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01AVS A Periodic table, elements and physical chemistry PM 13th June COPY > Chapter 24 Key Concepts > Flashcards

Chapter 24 Key Concepts Flashcards

1
Q

Properties of the d block elements

A

catalysts

color change

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2
Q

uses of Ag Ni Cu Zn

A

coinage

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3
Q

uses of iron

A

construction

making tools

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4
Q

uses of copper

A

electric cables

water pipes

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5
Q

uses of Ti

A

aerospace
joint replacement
cosmetic dentistry

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6
Q

what are the two strange d block elements and what is so strange about them

A

Chromium
-should be 3d4 4s2 but it is 3d5 4s1. this is for added stability the half filled d5 shell brings
Copper
- should be 3d9 4s2 but it is 3d10 4s1. this is for added stability that a fully filled d10 sub shell brings

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7
Q

what two d block elements are, by definition NOT transition elements

A

Scandium
-only makes Sc 3+. the highest energy level is 3p. d orbital is empty
Zinc
-only makes Zn2+. highest energy level is 3d10. not a partially filled d orbital.

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8
Q

characteristics of a transition elements that sets them apart from other entals

A

form colored compounds
their elements and compounds can act as catalysts
they form compounds where the transition element has different ox states

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9
Q

Ti oxidation state and colour

A

2
3 pink
4
5

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10
Q

V oxidation state and colour

A

2 pink
3 green
4 blue
5 yellow

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11
Q

Cr oxidation state and colour

A 
2 blue
3 green
4
5
6 orange
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12
Q

Mn oxidation state and colour

A 
2 pink
3
4 mauve
5
6 green
7 violet
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13
Q

Fe oxidation state and colour

A 
2 pale green
3 pale yellow
4
5
6
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14
Q

Co oxidation state and colour

A

2 pink
3 green
4
5

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15
Q

Ni oxidation state and colour

A

2 green
3
4

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16
Q

Cu oxidation state and colour

A

1
2 blue
3

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17
Q

what’s the color of K2Cr207

A

bright orange

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18
Q

color of Nickle 2 sulfate?

A

green

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19
Q

color of hydrated copper sulfate?

A

blue

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20
Q

whats the transition metal catalyst in the Haber process?

A

Fe

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21
Q

whats the transition metal catalyst in the contact process?

A

Valadium as Valadium trioxide

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22
Q

whats the transition metal catalyst in the hydrogenation of vegetable fats to make margarine?

A

ni

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23
Q

whats the transition metal catalyst in the catalytic decomposition of hydrogen peroxide?

A

Manganese as Mn02

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24
Q

whats the aq transition metal catalyst in the reaction of Zn with acids

A

Cu2+ aq

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25
Q

whats the aq transition metal catalyst in the reaction iodide ions and peroxodisulphate iond S2082-

A

Fe2+ aq

26
Q

how is a complex ions formed

A

when one or more molecules or negatively charged ions bind to a central mental ion to make a coordinate bond

27
Q

what color is [Cr(H20)6]3+

A

blue

28
Q

what color is [Cu(H20)6]2+

A

blue

29
Q

examples of monodentate ligands

A 
H20
NH3
Cl-
CN-
OH-
30
Q

examples of bidentate ligands

A 
1,2-diamoethane (em)
ethandioate ion (oxalate ion) 2-
31
Q

shape when 6 coordinate complexes?

A

octahedral . bond angle around the central metal ion is 90 degrees.
eg MnSo4 dissolved in water making [Mn(H206)]2+
eg. [Co(H2NCH2CH2NH2)

32
Q

shape when 4 coordinate complexes?

A

Tetrahedral
more common. 109.5. eg [Cu(Cl4)]2- (yellow) and [Co(Cl4)]2- (blue)

or square planar
only in complex ions of transition metals with 8 d electrons in the highest energy d sub-shell. eg Platinum 2+ Palladium 2+ Gold 3+.
eg.
[Pt(NH3)4]2+. 90 degrees

33
Q

Two types of steoisomerism that transition metals can show

A

cis trans

optical

34
Q

cis trans occurs in…

A

-some square planar with no more than 2 identical ligands attached to the central metal ion eg [Pd(NH3)2Cl2]

-octahedral complex ions
monodentate 4 or 2 of the other [Co(NH3)4Cl2]2+
bidentate [Co(en)2Cl2]+

35
Q

cis trans AND optical occur in …

A

some octahedrals containing two or more bidentate ligands

36
Q

angle of the identical ligands in the trans isomenr

A

180

37
Q

angle of the idential ligands in the cis isomenr

A

90

38
Q

what happens when CO binds to haemoglobin

A

makes carboxyhaemoglobin. when con too high O2 transport prevented and leads to death,

ligand sub takes lace, O2 replaced by CO

CO binds more strongly than O2, so strong the process is irreversible

small CO can prevent a lot of hemoglobin molecules carrying O2

39
Q

Cu ppt reaction with ammonia

A

1.Cu2+ + 2OH- —> Cu(OH)2 (s)
pale blue to blue ppt

2.[Cu(H20)6]2+ +4NH3–> [Cu(NH3)4(H20)2]2+ +4H20

ppt distolves in excess ammoniua to make to dark blue solution

40
Q

Cr ppt reaction with ammonia

A

1.Cr3+ + 2OH- —> Cr(OH)3 (s)
violet to grey-green ppt

2.[Cr(H20)6]3+ +6NH3–> [Cr(NH3)6]3+ +6H20

green ppt distolves in excess ammoniua to make to dark purple solution

41
Q

Fe 2+ ppt reaction with ammonia

A 
Fe2+ + 2OH- ---> Fe(OH)2 (s)
pale green to green ppt.
in air 
Fe(OH)2 ---> Fe(OH)3
orange brown ppt  
no further reaction with NH3 as these ppt don't dissolve
42
Q

Fe 3+ ppt reaction with ammonia

A

Fe3+ + 2OH- —> Fe(OH)3 (s)
pale yellow to orange-brown ppt

no further reaction with NH3 as these ppt dont dissolve

43
Q

Mn ppt reaction with ammonia

A

Mn2+ + 2OH- —> Mn(OH)2 (s)
pale pink to light brown ppt
no further reaction with NH3 as these ppt dont dissolve

44
Q

Cu ppt reaction with aq NaOH

A

1.Cu2+ + 2OH- —> Cu(OH)2 (s)
pale blue to blue ppt

ppt is insoluble in excess NaOH

45
Q

Fe 2+ ppt reaction with aq NaOH

A 
Fe2+ + 2OH- ---> Fe(OH)2 (s)
pale green to green ppt.
in air 
Fe(OH)2 ---> Fe(OH)3
orange brown ppt

ppt is insoluble in excess NaOH

46
Q

Fe 3+ ppt reaction with aq NaOH

A

Fe3+ + 2OH- —> Fe(OH)3 (s)
pale yellow to orange-brown ppt

ppt is insoluble in excess NaOH

47
Q

Mn ppt reaction with aq NaOH

A

Mn2+ + 2OH- —> Mn(OH)2 (s)
pink to light brown ppt

ppt is insoluble in excess NaOH

48
Q

Identifying Carbonate ions

A

add dilute HNO3 (aq) look for effervescence

H+(aq) + CO32-(aq) —> CO2(g) + H20(l)

49
Q

eq for Ox Fe2 to Fe3

A

basis of a redox titration.
add MnO4- ions in acid conditions
MnO4- (aq) +5Fe2+ (aq) +8H+(aq) => Mn2+ (aq) + 2Fe3+ (aq) + 7H20(l)

purple to colourless

50
Q

eq for Red of Fe3 to Fe2

A

2Fe3+ (aq) + 2I-(aq) –> 2Fe2+(aq) + I2(aq)
orange brown pale green brown

-colour change obscured by the ox of Iodide ions to make Iodine

51
Q

eq for dicromate (VI) to Cr3+

A

3Zn(s) +Cr2O72- (aq) +14H+(aq) => 3Zn2+ (aq) + 7H20 + 2Cr3+ (aq)

orange to green

52
Q

what do you get when you add hot alkaline hydrogen peroxide to Cr3+ aq? write the full eq

A

Oxidation of Cr3+ to Cr042-
10OH- + 4H202 + 2Cr3+ => 2Cr042- +8H20

*H202 is a a very strong ox agent

53
Q

what do you get when yu react hot dilute H2SO4 with Cu2O?

A

water, blue solution of CuSO4 and brown ppt of Cu

54
Q

aq Cu2+ reacts with excess iodide ions. what do you get? and what is the eq

A

reduction of Cu2+ to Cu+.
2Cu2+ (aq) + 4I(aq) –> 2CuI(aq) + I2(s)
pale blue white ppt brown

55
Q

write the further reduction of Cr3+ to Cr2+ in excess Zn

A

zn(s) +2Cr3+ (aq) => Zn2+ (aq) + 2Cr2+ (aq)

green pale blue

56
Q

what does a more positve e mean?

A

E value more positve

Eq more likely to gain electrons shift right and undergo reduction

57
Q

what does a more neg e mean?

A

E value more neg

Eq more likely to lose electrons shift left and undergo oxidation

58
Q

what does a more positive e mean?

A

E value more positive

Eq more likely to gain electrons shift right and undergo reduction

59
Q

[Cu(H2O)2(NH3)4]2+

A

Deep blue

60
Q

[Co(NH3)6]2+

A

Brown yellow solution

61
Q

[CuCl4]2-

A

Yellow

62
Q

[CoCl4]2-

A

Blue solution

01AVS A Periodic table, elements and physical chemistry PM 13th June COPY (14 decks)

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