Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > 4. inorganic chemistry and the periodic table > Flashcards

4. inorganic chemistry and the periodic table Flashcards

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

what do group 2 metals form when they react

A

2+ ions

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

what happens to the atomic radius of group 2 metals down the group

A

it increases due to increased electron shells

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

what happens to the reactivity of group 2 metals down the group

A

it increases due to increased shielding

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

what happens to first ionisation energy of group 2 metals down the group

A

it decreases due to greater atomic radius and increased shielding

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

what happens when group 2 metals react with water

A

produces a metal hydroxide and hydrogen.

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

what happens when group 2 metals react with chlorine gas

A

they form metal chlorides ( white precipitate)

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

what happens when group 2 metals react with oxygen

A

they form oxides

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

what happens when strontium and barium react with excess oxygen and heat energy

A

they form metal peroxides

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

what happens when group 2 metals react with dilute acids

A

produces hydrogen gas and solutions of metal compounds

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

what happens when group 2 hydroxides react with dilute acid

A

they form a salt and water - neutralisation

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

what happens to the solubility of group 2 hydroxides down the group

A

they increase

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

what happens to the solubility of group 2 sulfates down the group

A

they decrease

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

what can you use to test for sulfate ions

A

barium chloride, it reacts to form barium sulfate which is a white precipitate

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

what group 2 metals undergo thermal decompositions

A

group 2 carbonates and nitrates

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

how does thermal decomposition occur

A

heating the substance in lots of oxygen

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

what do group 2 carbonates produce when they undergo thermal decomposition

A

carbon dioxide and a metal oxide which forms as a white powder

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

what do group 2 nitrates produce when they undergo thermal decomposition

A

nitrogen dioxide and oxygen with a metal oxide which forms as a white powder

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

what is required as you go down group 2 for thermal decomposition

A

more heat as the ions increase in size and thermal stability increases.

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

how do group 1 carbonates react in thermal decomposition

A

they dont decompose upon heating in a lab as they require extremely high temperatures

20
Q

how do group 1 nitrates react in thermal decomposition

A

they produce a metal nitrite and oxygen.

21
Q

what group 1 element decomposes in the same way as group 2 elements

A

lithium

22
Q

explanation of thermal stability trend down groups 1 and 2

A

as you go down the group they form more stable carbonates and nitrates so they require more energy to undergo thermal decomposition.

23
Q

what happens to the charge density as you go down group 1 and 2

A

it decreases as the ionic radius increases as you go down but the charge stays the same so the charge density decreases.

24
Q

how to carry out a flame test

A
  1. nichrome wire and clean it in concentrated HCL then into a blue flame
  2. repeat the cleaning until no colour is produced in the flame
  3. dip the wire into the unknown metal compound and place it into the flame
  4. observe the colour produced
25
Q

flame colour of lithium

A

red

26
Q

flame colour of sodium

A

orange/yellow

27
Q

flame colour of potassium

A

lilac

28
Q

flame colour of magnesium

A

no colour

29
Q

flame colour of calcium

A

brick red

30
Q

flame colour of strontium

A

crimson red

31
Q

flame colour of barium

A

pale green

32
Q

how do the colours in the flame tests occur

A

electron transitions:
when energy is supplied by heat, the electrons move to orbitals with higher energy then drop back down to their original orbital. this produces energy in the form of light.
the amount of energy released during this is shown through a unique wavelength that produces the colour.
if the wavelength produces a colour not on the visible spectrum you will not see a colour emitted.

33
Q

what are group 7 elements

A

halogens, highly reactive non metals

34
Q

what happens to the atomic radius of group 7 elements down the group

A

it increases due to additional electron shells

35
Q

what happens to the electronegativity of group 7 elements as you go down the group

A

decreases as the atomic radius and electron shielding increases meaning the outer electrons are less strongly attracted to the nucleus and can be removed easier

36
Q

what happens to the melting and boiling points down group 7

A

it increases. they are simple covalent molecules that are held together by london forces. as the relative atomic mass increases, the amount of london forces increases meaning more energy is required to overcome them.

37
Q

what happens to reactivity down group 7

A

it decreases due to the increased distance from the nuclei to the outer electrons, this increases atomic radius and increased shielding makes it harder to attract electrons to react.

38
Q

why are group 7 good oxidising agents

A

the oxidising power decreases down the group so the halogen will replace the halide beneath it. cl2 can displace br- and br2 will displace i-

39
Q

what is a halide ion

A

a negative ion of a halogen

40
Q

halide ions are good reducing agents what happens to reducing power down the group

A

it increases a electrons are easier to lose and they form larger ions due to shielding and larger atomic radius

41
Q

how to distinguish halide ions

A
  1. add acidified silver nitrate
    Cl- white precipitate
    Br- cream precipitate
    I- yellow precipitate
    Can be tested further by using dilute and concentrated ammonia
42
Q

what happens when a hydrogen halide reacts with ammonia gas

A

forms ammonia salts

43
Q

what happens when hydrogen halides react with water

A

form dilute acids

44
Q

how to test for sulfate ions

A

acidified barium chloride - white precipitate produced. barium sulfate

45
Q

how to test for carbonate and hydrogencarbonate

A

add HCl - bubbles produced
collect gas and bubble through limewater, limewater turns cloudy if CO2 is present

46
Q

test for ammonium ions

A

add NaOH and gently warm to produce ammonia gas. hold damp red litmus paper over the substance and it will turn blue if ammonium ions are present

47
Q
A

Chemistry (14 decks)

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