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a level chemistry > reaction of aqueous ions > Flashcards

reaction of aqueous ions Flashcards

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1
Q

write the formula of a metal aqua ion (2+ and 3+ charges)

A

[M(H2O)6] 2+

[M(H2O)6] 3+

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2
Q

why are aqueous metal ions acidic

A
  • the aqueous metal ion is polarising
  • pulls electron density off H2O ligands
  • weakens O-H bond

(water ligands can be deprotonated

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3
Q

how many water ligands are deprotonated for 2+ and 3+ metal aqua ions

A

2 for 2+ ions

and

3 for 3+ ions

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4
Q

explain why deprotonated metal aqua ions are insoluble

A

they have no overall charge

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5
Q

explain why [M(H2O)6] 3+ ions are more acidic than [M(H2O)6] 2+ ions

A

smaller and more highly charged so has high charge density so very polarising so pulls more electron density off of water ligands

easier to deprotonate water ligands in 3+ ions

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6
Q

write an equation for the reaction of aqueous Cu2+ ions with NaOH

A

[Cu(H2O)6] 2+ + 2OH- —> Cu(H2O)4 (OH)2 + 2H2O

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7
Q

write an equation for the reaction of aqueous Co3+ with dilute NH3

A

[Co (H20)6 ] 3+ + 3NH3 —> CO (H2O)3 (OH) 3 (s) + 3NH4+

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8
Q

what is the colour of aqueous [Cu (H20)6 ] 2+ ions

A

blue solution

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9
Q

what is colour of aqueous [Fe (H20)6 ] 2+ ions

A

green solution

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10
Q

what is the colour of aqueous [ Fe (H20)6 ] 3+ ions

A

brown/purple solution

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11
Q

what is the colour of aqueous [Al (H20)6 ] 3+ ions

A

colourless solution

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12
Q

write the simplest ionic equation for the reaction of [M (H20)6 ] 2+ ions with sodium hydroxide solution

A

[M (H20)6 ] 2+ (aq) + 2OH- (aq) —-> M (H2O)4 (OH)2 (s) + 2H2O (l)

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13
Q

write the simplest ionic equation for the reaction of [M (H20)6 ] 3+ ions with sodium hydroxide solution

A

[M (H20)6 ] 3+ (aq) + 3OH- (aq) —-> M (H2O)3 (OH)3 (s) + 3H2O (l)

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14
Q

give an observation when Fe2+ (aq) reacts with NaOH

A

green solution –> green ppt —> turns into brown ppt when in air due to oxidation with oxygen to Fe3+

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15
Q

give an observation when Cu2+ (aq) reacts with NaOH

A

blue solution —> blue ppt

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16
Q

give an observation when Fe3+ (aq) reacts with NaOH

A

brown/purple solution —> brown ppt

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17
Q

give an observation when Al3+ (aq) reacts with NaOH

A

colourless solution —> white ppt

18
Q

write the simplest ionic equation for the reaction of [M (H2O)6 ] 2+ ions with ammonia solution

A

[M (H2O)6 ] 2+ (aq) + 2NH3 (aq) —> M (H20)4 (OH)2 (s) + 2NH4+ (l)

19
Q

write the simplest ionic equation for the reaction of [M (H2O)6 ] 3+ ions with ammonia solution

A

[M (H2O)6 ] 3+ (aq) + 3NH3 (aq) —> M (H20)3 (OH)3 (s) + 3NH4+ (l)

20
Q

what happens when excess ammonia is reacted with Cu2+ (aq)

and give equation for the reaction

A

blue ppt —> royal blue solution

[Cu (H2O)6] 3+ (aq) + 4NH3 —> [Cu (H2O)2 (NH3)4 ] 2+

due to a ligand displacement reaction

21
Q

Write the simplest ionic equation for the reaction of [M (H2O)6 ] 3+

A

2 [M(H2O)6 ] 3+ (aq) + 3CO3 2- (aq) ——> 2M (H2O)3 (OH)3 (s) + 3H2O + 3CO2

22
Q

What observation is made when M3+ ions react with sodium carbonate solution

A

Bubbles/ effervescence due to CO2 production

23
Q

Explain why [M (H2O)6 ]2+ ions do not react with sodium carbonate solution

A

[M (H2O)6 ] 2+

24
Q

Why can Al(OH)3 be described as amphoteric

A

Acts as both an acid and a base

25
Q

When happens when excess NaOH is added to Al3+ (aq) ppt

A

Precipitates redissolves, because Al3+ ions more acidic and can further deprotonated

Al(OH)3 acts as an acid

26
Q

Write the simplest ionic equation for the reaction of [M(H2O)6 ] 2+ with sodium carbonate solution

A

M(CO3) + 6H2O

27
Q

write the equation for when Al (H2O)3 (OH)3 reacts with excess NaOH

A

Al (H2O)3 (OH)3 + OH- —-> [Al (H2O)2 (OH)4 ]- + H2O

28
Q

write the equation for when Al (H2O)3 (OH)3 reacts with excess HCl

A

Al (H2O)3 (OH)3 + 3HCl —–> AlCl3 + 6H2O

29
Q

define a bronstead lowry acid

A

proton ( H+) donor

30
Q

define a bronstead lowry base

A

proton (H+) acceptor

31
Q

put these bases in order of their strength

NH3
NaOH
Na2CO3

A

NaOH ( OH-) strong base

NH3 (NH3) weak base

Na2CO3 ( CO3 2-) very weak base

32
Q

what will sodium carbonate deprotonate

A

stronger M3+ ions

not M2+ ions

33
Q

define a lewis acid

A

electron pair acceptor

34
Q

define lewis base

A

electron pair donor

35
Q

what colour is FeCO3

A

green ppt

36
Q

what colour is CuCO3

A

blue/green ppt

37
Q

what 3 ways can the exam board refer to aqueous metal ions

A
  • aqueous metal ions
  • aqua metal ions
  • metal aqua ions
38
Q

what 2 factors affect the relative acidity of metal ions

A

size

charge

(charge density which then affects polarisability)

39
Q

write the product formed when aqueous aluminium reacts with excess NaOH

A

[Al (H2O)2 (OH)4 ]-

40
Q

write the product formed when aqueous aluminium reacts with excess NH3

A

Al (H2O)3 (OH)3

a level chemistry (49 decks)

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