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Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

First Ionisation Energy

A

Energy required to remove one electron from each atom in a mole of gaseous atoms to form one mole of gaseous ions

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2
Q

Relative atomic mass

A

The weighted mean mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12

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3
Q

Relative molecular mass

A

Relative molecular mass
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12

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4
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element present in a compound

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5
Q

Dative covalent bond

A

A covalent bond where both electrons in the shared pair come from the same atom

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6
Q

Eletcronegativity

A

The power of an atom to attract negative charge towards itself in a covalent bond

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7
Q

Enthalpy change

A

Heat energy change measured at constant pressure (ΔH)

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8
Q

Standard Enthalpy of Formation

A

The change in Enthalpy that accompanies the formation of 1 mole of a compound from its elements with all substances in their standard states

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9
Q

Standard Enthalpy of Combustion

A

The enthalpy change when one mole of a substance is completely burnt in oxygen under standard conditions

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10
Q

Mean Bond Enthalpy

A

The average enthalpy change when breaking a certain type of bond, averaged over a range of compounds

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11
Q

Specific Heat Capacity

A

The energy required to raise the temperature of one gram of a substance by one degree Celsius

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12
Q

Hess’s Law

A

The enthalpy change of a reaction is independent of the route taken

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13
Q

Activation Energy

A

The minimum amount of kinetic energy that particles need in order to react

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14
Q

Reaction Rate

A

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

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15
Q

Catalyst

A

A substance that increases the rate of reaction without being used up in the reaction. It does this by offering an alternative path with a lower activation energy

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16
Q

Dynamic Equilibrium

A

Equlibrium where the froward and backwards reactions occur at the same rate. In a closed system

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17
Q

Le Chatelier’s Principle

A

If a reaction at equilibrium is subjected to a change in concentration, pressure or temperature, the position of equilibrium will move to counteract the change

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18
Q

Compromised Conditions

A

Conditions that take into consideration max. yield and rate of reaction

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19
Q

Oxidation

A

Loss of electrons

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20
Q

Reduction

A

Gain of electrons

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21
Q

Oxidation State

A

No. of electrons accepted or donated

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22
Q

Oxidising Agent

A

Electron acceptor and gets reduced

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23
Q

Reducing Agent

A

Electron donor and gets oxidised

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24
Q

Lattice energy of dissociation

A

The enthalpy change when 1 mole of a solid ionic compound is completely dissociated into its gaseous ions under standard conditions

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25
Q

Lattice formation of enthalpy

A

The enthalpy change when 1 mole of a solid ionic
compound is formed from its constituent gaseous ions under standard conditions

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26
Q

Atomisation enthalpy

A

The enthalpy change when one mole of gaseous atoms is formed from its constituent element under standard conditions

27
Q

Enthalpy of electron affinity

A

The enthalpy change when one mole of electrons is added to a mole of gaseous atoms under standard conditions

28
Q

Enthalpy of solution

A

The enthalpy change when one mole of an ionic solid dissolves in an infinite amount of water so that the dissolved ions are separated and do not interact with each other, under standard conditions

29
Q

Enthalpy of hydration

A

The enthalpy change when one mole of gaseous ions is dissolved in an infinite amount of water to form to one mole of aqueous ions under standard conditions

30
Q

Entropy

A

Measure of disorder

31
Q

Free Energy Change ΔG?

A

A measure used to predict wether a reaction is feasible

32
Q

Overall Order of Reaction

A

The sum of the powers to which the concentration terms are raised in the rate equation

33
Q

Standard Electrode Potential

A

The voltage measured under standard conditions when a half cell is connected to a standard hydrogen electrode

34
Q

Electrochemical Series

A

A list of electrode potentials in numerical order

35
Q

Bronsted Lowry acid

A

proton donor

36
Q

Bronsted Lowry base?

A

proton acceptor

37
Q

pH

A

measure of hydrogen ion concentration

38
Q

Buffer

A

A solution that resists change in pH when small volumes of acid or base are added

39
Q

Disproportionation reaction

A

When something is both reduced and oxidised

40
Q

Amphoteric

A

Can act as an acid or a base

41
Q

Transition metal

A

Elements in the d block of the periodic table with a partially filled d orbital

42
Q

Complex

A

Central metal atom or ion surrounded by co-ordinately bonded ligands

43
Q

Ligand

A

atom/ion/molecule that donates a pair of electrons to a central transition metal ion to form a co ordinate bond

44
Q

Chelate Effect

A

Positive entropy change is favourable so monodenatate lingands are substituted with bidentate and multidentate ligands (more moles on RHS)

eg [Fe (H2O)6]3+ + EDTA 4- –> [Fe (EDTA)]- +6H2O) more moles formed so favourable

45
Q

Heterogeneous catalyst

A

A catalyst that is in a different phase or state to the species in the reaction

46
Q

Homogenous catalyst

A

A catalyst that is in the same phase/state as the species in the reaction

47
Q

Homologou series

A

Series of organic compounds which contain the same functional group

48
Q

Stereoisomerism

A

Same molecular formula but different spatial arrangement

49
Q

Biofuel

A

Fuel that’s made from biological material that’s recently died

50
Q

Esterification

A

Making esters by reacting carboxylic acids and alcohols

51
Q

Saponification

A

Alkaline hydrolisis of fats into glycerol and the salts of the fatty acids present in the fat

52
Q

Trans-esterification

A

Reacting an ester with an alcohol to produce a different ester and a different alcohol (eg production of biodiesel)

53
Q

Acid derivatives

A

Compounds that are related to carboxylic acids, the OH group has been replaced by something else

54
Q

Acylation

A

The process in which an acyl group is added to a molecule

55
Q

Arene

A

An aromatic compound - contains a benzene ring as part of its structure

56
Q

Nitration

A

When you warm benzene with conc. nitric and sulfuric acid and get nitrobenzene

57
Q

Inductive effect

A

An electron pushing effect - alters the electron density distribution in a molecule

58
Q

Amphoteric

A

Has both acidic and basic properties

59
Q

Zwitterion

A

Dipolar ion that has both positive and negative charge in different parts of the molecule

60
Q

Isoelectric point

A

pH where average overall charge is zero

61
Q

Proteins

A

Sequences of amino acids joined by peptide bonds

62
Q

Enzymes

A

Proteins that act as biological catalysts

63
Q

Inhibitor

A

Slows down rate of reaction (bonds to active site ∴ blocking it)

64
Q

DNA

A

Polymer of nucleotides

Chemistry (10 decks)

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