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Chemistry > Definitions For EEE > Flashcards

Definitions For EEE Flashcards

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1
Q

Acid Base pair

A

A pair of two species that transform into each other by gain or loss of a proton

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2
Q

Activation energy

A

The minimum energy required to start a reaction by the breaking of bonds

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3
Q

Adsorption

A

The process by which a solid holds molecules of a gas or liquid or solute as a thin-film on the surface of a solid or, more rarely, a liquid

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4
Q

Alkali

A

A type of base that dissolves in water to form hydroxide ions

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5
Q

Average bond enthalpy

A

The average and enthalpy change that takes place when breaking by Homolytic fission one mole of a given type of bond in the molecules of gaseous species

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6
Q

Bond dissociation enthalpy

A

The enthalpy change that takes place when breaking by homolytic fission one mole of a given bond in the molecules of gaseous species

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7
Q

Bronsted Lowry acid

A

A species that is a proton donor

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8
Q

Bronsted Lowry base

A

A species that is a proton acceptor

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9
Q

Buffer solution

A

Assistant that minimises PH changes on addition of small amounts of an acid or a base

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10
Q

Complex ion

A

The transition metal ion bonded to one or more ligands by coordinate bonds

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11
Q

Concentration

A

The amount of solute, in mol, per 1dm^3

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12
Q

Conjugate acid

A

The species formed when a proton is added to a base

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13
Q

Conjugate base

A

The species formed when a proton is added to an acid

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14
Q

Coordinate bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only, also called a dative covalent bond

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15
Q

Coordination number

A

The total number of coordinate bonds formed between the central metal ion and any ligands

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16
Q

Dynamic equilibrium

A

The equilibrium that exists in a closed system when the rate of forward reaction is equal to the rate of the reverse reaction

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17
Q

First electron affinity

A

The enthalpy change that accompanies the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions

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18
Q

Second electron affinity

A

The enthalpy change that takes accompanies The addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions

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19
Q

Electronic structure or configuration

A

The arrangement of electrons in an atom

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20
Q

Endpoint

A

The point in a titration at which there are equal concentrations of the week acid and conjugate base forms of the indicator. The colour at the end point is midway between the colours of the acid and conjugate base forms

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21
Q

Standard enthalpy change of atomisation

A

The enthalpy change that takes place when 1 mole of gaseous atoms forms the element in its standard state

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22
Q

Standard enthalpy change of combustion

A

The enthalpy change that takes place when one mole of a substance reacts completely with oxygen understand the conditions, all reactants and products being in their standard states

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23
Q

Standard enthalpy change of formation

A

The enthalpy change takes place when one mole of a compound in its standard state is formed from its constituent elements in their Standard states under standard conditions

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24
Q

Standard enthalpy change of hydration

A

The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water, forming one mole of aqueous ions, under standard conditions

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25
Q

Standard enthalpy change of neutralisation

A

The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H20 under standard conditions

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26
Q

Standard enthalpy change of reaction

A

The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states

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27
Q

Standard enthalpy change of solution

A

The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions

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28
Q

Enthalpy cycle

A

A diagram showing alternative routes between reactants and products that allows the indirect determination of an enthalpy change from other known enthalpy changes using hess law

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29
Q

Enthalpy profile diagram

A

A diagram for a reaction to compare the enthalpy of the reactants and the enthalpy of the products

30
Q

Enthalpy

A

The heat content that is stored in a chemical system

31
Q

Entropy

A

The quantitative measure of the degree of disorder in the system

32
Q

Standard entropy change of reaction

A

The entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states

33
Q

Equivalence point

A

The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution. This matches the stoichiometry of the reaction that is taking place

34
Q

Free energy change

A

The balance between enthalpy, entropy and temperature for a process. Spontaneous when ΔG<0

35
Q

Group

A

A vertical column in the periodic table. Elements in a group have similar chemical properties and the atoms have the same number of outer shell electrons

36
Q

Half life

A

The time taken for the concentration of a reactant to reduce by half

37
Q

Hesses law

A

If a reaction can take place by more than one route and initial and final conditions are the same, the total enthalpy change is the same for each route

38
Q

Ionic product of water

A

Kw = 1x10^-14

39
Q

First ionisation energy

A

The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions

40
Q

Second ionisation energy

A

The energy required to remove one electron from each ion in one molecule of gaseous 1+ ions to form one mole of gaseous 2+ ions

41
Q

Isoelectric point

A

The pH value at which the amino acid exists as a zwitterion

42
Q

Lattice enthalpy

A

The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions

43
Q

Le Chateliers principle

A

When a system in dynamic equilibrium is subjected to a change, the system readjusts itself to minimise the effect of the change and to restore equilibrium

44
Q

Ligand

A

A molecule or ion that can donate a pair of electrons with the transition metal Ion to form a coordinate bond

45
Q

Ligand. Substitution

A

A reaction in which one Ligand in a complex ion is replaced by another Ligand

46
Q

Limiting reagent

A

The substance in a chemical reaction that runs out first

47
Q

Lone pair

A

And outer shell pair of electrons that is not involved in chemical bonding

48
Q

Neutralisation

A

A chemical reaction in which an acid and a base react together to produce a salt and water

49
Q

Nomenclature

A

A system of naming compounds

50
Q

Order

A

The power to which the concentration of the reactants is raised in the rate equation

51
Q

Overall order

A

The sum of the individual orders

52
Q

Oxidation

A

Loss of electrons or an increase in oxidation number

53
Q

Oxidation number

A

A measure of the number of electrons is that an atom uses to bonded atoms of another element.

54
Q

Oxidising agent

A

A reagent that oxidises another species (takes electrons from)

55
Q

Period

A

A horizontal row of elements in the periodic table. Elements show trends in properties across a period

56
Q

Periodicity

A

A regular periodic variation of properties of elements with atomic number and position in the periodic table

57
Q

rate constant

A

The constant that links the rate of reaction with the concentrations of the reactions raised to the powers of their orders in the rate equation

58
Q

Rate of reaction

A

The change in concentration of a reactant or product per unit time

59
Q

Rate determining step

A

The slowest step in the reaction mechanism of a multi step reaction

60
Q

Redox reaction

A

A reaction in which both reduction and oxidation take place

61
Q

Reducing agent

A

A reagent that reduces (adds electrons to) another species

62
Q

Reduction

A

Gain of electrons or a decrease in oxidation number

63
Q

Reflux

A

The continuous boiling and condensing of the reaction mixture to ensure that the reaction takes place without the contents of the flask boiling dry

64
Q

Specific heat capacity

A

The energy required to raise the temperature of 1 g of a substance by 1°

65
Q

Spectator ions

A

I am is that a present but play no part in a chemical reaction

66
Q

Stability constant

A

The equilibrium constant for equilibrium existing between a transition metal ion surrounded by water Ligand and the complex formed when the same ion has undergone a Ligand substitution reaction

67
Q

Standard electrode potential

A

The EMF of a half cell compared with a standard hydrogen half cell, measured at standard conditions

68
Q

Strong acid

A

And acid that completely dissociates in solution

69
Q

Transition element

A

A D block element which phones and I am on with an incomplete d sub shell

70
Q

Weak acid

A

And acid that partially dissociates in solutions

Chemistry (4 decks)

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