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Definitions For EEE Flashcards

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
Standard enthalpy change of neutralisation
The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H20 under standard conditions
26
Standard enthalpy change of reaction
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
27
Standard enthalpy change of solution
The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
28
Enthalpy cycle
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
29
Enthalpy profile diagram
A diagram for a reaction to compare the enthalpy of the reactants and the enthalpy of the products
30
Enthalpy
The heat content that is stored in a chemical system
31
Entropy
The quantitative measure of the degree of disorder in the system
32
Standard entropy change of reaction
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
Equivalence point
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
Free energy change
The balance between enthalpy, entropy and temperature for a process. Spontaneous when ΔG<0
35
Group
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
Half life
The time taken for the concentration of a reactant to reduce by half
37
Hesses law
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
Ionic product of water
Kw = 1x10^-14
39
First ionisation energy
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
Second ionisation energy
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
Isoelectric point
The pH value at which the amino acid exists as a zwitterion
42
Lattice enthalpy
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
43
Le Chateliers principle
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
Ligand
A molecule or ion that can donate a pair of electrons with the transition metal Ion to form a coordinate bond
45
Ligand. Substitution
A reaction in which one Ligand in a complex ion is replaced by another Ligand
46
Limiting reagent
The substance in a chemical reaction that runs out first
47
Lone pair
And outer shell pair of electrons that is not involved in chemical bonding
48
Neutralisation
A chemical reaction in which an acid and a base react together to produce a salt and water
49
Nomenclature
A system of naming compounds
50
Order
The power to which the concentration of the reactants is raised in the rate equation
51
Overall order
The sum of the individual orders
52
Oxidation
Loss of electrons or an increase in oxidation number
53
Oxidation number
A measure of the number of electrons is that an atom uses to bonded atoms of another element.
54
Oxidising agent
A reagent that oxidises another species (takes electrons from)
55
Period
A horizontal row of elements in the periodic table. Elements show trends in properties across a period
56
Periodicity
A regular periodic variation of properties of elements with atomic number and position in the periodic table
57
rate constant
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
Rate of reaction
The change in concentration of a reactant or product per unit time
59
Rate determining step
The slowest step in the reaction mechanism of a multi step reaction
60
Redox reaction
A reaction in which both reduction and oxidation take place
61
Reducing agent
A reagent that reduces (adds electrons to) another species
62
Reduction
Gain of electrons or a decrease in oxidation number
63
Reflux
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
Specific heat capacity
The energy required to raise the temperature of 1 g of a substance by 1°
65
Spectator ions
I am is that a present but play no part in a chemical reaction
66
Stability constant
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
Standard electrode potential
The EMF of a half cell compared with a standard hydrogen half cell, measured at standard conditions
68
Strong acid
And acid that completely dissociates in solution
69
Transition element
A D block element which phones and I am on with an incomplete d sub shell
70
Weak acid
And acid that partially dissociates in solutions

Chemistry (4 decks)

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