Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chem A2 > A2 chem definitions > Flashcards

A2 chem definitions Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Co-ordination number of six

A

6 dative covalent bonds bonded to central metal atom/ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Electron affinity

A

E change when 1 e- is added to each atom in 1 mole of gaseous atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Lattice Energy

A

Enthalpy change when 1 mole of solid ionic compound is formed from its gaseous ions under standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Enthalpy change of solution

A

Energy change when 1 mole of solute is dissolved in an infinite amount of water to form a dilute solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Enthalpy change of atomisation

A

Energy change when 1 mole of gaseous atoms are formed from its element in standard state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Enthalpy change of hydration

A

Energy change when 1 mole of gaseous ions is dissolved in an excess of water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Bond Energy

A

The energy change when 1 mole of covalent bonds is broken in gaseous state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Weak acid

A

An acid that is partially ionised

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Amphoteric

A

Can react with an acid or base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Standard cell potential

A

Potential difference between 2 half cells under standard conditions of 1 atm, 298K, solutions being 1moldm^-3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Standard electrode potential

A

Potential difference when a half cell is connected to standard hydrogen electrode under standard conditions of 1 atm, 298K, solutions being 1moldm^-3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Rate of reaction

A

Change in amount of reactants per unit time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Half-life of a reaction

A

The time is taken for the amount of reactant to halve

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Rate-determining step

A

Slowest step in the overall reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Heterogenous

A

Different states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Homogenous

A

Same States

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Heterogenous catalyst

A

Catalyst and the reactants are in the same phase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Entropy

A

Measure of disorder of a system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

△G

A

Gibbs Free Energy change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Order of reaction

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Reversible reaction

A

Reaction that can go in either direction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Dynamic equilibrium

A

Rate of forward reaction = Rate of reverse reaction.

The concentration of all species remain unchanged

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Partition coefficient, Kpc / Kpartition

A

Ratio of concentration of a solute in the two immiscible solvents at equilibrium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Transition element

A

Element that forms 1 or more stable ions with partially filled d-orbital

25
Q

Ligand

A

Species that uses LP to form dative covalent bonds to a central metal atom or ion

26
Q

Monodentate ligand

A

A species that donates a LP of e- to central metal atom or ion

27
Q

Bidentate ligand

A

An ion/molecule that donates 2 LPs of e- to central metal atom/ion

28
Q

Polydentate ligand

A

A species that donate more than 1 LPs of e- to central metal atom/ion

29
Q

Bidentate

A

An ion/molecule that donates 2 LPs of e- to central metal atom/ion

30
Q

Complex ion

A

An ion formed by a central metal atom/ion bonded to one or more ligands

31
Q

Degenerate

A

Orbitals have the same E

32
Q

Coordination number

A

The no. of dative covalent bonds formed by the central metal atom/ion

33
Q

Stability constant

A

Equilibrium constant for the formation of a complex ion in a solution

34
Q

Structural isomer

A

Same number and type of atoms but different structural formula

35
Q

Chiral centre

A

A carbon atom that has 4 different atoms or groups attached it

36
Q

Stereoisomerism

A

Compounds that have the same structural formula but different spacial arrangements

37
Q

Buffer solution / Buffer

A

A solution that resists the change of pH when a small amount of acid or alkali is added to it

38
Q

Electronegativity

A

The attraction by an atom of the e- in a bond

39
Q

Homolytic fission

A

Breaking of a bond to form two radicals

40
Q

Free radical

A

Species with an unpaired e-

41
Q

Protein

A

A polymer of amino acids joined by peptide bonds

42
Q

.

A

.

43
Q

Secondary structure

A

alpha-helix / beta-sheet

44
Q

Tertiary structure

A

folding of chains / 3D shape

45
Q

Polymerisation

A

Many monomers forming a polymer

46
Q

Condensation polymer

A

A polymer formed by the elimination of a small molecule

47
Q

Double helix

A

Two interlinked spirals

48
Q

Nano-sized

A

Measured in nm, btw (10^-9 to 10^-6)

49
Q

Nanosphere

A

Spheres with a diameter in the nanometre range

50
Q

Retention time

A

Time take for a compound to travel through the column

51
Q

Partition

A

Separation due to the different solubilities of the compounds in two phases

52
Q

Adsorption

A

Separation due to the different attractions between the compounds and the stationary phase, relative to their solubility in the solvent

53
Q

Rf value

A

Distance travelled by a compound from baseline over the distance travelled by the solvent front

54
Q

Zwitterion

A

Species having positive and negative ionic charges but no overall charge

55
Q

Hydrophobic

A

Cannot form bonds with water molecules

56
Q

Density of a substance

A

Mass per unit volume

57
Q

Transition metal complex

A

Ion or molecule formed by a central metal atom/ion and surrounded by 1 or more ligands

58
Q

Electronegativity, and how it relates to the concept of bond polarity

A

Electronegativity is the attraction by an atom of the electrons in a bond.
Bond polarity is the difference in electronegativities at each end of the bond.

chem A2 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions