1. Explain why Mn2+ is more stable than Mn3+
Outer Electronic Configurations of
Mn (Z = 25) - 3d54s2
Mn2+ - 3d5 and
Mn3+ - 3d4
Mn2+ has stable half filled d – orbital when compared to Mn3+ which has partially filled d – orbital. Hence Mn2+ is more stable than Mn3+.
Or
Half filled 3d – orbital in Mn2+ have been most stable than Mn3+due to symmetry (Hund’s rule)
Hence Mn2+ is more stable than Mn3+.
2. What is the action zinc on hot NaOH solution?
Zinc dissolves in hot NaOH solution forming soluble zincate ion.
Zn + 2NaOH + 2H2O → Na2ZnO2 + H2O
Sodium zincate
3. Why are transition metal ions coloured?
1. The presence of unpaired electrons in transition metal ions.
2. The energy gap between two energy levels in the same d- subshell being small.
3. The very small amount of energy required for excitation of electrons from one energy level to the other is easily provided by the visible light.
4. The colour observed corresponds to the complementary colour of the light absorbed.
4. Why do d-block elements exhibit variable oxidation states? Or The transition elements show variable oxidation states. Give reason.
1. These elements have several (n – 1) d and ns electrons.
2. The energies of (n – 1) d and ns orbitals are fairly close to each other.
5. Why do transition elements form complexes? Or d-block elements form complexes compounds. Why?
1. Small size and high positive charge density.
2. Presence of vacant (n – 1) d orbitals which are of appropriate energy to accept lone pair and unshared pair of electrons from the ligands for bonding with them.
6. Write a note on chrome plating. Or How is chrome plating done?
In chrome – plating generally the articles are first plated with nickel and then subjected to chromium plating.
Anode - Lead.
Cathode - The articles to be plated with chromium.
Electrolyte – Chromic acid and Sulphuric acid
During electrolysis chromium deposits on the article (Cathode).
7. Write the action of aqua regia on gold. Or Write the reaction of gold with aqua regia.
Gold dissolves in aquaregia (3 parts of Con.HCl + 1 part of Con.HNO3) to form auric chloride.
2Au + 9 HCl + 3HNO3 → 2AuCl3 + 6H2O + 3NOCl
8. A substance is found to have a magnetic moment of 3.9 BM. How many unpaired electrons does it contain?
Squaring on both sides
15.21 = n2 + 2n
n2 + 2n – 15.21 = 0
Solving
Number of unpaired electrons n= 3
9. Explain Chromyl chloride test with equation.
When salt containing chloride is treated with K2Cr2O7 and Con. H2SO4 reddish brown vapours of chromyl chloride (CrO2Cl2) are obtained.
When salt containing chloride is treated with K2Cr2O7 and Con. H2SO4 reddish brown vapours of chromyl chloride (CrO2Cl2) are obtained.
K2Cr2O7 + 4KCl + 6H2SO4 → 2CrO2Cl2 + 6 KHSO4 + 3H2O
10. Explain electrolytic refining of copper.
For electrolytic refining of copper,
Anode - Impure copper metal.
Cathode - Pure copper metal.
Electrolyte - Copper sulphate solution acidified with Sulphuric acid.
When electric current is passed through the electrolytic solution pure copper get deposited on the cathode, impurities settle near the anode in the form of sludge called anode mud.
11. Give any two evidences for the oxidising nature of potassium dichromate.
In presence of dil. H2SO4, one mole of K2Cr2O7 gives three atoms of oxygen.
K2Cr2O7 + 4 dil. H2SO4 → K2SO4 + Cr2 (SO4)3 + 4H2O+ 3(O)
K2Cr2O7 liberates I2 from KI
K2Cr2O7 + 7H2SO4 + 6KI → 4K2SO4 + Cr2 (SO4)3 + 3I2 + 7H2O
K2Cr2O7 oxidises ferrous to ferric salt
K2Cr2O7 + 7H2SO4 + 6 FeSO4 → K2SO4 + Cr2 (SO4)3 + 3Fe2 (SO4)3+ 2H2O
K2Cr2O7 oxidises H2S to sulphur
K2Cr2O7 + 4H2SO4 + 3H2S → K2SO4 + Cr2 (SO4)3 + 7H2O + 3S
12. How is Purple of Cassius prepared?
Purple of Cassius is prepared by mixing very dilute solution of gold chloride with stannous chloride solution. It is only a form of colloidal gold
2AuCl3 + 3 SnCl2 → 2Au↓ + 3SnCl4
The gold thus precipitated is adsorbed by stannic hydroxide formed by the hydrolysis of SnCl4.
SnCl4 + 4H2O → Sn(OH)4 + 4HCl
Purple of Cassius is a combination of gold with colloidal stannic hydroxide.
13. What happens when KI solution is added to an aqueous solution of copper sulphate?
When KI is added to a solution of CuSO4, a white precipitate of Cuprous iodide (Cu2I2) is produced.
When KI is added to a solution of CuSO4, a white precipitate of Cuprous iodide (Cu2I2) is produced.
CuSO4 + 2KI → CuI2 + K2SO4
(Unstable)
2CuI2 → Cu2I2 + I2
(White ppt.)
14. What is spitting of silver? How is it prevented?
Molten silver absorbs about 20 times its volume of oxygen which it again expels on cooling.
Globules of molten silver are thrown off. This is called “spitting of silver”.
This can be prevented by covering the molten metal with a layer of charcoal.
Molten silver absorbs about 20 times its volume of oxygen which it again expels on cooling.
Globules of molten silver are thrown off. This is called “spitting of silver”.
This can be prevented by covering the molten metal with a layer of charcoal.
15. What is the action of heat on copper sulphate crystals? Write the equation.
On heating CuSO4.5H2O loses its water of crystallization and decomposes at 720°C to give cupric oxide and sulphur trioxide.
On heating CuSO4.5H2O loses its water of crystallization and decomposes at 720°C to give cupric oxide and sulphur trioxide.
100°C 230°C 720°C
CuSO4 .5H2O → CuSO4 .H2O → CuSO4 → SO3↑ + CuO
(Blue) – 4H2O – H2O (White)
16. What is the reaction of CuSO4 with KCN?
A yellow precipitate of cupric cyanide is first formed with KCN and it decomposes to give cyanogen gas.
A yellow precipitate of cupric cyanide is first formed with KCN and it decomposes to give cyanogen gas.
CuSO4 + 2KCN → Cu(CN)2 + K2SO4
2Cu(CN)2 → Cu2(CN)2 + (CN)2
17. Why are Zn2+ salts colourless while Ni2+ salts are coloured?
and Ni2+ - 3d8
Outer Electronic Configurations of Zn (Z = 30) - 3d104s2 and Ni (Z = 28) - 3d84s2
Zn2+ - 3d10
↑↓
|
↑↓
|
↑↓
|
↑↓
|
↑↓
|
and Ni2+ - 3d8
↑↓
|
↑↓
|
↑↓
|
↑
|
↑
|
Zn2+ salts are coloureless because of the absence of vacant d - orbitals to which electrons can be excited.
Ni2+ salts are coloured because of the presence of 2 unpaired electrons in d - orbitals and the energy gap between two energy levels in the same d-subshell being small, can be excited from one energy level to the other by the visible light leading to green colour.
18. Give the
percentage composition and use of Nichrome
Alloy
|
% Composition
|
Uses
|
Nichrome
|
Cr = 15%,
Ni = 60%,
Fe = 25%
|
It is used in resistance wires,
for electrical heating
|
19. What is the
action of heat on heating, K2Cr2O7?
On
heating, K2Cr2O7 decomposes
to give potassium chromate with evolution of O2 gas.
4K2Cr2O7 →
4K2CrO4 + 2Cr2O3 + 3O2↑
20. Most of the transition metals and their compounds have catalytic
activity. Why
Most of the transition metals and their compounds are
used as catalyst. The catalytic activity of transition
metals is due to the following reasons.
1.
They show a variety of oxidation states and thereby can form intermediate products
with various reactants.
2.
They are also capable of forming interstitial compounds which can adsorb and
activate the reacting species
21. Why do transition elements form alloys?
Transition
metals form alloys with each other. This is because they have almost similar
size and the atoms of one metal can easily take up positions in the crystal
lattice of the other.
Eg. Alloys of Cr - Ni, Cr – Ni - Fe, Cr – V - Fe, Mn - Fe, etc.
22. How is lunar caustic prepared?
Lunar
caustic (Silver nitrate) is prepared by dissolving silver in dilute Nitric
acid.
3Ag + 4HNO3 → 3AgNO3 + 2H2O + NO↑
23. What is the action of heat on Silver nitrate?
On heating
AgNO3 decomposes in two stages
723 K
2AgNO3 → 2AgNO2 + O2
980 K
AgNO2
→ Ag + NO2
24. What is Philosopher’s wool? How is it formed?
When Zinc is
heated in air at 773 K, it burns to form a white cloud of Zinc oxide which
settles to form a wooly flock called philosopher’s wool.
773 K
2Zn + O2 → 2ZnO
25. Write two alloys of copper and their uses
Alloy
|
Uses
|
Brass
|
For making utensils, condenser tubes, wires, etc.
|
Bronze
|
For making cooking utensils, statues, coins, etc.
|
Gun metal
|
For making gun barrels, gears, castings, etc.
|
26. What is called Bordeaux mixture? Mention its use
A mixture of
Copper sulphate and Lime, commonly known as Bordeaux mixture.
It is used as
Fungicide.
27. Give the reaction of ammoniacal silver nitrate with Formic acid
Ammoniacal
silver nitrate (Tollen’s reagent) is reduced to Silver mirror by compounds like
Formic acid, Formaldehyde or Glucose
2AgNO3 + 2NH4OH → Ag2O + 2NH4NO3 + H2O
Ag2O + HCOOH → 2Ag↓ + H2O + CO2
28. How will you convert potassium chromate to
potassium dichromate? Mention the colour change involved in the
reaction.
29. A transition element has 3 unpaired electrons.
Calculate its magnetic moment.
30. What is Lunar caustic? How is it prepared?
Unit – 5 f – Block Elements
1. What are inner transition (f - block) elements?
Give two examples.
2. What is the difference in the electronic
configuration of transition and inner transition elements?
3. What are lanthanides? Give the various oxidation
states of lanthanides.
4. What are mish metals? Give their uses.
5. Account : + 3 oxidation state of lanthanides is
the most stable.
6. Account : A few 4f elements show + 2 or + 4
oxidation states in addition to the characteristic oxidation state of + 3.
7. Account : Lanthanides are grouped together.
8. Comparing La(OH)3 and Lu(OH)3, which is more basic and explain why?
9. Discuss the position of lanthanides in the
periodic table.
Unit – 6 Coordination Compounds
1. What are simple salts? Give examples.
2. What are double salts? Give examples.
3. In what way complex salt differs from double
salt?
4. What are ligands and coordination number?
5. Give one example for a monodentate ligand, a
bidentate ligand and a chelating ligand.
6. Calculate the charge on the central metal ion
present in the following complexes.
a) [Fe(NH3)4Cl2] NO3 b)
Na[B(NO3)4]
7. Name the following complexes a) [Co(NH3)5(H2O)]Cl3 b)
Na[B(NO3)4]
8. Write the formula structure of the following
a)
Tris(ethylenediamine)cobalt(III) ion b) Pentaamminesulphatocobalt(III)
chloride
9. Draw the structure of cis and trans-[Pt(NH3)2Cl2]
10. What are chelates? Give examples.ONE MARKS FIVE MARKS
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