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Chemsitry A Level > Key Words > Flashcards

Key Words Flashcards

1
Q

Ligind

A

Molecule or anion with a lone pair of electrons that can form a dative covalent bind with a central metal cation.

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2
Q

Pair of optical isomer

A

2 non superimposable mirror images

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3
Q

Electrophile

A

Positively/ partially positively charged species (no line pair)-can break a double bond

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4
Q

Nucleophile

A

Partially/fully negatively charged species that donates electrons to have a positive charge= forms a covalent bond

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5
Q

Year 1 mechanisms

A

Nucleophilic substitution-reaction with water/hydroxide ions

Electrophilic addition-bromine across a double bond

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6
Q

Year 2 mechanisms

A

Electrophilic substitution-eg swapping a H in a benzene ring

Nucleophilic addition-breaking double O bonds in carbonyls

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7
Q

Electron donating group

A

Pushed onto 2,4,6 positions
Lone pair delocalises into the ring
More reactive than benzene in electro sub

Eg OH and NH_2

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8
Q

Electron withdrawing groups

A

-3,5 positions
Pulls electrons away from group
Less reactive than benzene in electro sub

Eg NO_2

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9
Q

Aliphatic

A

Straight chained, branches or non aromatic rings

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10
Q

Alicyclic

A

Alicyclic compound arranges in a non aromatic ring with side chains

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11
Q

Aromatic

A

Compounds that contain an arene (benzene) ring

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12
Q

Co-polymerisation

A

Mix up of different monomers (more than 2)

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13
Q

Thermosetting polymers

A

Once moulder do not soften again eg tyres

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14
Q

Thermoplastic polymer

A

Becomes pliable/mouldable at a specific temperature and solidified upon cooling

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15
Q

Amine

A

H of NH_2 group replaces by a carbon

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16
Q

Amide

A

N attached to C=O

17
Q

Nitrile

A

R-CN

18
Q

Lattice enthalpy

A

1 mole of ionic compound formed from gaseous ions in standard conditions

19
Q

Enthralled of solution

A

1 mole of solute dissolves in a solvent (water)

20
Q

Enthalpy of ionisation

A

1 electron removes from each atom in 1 mole of gaseous atoms

Ea is the reverse

21
Q

Enthalpy of formation

A

1 mole of compound formed from elements in standard states and conditions
(Products)-(reactants)

22
Q

Exothermic

A

Heat energy transferee to the surroundings (bond making)

23
Q

Endothermic

A

Heat energy is absorbed from the surroundings (bond breaking)

24
Q

Standard enthalpy of combustion

A

When 1 mole of substance is completely burned in O2 under standard conditions

25
Q

Standard enthalpy of neutralisation

A

When acid and base react in standard states to form 1 mole of water

26
Q

Bond enthalpy

A

Average energy required to break 1 mole of binds in gaseous molecules

27
Q

Trends in group 2

A

Reactivity increases down the group

First ionisation energy decreases

Oh increased down the group and alkability increases

28
Q

Ka=[H+]2/[HA] assumptions

A

HA equilibrium= initial
All H+ from HA
[H+]=[A-]

29
Q

Buffer assumptions

A

[weak acid] equilibrium=initial

All conjugate base from salt not acid

30
Q

Buffer
Add H+

Add OH-

A

H+= shift to left

OH-= shift to right to restore H+
Reacts to produce water

31
Q

Examples bidentate liginds

A

C_2O_42-

H_2NCH_2CH_2NH_2

32
Q

Periodicity

Down a group

A

Atomic radius increases=increased shielding

Increase nuclear charge rules out

First ionisation energy decreases

33
Q

Periodicity

Across period

A

Atomic radius decreases

Shielding stays the same

Higher nuclear charge=strong attraction

First ionisation energy increases

34
Q

Qualitative analysis

A

1-carbonate-dilute nitric acid

2-Sulphate test-add barium

3-halide test-add silver nitrate

4-test for cations-NaOH=produce ammonia gas

35
Q

Primary cell

A

Non rechargeable
Low current
Long storage
Alkaline based

36
Q

Secondary cells

A

Rechargeable

Lead-acid nickel-calcium lithium-ion

37
Q

Fuel cells

A

Fuel react with O_2
Operate continuously
Not have to be recharged

Hydrogen fuel cell- +1.23V
Acid or alkali
H_2 +1/2 O_ = H_2O

Chemsitry A Level (5 decks)

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