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A2 Chemistry > Chemistry Definitions > Flashcards

Chemistry Definitions Flashcards

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0
Q

DEFINE: electrophile

A

Atom or group that is attracted to an electron rich centre where it accepts a pair of electrons to form a new covalent bond

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1
Q

DEFINE: delocalised electrons

A

Electrons shared between more than 2 atoms

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2
Q

DEFINE: redox

A

Reaction where oxidation and reduction takes place

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3
Q

DEFINE: reflux

A

Continual boiling and condensing of a reaction mixture to ensure a reaction takes place without the contents of flask boiling dry.

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4
Q

DEFINE: nucleophile

A

Atom or group attracted to a election deficient centre where it donates a pair of electrons to form a new covalent bond

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5
Q

DEFINE: hydrolysis

A

Reaction with water or hydroxide ions that breaks a chemical compound into two

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6
Q

DEFINE: LDL

A

Protein responsible for carrying cholesterol and triglycerides from the liver to the tissues

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7
Q

DEFINE: HDL

A

Protein that can remove cholesterol from the arteries and transport it back to the liver for excretion

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8
Q

DEFINE: primary amine

A

Amine in which the nitrogen atom is attached to one carbon

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9
Q

DEFINE: peptide

A

Compound made of amino acids linked by peptide bonds

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10
Q

DEFINE: zwitterion

A

Di polar ionic form of an amino acids that is formed by the donation of an hydrogen ion from the carboxyl group to the amino group. Because both charges are present there is no overall charge

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11
Q

DEFINE: isoelectric point

A

The pH value at which an amino acids exists as a zwitterion

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12
Q

DEFINE: condensation reaction

A

Reaction in which two smaller molecule react to form a larger molecule and eliminate a small molecule such as water.

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13
Q

DEFINE: stereoisomers

A

Species with same structural formula but different arrangement of atoms in space

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14
Q

DEFINE: chiral carbon

A

Carbon atom attached to four different groups of atoms

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15
Q

DEFINE: optical isomer

A

Stereoisomers that are non superimposable mirror images of each other

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16
Q

DEFINE: biodegradable polymer

A

A polymer that breaks down completely into carbon dioxide and water

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17
Q

DEFINE: degradable polymer

A

A polymer that breaks down into smaller fragments when exposed to light heat or moisture

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18
Q

DEFINE: pharmacological activity

A

Beneficial/ adverse effects of a drug on living matter

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19
Q

DEFINE: mobile phase

A

Phase that moves in chromatography

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20
Q

DEFINE: stationary phase

A

Phase that does move in chromatography

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21
Q

DEFINE: adsorption

A

Process by which a solid hold molecules of a gas or liquid or solute as a thin film on the surface of a solid

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22
Q

DEFINE: chromatogram

A

Visible record showing the result of a separation of the components of a mixture

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23
Q

DEFINE: Rf Value

A

Distance moved by component divided by distance moved by solvent front

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24
Q

DEFINE: retention time

A

GC - time for the component to pass from the column inlet to the detector

25
Q

DEFINE: rate of reaction

A

Change in concentration of a reactant or product per unit time

26
Q

DEFINE: initial rate of reaction

A

Change in concentration of a reactant or product per unit time at the start of the reaction when t=0

27
Q

DEFINE:order of a reactant

A

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

28
Q

DEFINE: half life

A

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

29
Q

DEFINE: reaction mechanism

A

A series of steps that together make up the overall reaction

30
Q

DEFINE: rate determining step

A

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

31
Q

DEFINE: intermediate

A

A species formed in one step of a multi step reaction that is used up in a subsequent step and is not in the overall equation as a reactant or product.

32
Q

DEFINE: dynamic equilibrium

A

Exists in a closed system when the rate of the forward reactions is equal to the rate of the reverse reaction

33
Q

DEFINE: homogeneous equilibrium

A

An equilibrium in which all the species making up the reactants and products are in the same physical state

34
Q

DEFINE: heterogeneous equilibrium

A

Equilibrium in which the species making up the reactants and products are in different physical States

35
Q

DEFINE: Bronsted-Lowry acid

A

Proton donor

36
Q

DEFINE: Brønsted-Lowry base

A

Proton acceptor

37
Q

DEFINE: alkali

A

Base that dissolves in water forming OH- ions

38
Q

DEFINE: neutralisation

A

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

39
Q

DEFINE: acid base pair

A

Pair of species that transform into each other by gain or loss of a proton.

40
Q

DEFINE: strong acid

A

Acid that completely dissociates in solution

41
Q

DEFINE: weak acid

A

Acid that partially dissociates in solution.

42
Q

DEFINE: Kw

A

Ionic product of water

43
Q

DEFINE: buffer solution

A

Mixture that minimises small changes in pH on addition of small amounts of acid/base

44
Q

DEFINE: equivalence point

A

Point of a titration at which the volume of one solution has reacted exactly with the volume of the second solution

45
Q

DEFINE: end point

A

Point in a titration at which there are equal concentrations of weak acid and conjugate base forms of the INDICATOR

46
Q

DEFINE: standard enthalpy change of neutralisation

A

Energy change accompanying the neutralisation of an acid by a base to form one mol of h2o under standard conditions

47
Q

DEFINE: standard enthalpy change of formation

A

Energy change that takes place when one mol of a compound is formed from its constituent elements in their standard states under standard conditions

48
Q

DEFINE: standard enthalpy change of atomisation

A

Enthalpy change that takes place when one mol of gaseous atoms forms from the element in its standard state

49
Q

DEFINE: 1st ionisation energy

A

Enthalpy change that accompanies the removal of one electron from each atom in one mol of gaseous atoms to form one mol of gaseous 1+ ions

50
Q

DEFINE: 1st electron affinity

A

Enthalpy change accompanying the addition of one electron to each atom in one mol of gaseous atoms to form one mol of gaseous 1- ions

51
Q

DEFINE: standard enthalpy change of Solution

A

Enthalpy change that takes place when one mol of a compound is completely dissolved in water under standard conditions

52
Q

DEFINE: standard enthalpy change of hydration

A

Enthalpy change that takes place when one mol of isolated gaseous ions is dissolved in water forming one mol of aqueous ions under standard conditions

53
Q

DEFINE: entropy

A

The measure of disorder in a system

54
Q

DEFINE: oxidation

A

Loss of electrons and increase in oxidation number

55
Q

DEFINE: reduction

A

Gain of electrons and decrease in oxidation number

56
Q

DEFINE: standard electrode potential of a half cell

A

The emf of a half cell compared with a standard hydrogen half cell measured at 298K 100KPa and solution concentrations of 1moldm-3

57
Q

DEFINE: translation element

A

D block element that forms an ion with a incomplete d sub shell

58
Q

DEFINE: complex ion

A

Transition metal ion bonded to one or more Ligands by dative covalent bonds

59
Q

DEFINE: ligand

A

Molecule or ion that can donate a pair of electrons with the transition metal ion to form a co ordinate bond

60
Q

DEFINE: co ordination number

A

Total number of co ordinate bonds formed between a central metal ion and its Ligands

61
Q

DEFINE: ligand substitution

A

Reaction in which one ligand in a complex ion is replaced by another ligand

A2 Chemistry (2 decks)

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