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Chemistry > Definitions > Flashcards

Definitions Flashcards

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0
Q

Lewis acid

A

Electron pair acceptor

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1
Q

Amphoteric

A

An amphoteric oxide is one which is capable of reacting with both acids and bases- eg aluminium oxide

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2
Q

Lewis base

A

Electron pair donor

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3
Q

Standard electromotive force

A

The potential difference between the electrodes of a standard electrochemical cell measured under zero conditions

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4
Q

Primary cell

A

Irreversible cell and is not intended to be recharged by electric current

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5
Q

Secondary cell

A

Reversible and rechargeable

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6
Q

Fuel cell

A

Generates electricity from continuous oxidation or an external source of fuel

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7
Q

Delta H

A

The standard enthalpy change at 298k

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9
Q

Electron affinity

A

Standard molar enthalpy change for the addition of an electron to an isolated atom in the gas phase

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9
Q

Enthalpy change

A

Amount if heat energy released or absorbed when a chemical/ physical change occurs at constant pressure

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10
Q

Enthalpy of atomisation

A

Standard enthalpy change for the formation of one mole of gaseous atoms from the element in its standard state

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11
Q

Enthalpy of fusion

A

Enthalpy change then a solid forms a liquid at its melting point

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12
Q

Enthalpy of hydration

A

Enthalpy change for the formation. Of aqueous ions from gaseous ions

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13
Q

Lattice enthalpy of formation

A

Enthalpy change for the formation of a solid ionic lattice from its gaseous atoms

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14
Q

Lattice enthalpy of dissociation

A

Enthalpy change for the separation of a solid ionic lattice into its gaseous ions

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15
Q

Enthalpy of solution

A

Enthalpy change that occurs when an ionic solid dissolves in enough water that the ions are well separated and do not interact with one another

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16
Q

Enthalpy of sublimation

A

Enthalpy change that occurs on sublimation, when a solid changes directly to a gas without forming liquid phase

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17
Q

Enthalpy of vaporisation

A

The standard molar enthalpy change when a liquid forms a gas at its boiling point

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18
Q

Entropy

A

A measure of disorder of a system

19
Q

First ionisation enthalpy

A

Enthalpy change for the removal of an electron from an atom in the gas phase to form a positive ion and an election in the gaseous phase.

20
Q

Electrochemical series

A

A list of standard electrode potentials arranged in order of their numerical values

21
Q

Adsorption

A

The process by which a substance is weakly bonded to and held in place on a solid surface.

22
Q

Acidity reaction

A

A reaction of a metal aqua ion in which an 0-H bond in a co-ordinated water molecule is broken, releasing H+ ions.

23
Q

Aqua ion

A

A metal surrounded by water Ligands

24
Q

Beer-Lambert law

A

A=ecl where absorbance A, concentration C, cell-path-length L, and molar absorbance coefficient e, are linked

25
Q

A change in colour in a complex can arise from….

A

Change in co-ordination number, ligand or oxidation state.

26
Q

Chelate effect

A

The effect of driving a reaction in the forward direction when a bidentate or multidentate reacts with a compound surrounded by unidentate Ligands.

27
Q

Combined heat and power systems

A

Domestic electricity generation systems which use up waste heat to provide local heating- these systems are more cost efficient by feeding excess electrical power backwards- into the grid

28
Q

Feasible change

A

One which has a natural tendency to occur without being driven my external influences

29
Q

Free radical

A

A species which results from homolytic fission, containing an unpaired electron

30
Q

Fuel cell

A

One in which produces electrical power from an external supply of a fuel and an oxidant

31
Q

Gas electrode

A

An inert metal surrounded by gas in equilibrium with a solution of its ions

32
Q

Ground state

A

The lowest energy state of electrons in a species

33
Q

Haemoglobin

A

A octahedrally co-ordinated iron2 complex, responsible for the red pigment in red blood cells and transporting oxygen in the blood

34
Q

Heterolytic fission

A

Formation of ions when a covalent bond breaks with an unequal splitting of the bonding pair of electrons

35
Q

Homolytic fission

A

Formation of radicals when a covalent bond breaks with an equal splitting of the bonding pair of electrons

36
Q

Inert support medium

A

An I reactive solid used to dilute a reagent or a catalyst

37
Q

Mixed catalyst

A

Those prepared by mixing two or more catalytic substances

38
Q

Non rechargeable cell

A

One not intended to be recharged by an electric current- also known as a primary cell

39
Q

Nucleophile

A

Electron pair donor

40
Q

Oxidation state

A

The charge a central metal atom in a complex would have if it existed as a solitary simple ion without bonds to other species

41
Q

Planck’s constant

A

The constant of proportionality between energy (delta E) of absorbed light and it’s frequency. Delta E=hv

42
Q

Salt bridge

A

An electrolyte solution used to complete electrical contact between two electrode compartments- allows the transfer of ions between compartments

43
Q

Sequestering ability

A

The peppery of a substance to keep metal ions in solution even when anions which normally cause precipitation are added

44
Q

Titrations using potassium dichromate

A

When using an oxidising agent in acidic solution there is no distinctive colour change at the end-point, and indicator is needed- sodium diphenlyaminesulfonate- colourless to pink

45
Q

Visible spectrophotometer

A

A device that uses visible light of varying frequencies to measure the amount of light absorbed by a coloured solution. Absorption is proportional to the concentration of absorbing species under test

Chemistry (2 decks)

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