Brainscape's Knowledge GenomeTM

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


See full index

A Level Chemistry > Periodic table > Flashcards

Periodic table Flashcards

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

what do elements in the same group have ?

A

same no. of electrons in outer shell — similar chemical properties

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

define first ionisation energy

A

energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms

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

what type of reaction is ionisation energy reactions ?

A

endothermic - energy needed to ionise an atom

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

what are the 3 factors of ionisation energy ?

A
  • nuclear charge
  • atomic radius
  • shielding (greatest factor)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what causes high ionisation energy ?

A

strong attraction between electron and nucleus, so more energy is needed to overcome the attraction and remove the electron

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

ionisation energy … down a group

A

decreases

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

why does ionisation energy increase across a period ?

A

positive charge of nucleus increases (no. of protons increases) which pulls electrons closer, decreasing atomic radius

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

why is there a ionisation energy drop between group 2 and 3 ?

A
  • group 3 elements go in p orbitals, which are found further from nucleus than s orbitals (larger atomic radius)
  • s electrons provide some shielding
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

why is there a ionisation energy drop between group 5 and 6 ?

A
  • in group 6, electron being removed from orbital with two electrons
  • repulsion between two electrons makes it easier to remove an electron
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is an allotrope ?

A

element that has different forms (in the same state)

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

what is the shape of the molecules in diamond ?

A

tetrahedral (carbon bonded to 4 other carbons)

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

what does sublime mean ?

A

change from solid straight to gas (no liquid phase)

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

why is diamond a good thermal conductor ?

A

vibrations travel easily through the stiff lattice

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

what specific structure does diamond have ?

A

crystal lattice structure

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

what structure does silicon have similar to ?

A

diamond

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

what causes graphite to be a good lubricant ?

A

arranged in layers, with weak H-bonds between them (easily broken), so sheets can slide over each other

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

how can graphite conduct electricity ?

A

has delocalised electrons which are free to move and can carry charge - electric current can flow

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

why is graphite less dense than diamond ?

A

layers are quite far apart compared to length of covalent bonds

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

why does graphite have a high melting point ?

A

strong covalent bonds in hexagonal sheets

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

why is graphene known as the best conductor ?

A

delocalised electrons / as well as it being 2D, so electrons can move quickly above / below sheet

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

what else do the delocalised electrons in graphene do ?

A

strengthen covalent bonds between carbon atoms (making it strong)

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

a single layer of graphene is …

A

transparent and light

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

what structure do metals exist as ?

A

giant metallic lattice structures

24
Q

what is metallic bonding ?

A

electrostatic attraction between metal cations and (sea of) delocalised electrons

25
Q

how are metals malleable / ductile ?

A

no specific bonds holding ions together, so can slide past each other

26
Q

what affects metal melting points ?

A
  • no. of delocalised electrons per atom

- site of metal ion

27
Q

why are metals good thermal conductors ?

A

delocalised electrons can pass kinetic energy to each other

28
Q

what is group 2 known as ?

A

alkali earth metals

29
Q

group 2 metal + water =

A

metal hydroxide + hydrogen

30
Q

group 2 metal burnt in (+) oxygen =

A

solid white metal oxide

31
Q

group 2 metal + water =

A

dissolved metal hydroxide (OH- ions make really alkaline)

32
Q

what is the use for calcium hydroxide ?

A

agriculture to neutralise acidic soil

33
Q

what is the use for magnesium hydroxide / calcium carbonate ?

A

indigestion tablets as antacids

34
Q

give state and colour of fluorine

A

pale yellow gas

35
Q

give state and colour of chlorine

A

green gas

36
Q

give state and colour of bromine

A

red-brown liquid

37
Q

give state and colour of iodine

A

grey solid

38
Q

what is another way of saying that halogens get less reactive down the group ?

A

they become less oxidising

39
Q

what is the test for halides ?

A
  • add dilute nitric acid (remove ions)
  • add silver nitrate solution
  • silver halide precipitate formed
40
Q

in the halide test, what colour precipitate does chlorine give ?

A

white

41
Q

in the halide test, what colour precipitate does bromine give ?

A

cream

42
Q

in the halide test, what colour precipitate does iodine give ?

A

yellow

43
Q

for Cl, Br, I, describe with ammonia solution

A

Cl - dissolve in dilute
Br - dissolves in conc
I - insoluble in conc

44
Q

what is a disproportionate reaction ?

A

reaction where a molecule is both oxidised and reduced

45
Q

what type of reaction do halogens undergo with alkalis ?

A

disproportionate reaction

46
Q

what do you get if you react chlorine with sodium hydroxide ?

A

bleach (NaClO) (disproportionation)

47
Q

give the uses of bleach

A

water treatment / paper and textiles

48
Q

how is bacteria killed in water ?

A
  • chlorine mixed with water
  • HCl + chloric(I) acid as products
  • chloric acid ionises, making chlorate ions
  • chlorate ions kill bacteria
49
Q

what (two) types of reaction is chlorine + water ?

A

disproportionation and reversible

50
Q

what is the test for carbonates ?

A
  • add dilute HCl
  • carbon dioxide will be released
  • test for CO2 using limewater (turn cloudy)
51
Q

what is the test for sulfates ?

A
  • add dilute HCl
  • add barium chloride solution
  • white precipitate of barium sulfate
52
Q

what is test for ammonia gas ?

A

damp piece of red litmus paper will turn blue

53
Q

what is test for ammonium ions ?

A
  • add NaOH
  • warm mixture
  • ammonia gas will be given off
54
Q

state colour of chlorine:
RTP -
(aq) -
dissolved in hexane -

A

RTP - green
(aq) - colourless
dissolved in hexane - colourless

55
Q

state colour of bromine:
RTP -
(aq) -
dissolved in hexane -

A

RTP - brown
(aq) - orange
dissolved in hexane - orange

56
Q

state colour of iodine:
RTP -
(aq) -
dissolved in hexane -

A

RTP - grey/black
(aq) - brown
dissolved in hexane - purple

A Level Chemistry (21 decks)

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