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Chemistry Class 12 > Coordinate Compounds > Flashcards

Coordinate Compounds Flashcards

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1
Q

Coordinate compounds

A

Those compounds in which metal atoms or ions are bonded to ions or neutral molecules by coordinate bond

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2
Q

The product written in [] is called __ and outside is __

A

Complex part; counter ion

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3
Q

Product when Cuso4 + nh3

A

[Cu(NH3)⁴]SO⁴

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4
Q

Product of NiCl² + 4nh3

A

[Ni(nh3)⁴]Cl

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5
Q

Ligands are

A

Charged ions or neutral molecules that can give 2 e’s to form coordinate bond

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6
Q

How many ions will form when h20 + [Co(nh3)⁴Cl²]Cl?

A

2, i.e [Co(nh3)⁴Cl²] & Cl

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7
Q

Which will ionise in solution, Double salt or coordinate compds?

A

Double salt

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8
Q

Monodentate/unidentate ligands

A

Ligands which are able to form only 1 coordinate hond

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9
Q

Examples of monodentrate

A

NH³,H2O,PH³,P(C⁶H⁵)³,CH³-NH²
charged ligands like hallides, OH, NO², NO³

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10
Q

Ambidentate ligands

A

Ligands that can form bonds in 2 ways by 2 atoms

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11
Q

Ambidentate ligands examples

A

A metal with NO², SCN

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12
Q

Bidentate ligands

A

Ligands which can form only 2 bonds

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13
Q

Ex of bidentate

A

NH²–CH²-CH²–NH² where N has 1 lone pair, oxalic acid,glycine

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14
Q

Coordination compounds of Mg, Fe & Co

A

Chlorophyll,haemoglobin & Vitamin B¹²

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15
Q

Applications of coordination compounds

A

Electroplating, textile dyeing & medicinal chemistry

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16
Q

Ex of double salts

A

Carnallite,KCl.MgCl2.6H2O,Mohr’s salt,potash alum

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17
Q

Central atoms are also called

A

Lewis acids

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18
Q

Number of ligating groups are called

A

Denticity of the ligand

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19
Q

Oxalic acid structure

A

HooC-CooH

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20
Q

Among amino acids, which one is optically inactive

A

Glycine ²HN-CH²-COOH since it is not chiral

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21
Q

Ex of hexadentate ligands

A

Ethylene diamine tetraacetate ion(EDTA⁴-), [Co(en)³]³+

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22
Q

Among [Co(Nh3)⁶]³+ and [Co(en)³]³+ which is more stable?

A

[Co(en)³]³+ since it forms a ring structure

23
Q

Chelate ligand

A

Di- or polydentate ligand that uses its 2 or more atoms to bind

24
Q

Which complex is more stable? Chelate or unidendate?

A

Chelate

25
Q

Coordination polyhedral

A

Shape of the complex decided by no of bonds formed

26
Q

Coordination number

A

The no of coordination bonds the ligands are forming with metal

27
Q

Homoleptic vs heterolyptic complex

A

All ligands are same; different

28
Q

Cation complex

A

Complexes with only +vely charged part

29
Q

OH- name

A

Hydroxo

30
Q

NO² name

A

Nitrito-N or nitrito-O

31
Q

SO⁴ name

A

Sulphato

32
Q

(CO³)²- name

A

Carbonato

33
Q

Nh3 name

A

Ammine

34
Q

H20 & CO name

A

Aqua; carbonyl

35
Q

NO name

A

Nitrocyl

36
Q

(C2O8)²- name

A

Oxalato

37
Q

Werner’s theory

A

A metal ion has a primary & secondary valence where primary is satisfied by ions & secondary by ligands

38
Q

Postulates of werner’s theory

A

Metals show 2 linkages-primary & sec
Primary are satisfied by -ve ions and are ionisable
Secondary are non-ionisable & satisfied by neutral molecules
Ions bound by sec have spatial arrangements

39
Q

Elements from 20 to 30

A

Sc,Ti,Vi,Cr,Mn,Fe,Co,Ni,Cu,Zn

40
Q

Valence bond theory

A

Metal atoms or ion under the influence of ligands can use its orbitals for hybridization to yield a set of equivalent orbitals of definite geometry

41
Q

Why is [Co(nh3)⁶]³+ diamagnetic?

A

Absence of unpaired electrons

42
Q

Spin magnetic moment

A

No of unpaired electrons
Myu = [(n+2)n]½ BM

43
Q

Myu is 0 for

A

Diamagnetic substances

44
Q

2 exceptions btw 20 and 30 Atomic nos

A

Cromium and Copper

45
Q

If a substance has d²sp³ it is

A

An inner orbital complex

46
Q

How to identify strong and weak ligands

A

C>N>O>X

47
Q

Hybridisation & shape of 4 ligands

A

sp³ - tetrahedral
dsp² - square planar

48
Q

Hybridisation & shape of 5 ligands

A

dsp³ & sp³d - trigonal bipyramidal

49
Q

Hybridisation & shape of 6 ligands

A

sp³d² or d²sp³ - octahedral

50
Q

Total magnetic moment

A

Orbital MM + spin MM

51
Q

Drawbacks of VBT

A

Doesn’t tell why some subs are inner orbital and outer orbritsl complexes
Doesn’t differentiate b/n strong & weak ligands
In some, actual MM & calculated MM are not same
Couldn’t explain why [Cu(NH3)⁴]²+ is square planar & not tetrahedral
Couldn’t explain why some NI(||) complexes are paramagnetic

52
Q

Crystal field theory

A

When a metal atoms or ion is surrounded by -vely charged ligands, electrostatic forces exist b/n them (ionic bond).
Ligands are point -ve charges.
Degeneration of metal orbitals are lost due to repulsion b/n orbitals.
D-orbitals will be split according to the geometry of the complex

53
Q

Among d(xy), d(yz), d(xz), d(x²-y²) & d(z²), which has more energy?

A

d(x²-y²) & d(z²)

54
Q

Energy difference caused due to splitting is

A

Crystal field splitting theory
Denoted by delta°

Chemistry Class 12 (10 decks)

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