of an acid-base equilibrium equation that are related to each other by the difference of a hydrogen ion
35
solubility product
the product of the concs of each ion in a **saturated** solution of a **sparingly soluble** salt at 298k, raised to the power of their relative concs
36
partition coefficient
the ratio of the conc of a solute in two immiscible solvents in contact with each other when equilibrium is esstablished.
37
order of reaction
the power to which the conc of the reactant is raised in the rate equation
38
half life
the time taken for the amount/conc of the limiting reactant in a reaction to decrease to half its initial value
39
Limiting reactant
the reactant which is not in excess
40
homogenous catalysis
the type of catalysis in which the catalyst and reactants are in the same phase
41
heterogenous catalysis
the type of catalysis in which the catalyst and reactants are in the different phase
42
ggibbs free energy change
the energy change that takes into account both the entropy change of a reactionn and the enthalpy change
43
coordination no.
the nomber of cooridante bonds formed by ligands with a transition element ion in a complex
44
electrophoresis
the separation of ions place in an elcetric field between a posivit and a negative electrode
45
entropy
the number of possible arrangemtnets of the particles and their energy in a given system
46
complex
a molecule or ion formed by a metal ion surrounded by one or more ligands, dative covalently bonded
47
kstab
the equilibrium constant for the formation of the complex ion in a solvent (from its constituent ions or molecules)

Chemistry (11 decks)

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