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Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

D block

A

Elements where d shell level is the highest energy sub shell containing electrons

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2
Q

Cr electron structure

A

[Ar] 4s 1 3d 5
Gives additional stability to atom half filled sub shell

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3
Q

Cu electron structure

A

[Ar]4s1 3d10 full d orbital giving additional stability

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4
Q

Transition elements

A

D block elements that form at least one ion with a partially filled d orbital
Sc and zinc aren’t (Sc loses 3e-) (Zn forms a full d orbital)

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5
Q

Properties of trans metals and compounds

A

Form compounds which transition element has different oxidation states
Form coloured compounds
Act as catalysts

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6
Q

Complex ions

A

One of most important properties of d block element
When one or more negatively charged ions bond to a central metal ion molecules are called ligands

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7
Q

Ligand

A

A molecule or ion that donates a pair of electrons to form a coordinate bond

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8
Q

Coordinate bond

A

When one of the bonded atoms provide both of the electron for the shared pair

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9
Q

Coordination number

A

Number of coordinate bonds attached to the central metal ion

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10
Q

Monodentate ligands

A

Donate one pair of electrons to a central metal ion

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11
Q

Shapes of complex ions

A

Octahedral
Tetrahedral
Square planar

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12
Q

Octahedral

A

The most common shape
6 coordinate bonds

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13
Q

Tetrahedral

A

4 coordinate bonds
109.5 degrees
CuCl4 for example

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14
Q

Square planar

A

4 coordinate bonds occurs in ions with 8 d electrons
90 degree bond angles

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15
Q

Cis trans in complex ions

A

Most common in square planar complexes
Cis= 2 adjacent identical groups 90
Trans = 2 identical opp side 180

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16
Q

Monodentate ligands in cos trans

A

Octahedral
90 degrees away = cis
180 degrees away = trans opposite side

17
Q

Bidentate ligands cis trans

A

Bidentate ligands adjacent = cis
Bidentate ligands are opp = trans

18
Q

Optical isomerism

A

Non superimposable mirror images of each other
Only possible with 3 Bidentate ligands 2 Bidentate + 2 mono
1 hexadentate ligand

19
Q

Ligand substitution

A

When one ligand is replaced by a different / another ligand in a complex ion

20
Q

Ligand sub with nh3 and [Cu(H20)6]^2+

A

Pale blue to dark blue solution
4 H20 ligands replaced by 4 NH3 ligands
Cu(OH)2 pp forms and then dissolved in excess ammonia

21
Q

Ligand substitution with Cl- (conc HCl)

A

Pale blue to yellow solution
6 H2O replaced by 4 Cl-
Octahedral -> square planar
Cl- ions are larger than H2O so fewer can fit round Cu 2+

22
Q

Reactions of Cr ions

A

Cr(H2O)6 ^3+ violet
Ammonia - Cr(OH)3 (grey/green) formed dissolves in excess ammonia -> purple

23
Q

Ligand sub in haemoglobin

A

Oxygen bonds to Fe2+ of haem group
Co2 also bonds to Fe2+
Carbon monoxide binds to form carboxyhaemoglonin which binds v strongly so ligand sun doesn’t occur
Oxygen cannot be picked up

24
Q

Precipitation reactions

A

When 2 aq sol containing ions react together to form an insoluble ionic solid

25
Q

Transition metals and precipitation

A

+ aq sodium hydroxide and aq ammonia
Form pp
Some may dissolve further to form complex ions

26
Q

Addition of NaOH ( insoluble)

A

Cu2+ blue sop to form insoluble blue pp Cu(OH)2
Fe2+ pale green sol form green pp Fe(OH)2 turns brown at surface
Fe3+ pale yellow to form orange brown pp Fe(OH)3
Mn2+ pale pink to light brown pp Mn(OH)2

27
Q

Addition of NaOH ( soluble)

A

Cr3+ violet forms grey green pp
Soluble in excess forming dark green solution -> [Cr(OH)6]^3-

28
Q

Further addition of ammonia

A

Cu(OH)2 -> [Cu(NH3)4(H2O)2]2+ blue pp to deep blue sol
Cr(OH)3 -> [Cr(NH3)6]^3+ green pp to purple solution
Fe2+,Fe3+ and Mn2+ react with excess ammonia forming pp of Fe(OH)2 for example

29
Q

Iodine thiosulphate equation

A

2S2O3 2- + I2 => 2I- + S4O6 2-
Starch black blue to colourless

30
Q

S2O3 2-

A

Thiosulphate ions are oxidised lose 2e-
2 per I2
1:1 thiosulphate ions to iodide ions I-

31
Q

I2

A

Iodine is reduced
Gains 2e-

32
Q

Thiosulphate ratios

A

1:1 ratio = Cu 2+ : S2O3 2-
S2O3 2- : I-
2:1 ratio= S2O3 2- : I2

Chemistry (20 decks)

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