1. SOLID STATE

1) Define (i) unit cell (ii) space lattice/Crystal lattice (iii) lattice point (iv) F-centre

(i)The smallest portion of a crystal lattice which generates the entire crystal when repeated

in different directions is called unit cell.

(ii) A regular three dimensional arrangement of lattice points in space is called space

lattice/crystal lattice.

(iii) Each point of a crystal lattice occupied by constituent particle(atom/ion/molecule) is

called lattice point.

2) What is packing efficiency?

The percentage of total space filled by the particles is called packing efficiency. Volume occupied by the spheres in the unit cell Packing efficiency = ________________________________________ Total volume of the unit cell X 100

3) Write formula to calculate the density of the unit cell.

d= ZM / a3NA where d=density of the unit cell ; M= Molar mass, a= edge length of

the cell, NA= Avogadro number.

4) Calculate the packing efficiency in

(i) Simple cubic unit cell (SC) : (ref.text book for diagram)

The no. of atoms per unit cell in simple cube is only one. Each atom is considered as

one sphere.

So volume of one atom(one sphere)=4/3 πr3.

In simple cube, edge length a=2r.

Total volume a3=(2r)

3=8r

3

Packing efficiency = (volume of one atom/volume of the unit cell)x100

Packing efficiency =[(4/3πr3)/8r

3 ]x100=52.4%

(ii) Face centered cube(FCC): The no. of atoms per unit cell in fcc structure is 4. Each atom is considered as one

sphere.

So volume of four atoms(four spheres)=4x4/3 πr3=16/3 πr

3.

The face diagonal AC=b, then b=4r

In ABC, AC2=BC

2+AB

2

b2 = a

2+a

2

b2 =2a

2

b=√2 a=4r

a=4r/√2 = 2√2 r

volume of the cubic unit cell=a3=(2√2 r)

3

Packing efficiency = (volume of four atoms/volume of the unit cell)x100

Packing efficiency =[(16/3 πr3)/(2√2 r)

3 ]x100

=74%

(iii) Body centered cube(BCC): The no. of atoms per unit cell in bcc structure is 2. Each atom is considered as one

sphere.

So volume of two atoms(two spheres)=2x4/3 πr3.

The body diagonal AF=c and face diagonal FD=b, then AF=c=4r

In ∆EFD, FD2=EF

2+ED

2

b2=a

2+a

2=2a

2

b= √2 a

Now in∆AFD, AF2=AD

2+FD

2

C2=a

2+b

2

=a

2+2a

2=3a

2

C=√3a

But c=4r

Therefore,√3a=4r

A=4r/√3

Volume of the unit cell=a3=(4r/√3)

3

Therefore Packing efficiency = (volume of two atoms/volume of the unit cell)x100

Packing efficiency = [(2x4/3 πr3)/(4r/√3)

3 ]x100

=68%

5) Give any two differences between crystalline and amorphous solid.

S.No. Crystalline solids Amorphous soild

1 They have definite geometrical

shape.

They have irregular shape.

2 They have sharp melting point. They do not have sharp melting point.

3 They are true solids They are pseudo solid or super cooled liquids.

4 They are anisotropic They are isotropic

6) Give any two differences between Schottky defect and Frenkel defect.

S.No. Schottky defect Frenkel defect.

1 It is missing of both anion and

cation from crystal lattice.

It is the dislocation of cation from its normal site

to the interstitial site.

2 Density decreases Density remains same

3 It is found in ionic solids with high

co-ordination number

It is found in ionic solids with low co-ordination

number

7) Calculate the number of particles/atoms present in

(i) primitive unit cell/simple cubic unit cell (SC)

SCC contains 8 corner particles. Each corner particle is shared to 8 unit cells.

:. The contribution of corner particle is 1/8

:. No. of particles in the unit cell of SCC lattice= 8x1/8=1

(ii) Body centered cubic lattice (BCC)

BCC contains 8 corner particles and 1 particle at the center of the body.

The contribution of corner atom to the unit cell is 1/8.

The particle present at the body center is not shared by other unit cell.

So, the contribution of body center atom to the unit cell is 1.

:. No. of particles in the unit cell of BCC = (8x1/8)+1=1+1=2

(iii) face centered cubic lattice/ccp or fcc

FCC contains 8 corner atoms and 6 atoms at the faces.

The contribution of corner atom to the unit cell is 1/8.

The contribution of atom at the face is 1/2.

:. No. of particles in the unit cell of FCC = (8x1/8)+(6x1/2)=1+3=4

8) What are (i) Diamagnetic (ii) paramagnetic (iii) ferromagnetic substances. Give

examples.

Diamagnetic: The substances which are not attracted by a magnetic field are called diamagnetic

substances. Ex: Zn2+

, H2O.

Paramagnetic: The substances which are slightly(weakly) attracted by a magnetic field are

called paramagnetic substances. Ex: O2, Cu2+

.

Ferromagnetic:The substances which are strongly attracted by a magnetic field are called

ferromagnetic substances. Ex: Fe, Co.

9) Give any two differences between n-type and p-type semi conductors.

S.No n-type semi conductors p-type semi conductors

1 They are obtained by doping

pentavalentimpurities(atoms).

They are obtained by doping trivalent

impurity atoms.

2 Conduction is due to electrons. Conduction is due to holes.

3 P, As, Sb, Bi are used for doping. B, Al, Ga, In are used for doping.

2. SOLUTIONS

1) Name a colligative property.

Elevation in Boiling point/ Depression in freezing point/Relative lowering of vapour

pressure/Osmotic pressure.

2) State Henry’s law.

At constant temperature, solubility of a gas in a liquid is directly proportional to the

pressure of the gas

3) Name one concentration term which is independent of temperature.

Molality

4) Define Molality.

Number of moles of solute per kilogram of the solvent

5) Define molarity.

Number of moles of solute dissolved in one litre of the solution

6) What are isotonic solutions?

Solutions with same osmotic pressure

7) Define osmosis.

The movement of solvent molecules from low concentration to high concentration through

semi permeable membrane.

8) Define osmotic pressure.

The pressure applied on solution side to stop osmosis

9) Define reverse osmosis.

The movement of solvent molecules from higher concentration to lower concentration

through SPM when pressure applied on solution side is greater than osmotic pressure.

10) What is Van’t Hoff’s factor?

It is the ratio of normal molar mass to abnormal molar mass

11) State Raoult’s law of relative lowering of vapour pressure.

Relative lowering of vapour pressure is equal to the mole fraction of solute.

12) Write differences between ideal & non ideal solution

S.No Ideal Non ideal

1 Obeys Raoults law at all

concentration

Do not obey Raoult’s law

2 ∆Hmix = 0 ∆Hmix ≠0

3 ∆Vmix = 0 ∆Vmix ≠0

4 Intermolecular attractive forces

between A-A,B-B & A-B are

same

A-A, B-B & A-B are not

same.

13) What are azeotropes? Give example.

Binary mixtures having same composition in liquid & vapour phase & boil at constant

temperature. Ex (i) Ethanol-water mixture (ii) Nitric acid- water mixture

14) B.P of benzene is 353.23k. When 1.8g of non-volatile solute was dissolved in 90g of

benzene, B.P is raised to 354.11k. Calculate the molar mass of solute. Kb for benzene is

2.53k kg mol-1

1000 Kb W2

M2 = ---------------

∆ Tb W1

= 1000×2.53×1.8

------------------

0.88k × 90

= 589 mol-1

3. ELECTRO CHEMISTRY

1) How molar conductivity varies with dilution?

Increases

2) What is the concentration of H+ ions in the solution used in SHE ?

1 molar

3) What is the SI unit of molar conductivity?

Sm2mol

-1 or Scm

2 mol

-1

4) Define limiting molar conductivity.

Molar conductivity at infinite dilution

5) What is primary & secondary cell? Give examples.

Primary cell: Cell which cannot be recharged & used again- Ex: Dry cell, Mercury cell

Secondary cell: Cell which can be recharged & used again. Ex: Lead storage battery &

Ni-Cd cell

6) State Faraday’s I & II Law. Write its mathematical expression.

I law: The mass of the substance deposited or liberated at the electrode during electrolysis

is directly proportional to the quantity of electricity passed through the electrolyte.

W= ZIt

II law: When same quantity of electricity is passed through different electrolyte solutions

masses of different substances deposited or liberated is directly proportional to their

equivalent masses. Mass of A Equivalent mass of A ------------- = -------------------------- Mass of B Equivalent mass of B

7) Explain construction and working, cell reaction and cell representation of Daniel

cell.

Construction:

Zn rod dipped in ZnSO4 solution ; Cu rod dipped inCuSO4 solution. Metal rods are connected externally. Two solutions are connected internally using salt bridge

Working: Anode reaction: Zn → Zn2+

+ 2e-

Cathode reaction: Cu2+

+ 2e- → Cu

------------ ----------------- Cell reaction: Zn + Cu

2+ → Zn

2+ + Cu

------------------------------ Cell representation: Zn/Zn

2+ ll Cu

2+/Cu

8) Explain construction and working, cell reaction, cell representation and

Diagram of SHE.

Construction;

Pt foil is coated with Pt black. It is immersed in 1 M HCl acid. H2 gas at 1 bar

pressure is bubbled through 1 M HCl.

Working:

H2 gas bubbled is adsorbed on Pt surface.H+ ions of HCl solution will be in

equilibrium withH2 gas at 1 bar pressure.

Cell reaction: H+(aq) + e ↔1/2 H2 (g)

Cell representation: Pt (S) / H2 (g, 1 bar) / H+(aq, 1M)

9) Write Nernst equation and explain the terms. RT [M] Ecell = E

0 cell – ---- ln -----

nF [Mn+

] E

o cell – Standard electrode potential

R – Molar gas constant

T-Temperature

F- Faraday’s constant

n- number of electrons involved

[M n+

]-Concentration of metal ions.

[M]-Concentration of metal

10) Differences between metallic and electrolytic conductors. 2M

S. No Metallic conductor Electrolytic conductor

1 Conduction due to flow of electrons Conduction due to flow of ions

2 Does not cause chemical

decomposition

causes chemical decomposition

3 Conductance decreases with increase

in temperature

Conductance increases with increase

in temperature

11) State Kohlrausch’s law and write its mathematical expression. Mention two

applications of it.

Limiting molar conductivity of an electrolyte can be represented as the sum of the

limiting molar conductivities of cation and anion of the elctrolyte.

For AxBy, Λom= x λ

ocation + y λ

oanion

Application:

1. Degree of dissociation(α) and dissociation constant(K) of weak electrolyte can be

calculated.

2. Λom of weak electrolyte can be calculated.

12) What is corrosion? Mention two methods to prevent it.

Loss of metal due to the formation of its oxides and sulphides due to the action of

constituents of environment.

Methods to prevent corrosion:

1.By coating surface with oil, grease, paint or varnish.

2.By giving a coating with more reactive metal(Zn coating-galvanization, Sn coating-

tinning)

4. CHEMICAL KINETICS

1) Write differences between order and molecularity of a reaction.

S.No. Order Molecularity

1 It is the sum of the power of

reacting species involved in the rate

equation

It is the no. of species involved in

simultaneous collision in an elementary

reaction

2 Can be zero or fraction Can not be zero or fraction. Always whole

number

3 Experimental value Theoretical value

2) Derive an expression for rate constant of a first order reaction.

Consider a first order reaction R→ P

Rate= k[R]’ = −d[R]/dt

- d[R]/dt = k[R]

d[R]/[R] = −kdt

On integration,

∫d[R]/[R] = −k∫ dt

ln[R] = -kt +I ----------(1)

When t=0, [R] = [R]o. Substituting in (1)

ln[R]o = I

Substituting in (1) for I

ln[R] = -kt + ln[R]o

kt = ln[R]o - ln[R]

k = 1/t ln[R]o /[R] (where ln=2.303 log)

k = 2.303/t log [R]o /[R]

3) Derive an expression for rate constant of zero order reaction.

Consider a zero order reaction R → P

Rate = -d[R]/dt

k[R]0= k

d[R] = -kdt

on integration

∫d[R]= −k∫ dt

[R]= -kt + I --------1

When t=0, [R]= [R]0 Substituting in equation 1

[R]0 = I Sustituting value of I in 1

[R] = -kt + [R]0

[R]0 – [R] = kt

k= [R]0-[R] /t

4) Derive an expression half life for first order reaction/Show that t1/2 of a first order

reaction is independent of initial concentration for the first order reaction.

K= 2.303/t log [R]o/[R] ----1

When t=0, [R]= [R]o/2

Substituting in 1

k= 2.303/t1/2 log [Ro]/[Ro]/2

t1/2 = 2.303/k log 2 ( log 2=0.3010)

t1/2 = 2.303 x 0.3010/k = 0.693/k

t1/2 = 0.693/k

5) Derive an expression for half life of zero order reaction/ Show that t1/2 of a zero

order reaction is directly proportional to initial concentration

For a zero order reaction k= [R]0 – [R] /t --------1

When t=t1/2, [R]= [R0]/2

Substituting in 1

K= [R]0 – [R0]/2

_______________

t ½

t1/2 = [R]0 /2k

6) What is zero order reaction? Give example.

Reaction which is independent of initial concentration of reactant

Pt

Eg: 2NH3(g) ↔N2(g) + 3H2(g)

7) What is pseudo first order reaction? Give an example.

The one where a higher order reaction is converted to first order by taking the

concentration of all reactants except one in large excess.

Ex: (i) Acid hydrolysis of ethyl acetate.

H+

CH3COOC2H5 + H2O → CH3COOH + C2H5OH or

(ii)Inversion of cane sugar

H+

C12H22O11 + H2O → C6H12O6 + C6H12O6

8) Write Arrhenius equation & explain terms in it

K = A e –Ea/RT

Where A- Arrhenius factor ,K- Rate constant of the reaction, Ea- Energy of

activation, T- Temperature

9) What are the two criteria for effective collision according to collision theory?

1. Proper orientation of reactant molecules

2. Energy of activation of reactant molecules.

10) Rate constant of first order reaction is 6.93x10-3

min-1

.Calculate its half life period.

t1/2 = 0.693/k

= 0.693/6.93×10-3

= 693/6.93

= 100min

5. SURFACE CHEMISTRY

1) What is collision frequency?

Number of collisions per second per unit volume of reaction mixture.

2) What is emulsion? Give an example.

Emulsion is a colloidal system in which both dispersed phase and dispersed

medium are liquid. Ex: Milk

3) What is homogeneous and heterogeneous catalysis? Explain with example.

S. No. Homogeneous catalysis Heterogeneous catalysis

1 Reaction in which the reactants and

catalyst are in the same phase

Reaction in which the reactants and

catalyst are in the different phases.

2 Ex: Acid hydrolysis of methyl acetate

Ex: Manufacture of ammonia by

Haber’s process

4) What is peptization?

The process of conversion of freshly prepared precipitate into a colloidal solution by

adding an electrolyte containing common ion is called peptization.

5) Explain Bredig’s electric arc method for the preparation of gold. Two gold rods are dipped in ice cold water containing little KOH to stabilize gold

sol. The vessel is kept in freezing mixture. An electric arc is struck between two

gold rods. Heat produced by the spark causes a small amount of gold to vaporize.

The vapors of gold cooled suddenly to form colloidal gold.

6) Give any two differences between adsorption and absorption.

S.No adsorption absorption

1 It is a surface phenomenon It is a bulk phenomenon

2 Molecules are concentrated only on

the surface.

Molecules are concentrated in the bulk

as well as surface.

3 The process is fast at the beginning

and gradually becomes slower

It takes place at uniform rate.

7) Give any four differences between physisorption and chemisorption.

S.No physisorption chemisorption

1 It involves weak van der Waal’s

forces of attraction

It involves strong chemical

bond forces of attraction

2 Reversible Irreversible

3 Not specific in nature Highly specific in nature

4 It forms multimolecular layer It forms unimolecular layer

8) What is Tyndall effect?

The scattering of light by the colloidal particles in a colloidal solution is

called tyndall effect.Ex.Bluecolour of the sky, sea etc.

9) What is Brownian movement?

The zig-zag movement of colloidal particles in a colloidal solution is called Brownian

movement.

10) What is electrophoresis?

The movement of colloidal particles towards cathode or anode under an applied electric

potential is called electrophoresis.

11) State Hardy-Schulze rule.

The larger the valency of the coagulating ion, the greater is its precipitation action.

Eg. 1) Al3+

>Ba2+

>Na+ 2)PO4

3->SO4

2->Cl

-

12) Give any 2 applications of colloids.

1. It is used in the electrical precipitation of smoke or in controlling air pollution.

2. It is used in the purification of drinking water.

13) Give any four differences between lyophillic and lyophobic.

S.

No.

Lyophillic lyophobic

1 They have more affinity for the

medium

They have little or less affinity for the

medium

2 Reversible irrreversible

3 More stable Less stable

4 Particles are solvated Particles are not solvated

14) What is dialysis?

It is a process used to remove true solution impurity or electrolyte impurity from a

colloidal solution using parchment paper membrane.

15) What is meant by protective action of colloids?

Lyophobic colloids are less stable than lyophillic colloids so the stability of lyophobic colloid can

be increased by adding little lyophillic colloid. The added lyophillic colloid is called protective

colloid and the process is called protective action of colloids.

6. GENERAL PRINCIPLES AND PROCESS OF ISOLATION OF ELEMENTS

1) Give the composition of ‘copper matte’ .

Cu2S + FeS

2) What is the role of limestone in the extraction of iron from the concentrated

haematite ore?

Flux or Removes silica gangue as slag.

3) Which type of ore is concentrated by froth floatation?

Sulphide ores

4) Name the depressant used to separate two sulphide ores containing ZnS &

PbS.

NaCN ( Sodium cyanide)

5) Name the method used to refine semi conducting metals.

Zone refining process

6) Mention the chief ore of aluminium.

Bauxite or Al2O3.2H2O

7) Name the reducing agent used in the separation of gold from its complex.

Zinc dust.

8) Describe the three steps involved in the leaching of bauxite to pure

alumina(equations not expected).

i) Bauxite is concentrated by NaOH, at 473-573K and 35 bar pressure.

ii) Al2O3 is leached as sodium aluminate. Aluminate solution is neutralized by

passing CO2

iii) Hydrated alumina is precipitated by seeding. Hydrated alumina is filtered

and dried to get pure Al2O3.

9) Explain with equations Van-Arkel method of refining of Zirconium.

The crude metal is heated in an evacuated vessel with iodine .The

metal iodide being more covalent ,volatilizes.

Zr + 2I2 ZrI4

The metal iodide is decomposed on a tungsten filament, electrically

heated to about 1800K.The pure metal is thus deposited on the filament.

ZrI4 Zr + 2I2

10) a) How is zinc extracted from zinc oxide?

Zinc oxide is reduced to zinc using coke.

Coke/1673K

ZnO + C Zn + CO↑

The metal is distilled off and collected by rapid cooling.

b) What is the role of cryolite in the extraction of Al?

Lowers the melting point of the mix and increases the conductivity.

11) Write the reactions taking place in slag formation zone.

Reactions at slag formation zone:

∆

CaCO3(s) CaO(s) + CO2↑

CaO(s) + SiO2 CaSiO3

7. THE P-BLOCK ELEMENTS

1) Noble gases have very low boiling point. Why?

Due to weak dispersion forces between their atoms

2) What is the product formed when xenon reacts with PtF6?

Xenonhexafluoroplatinate(IV) or Xe+ [PtF6]

-

3) Mention the noble gas element used in cancer therapy

Radon

4) Which is the most abundant noble gas?

Argon

5) Complete the following equations:

1. 2F2 + 2H2O → 4HF + O2

2. H2S + Cl2 → 2HCl + S

3. 8NH3 (excess) + 3Cl2 → 6NH4Cl + N2

6) In the manufacture of ammonia by Haber’s process.

1.Write the equation for the formation of ammonia

Fe/Mo

N2 (g) + 3H2(g) → 2NH3(g) : ∆H= -ve.

723K/2-3atm

2.Mention the catalyst used

Iron oxide

3.What is the temperature maintained in the process?

723K

7) Name the gas liberated when concentrated HCl is heated with MnO2. Give the

equation for the reaction. Name the reagent used to obtain bleaching powder

from chlorine.

Chlorine. MnO2 + 4HCl → MnCl2 + 2H2O + Cl2

Dry slaked lime.

8) Write the chemical reactions in the manufacture of concentrated sulphuric acid

by Contact process.

1. Formation of SO2

S + O2 →SO2 or 4FeS2 + 11O2 →2Fe2O3 + 8SO2

2. Conversion of SO2 to SO3

V2O5/Pt

2SO2(g) + O2 2SO3(g) : ∆H= -ve

2-3 atm

3. Absorption of SO3 in 98% conc H2SO4.

SO3(g) + H2SO4→ H2S2O7

Oleum

H2S2O7 +H2O→2H2SO4

9) i)Write the structure of S8 molecule.

ii) What is aquaregia?

Mixture of conc. HNO3 and conc. HCl in the ratio 1:3 by volume.

iii) Explain the action of Cl2 on slaked lime.

Chlorine reacts with slaked lime give bleaching powder.

2Ca(OH)2 +2Cl2 → Ca(OCl)2 +CaCl2 + 2H2O.

10) Explain the charring action of conc. H2SO4 on carbohydrate. Give the equation.

Conc. H2SO4 is a strong dehydrating agent, it removes water from carbohydrates to form

carbon.

H2SO4

C12H22O11 12C+ 11H2O

11) Which allotropic form of phosphorous has tetrahedral P4 molecules? How is

phosphine prepared in the laboratory? Give the equation.

White phosphorous

By heating white phosphorous with conc. NaOH in inert atmosphere of CO2.

P4 + 3NaOH +3H2O PH3 +3NaH2PO2

12) Complete the following equations: MnO2/ heat

i) 2KClO3 ? Ans. 2KCl + 3O2

ii) SO2(g) + Cl2(g) ? Ans. SO2Cl2

iii) SO3 + conc. H2SO4 ? Ans. H2S2O7

13) Give two reasons for anomalous behavior of fluorine. Give an example for one

oxoacid of chlorine.

i)Small size

ii) Highest electronegativity.

iii)Low F-F bond dissociation enthalpy.

iv)Non-availability of d-orbitals in valence shell.(any two of the above)

HClO,HClO2,HClO3,HClO4.(any one)

14) Describe with equations the manufacture of nitric acid by Ostwald’s process.

This method is based upon catalytic oxidation of NH3 by atmospheric oxygen. Pt /Rh guaze catalyst 4NH3(g) +5O2(g) 4NO(g) + 6H2O(g) 500K, 9 bar

Nitric oxide thus formed combines with oxygen giving NO2

2NO(g) + O2(g) 2NO2(g)

Nitrogen dioxide formed ,dissolves in water to give HNO3

3NO2(g) + H2O(l) 2HNO3(aq) + NO(g)

NO thus formed is recycled and the aqueous HNO3 can be concentrated by distillation.

15) a)Complete the following equations:

i) H2S + Cl2 2HCl + S↓

ii) 2NaOH + Cl2 NaCl + NaOCl + H2O (Cold /dil.)

iii) 6NaOH + 3Cl2 5NaCl + NaClO3 + 3H2O (hot&conc.)

b) Give reason:`BrF5 is more reactive than Br2.

Br-F bond is weaker than Br-Br bond.

8. THE d-and f-BLOCK ELEMENTS 1) Write the general electronic configuration for d-block elements.

(n-1)d1-10

ns1-2

2) Name the element which exhibits maximum oxidation state in 3d series.

Manganese or Mn

3) Give the composition of chromite ore.

FeO.Cr2O3

4) Write the general electronic configuration for f-block elements

(n-2)f1-14

(n-1)d0-1

ns2

5) Name the radioactive element in Lanthanoid series

Promethium

6) Name the element which exhibits +4 oxidation state among lanthanoid series

Cerium

7) Name a transition element which does not exhibit variable oxidation state.

Scandium

8) What are interstitial compounds? Give an example.

Interstitial compounds are those which are formed when small atoms such as H, C, B and N

occupy or are trapped inside the crystal lattices of metals.

Example: TiC, Fe3H, Fe0.94O etc.,

9) The transition metals generally form coloured compounds. Explain.

Colour is due to the presence of incomplete d-subshell. When the ligands approach the transition

metal ions, they split into 2 sets, one consisting of lower energy(t2g) and the other consisting of

higher energy orbitals(eg). Since energy gap among two energy levels is small, the electrons get

excited from t2g to eg by absorbing visible light. The colour observed is complementary to the

colour absorbed.

10) Explain the catalytic property of transition metals and their compounds.

The catalytic property of d-block elements is due to

1) The presence of partially filled d-orbitals

2) The tendency to form reaction intermediates with reactants.

3) The tendency to exhibit variable oxidation states

11) The transition metals and their ions show strong tendency to form complexes. Give

reason.

The transition metals and their ions show strong tendency to form complexes due to

1) Small size

2) High ionic charge

3) Availability of vacant d-orbitals of suitable energy.

12) What are alloys? Give an example.

Alloys are homogeneous solid solutions of two or more metals obtained by melting the

components and then cooling the melt.

Example: Brass, Bronze, Alnico etc.,

13) Explain the manufacture of potassium dichromate from chromite ore.

Step1: Preparation of sodium chromate: The ore is finely powdered, mixed with sodium carbonate,

quick lime and then roasted.

4FeOCr2O3 + 8Na2CO3 +7O2 8Na2CrO4 + 2Fe2O3 + 8CO2

Step2: Conversion of sodium chromate into Sodium dichromate

2Na2CrO4 +H2SO4 Na2Cr2O7 + Na2SO4 + H2O

Step3: Conversion of sodium dichromate into potassium dichromate

Na2Cr2O7 + 2KCl K2Cr2O7 + 2NaCl

14) Explain the manufacture of potassium permanganate.

MnO2(pyrolusite) is fused with KOH in the presence of oxidizing agent like KNO3, potassium

manganate is formed.

2MnO2 + 4KOH + O2 2K2MnO4 + 2H2O

The potassium manganate undergoes disproportionation in acidic or neutral medium to give

permanganate.

3MnO42-

+ 4H+ 2MnO4

- + MnO2 + 2H2O

The purple solution so obtained is concentrated to get dark purple crystals of KMnO4.

15) What is Lanthanoid contraction? What are its consequences?

The regular decrease in the atomic and ionic radii of lanthanoids with increasing atomic no. is

known as lanthanoid contraction.

Consequences of lanthanoid contraction

a) Difficulty in separation of lanthanoids due to very small difference in ionic radii among

them.

b) Similarity in size of elements belonging to the same group of 2nd

and 3rd

transition

elements. Example: Zr & Hf

16) Write any four differences between lanthanoids and actinoids

Lanthanoids Actinoids

1 Binding energies of 4f electrons are

higher.

Binding energies of 5f electrons are lower.

2. Besides +3 OS, they show +2 & +4

OS only in few cases.

Besides +3 OS, they show higher OS of +4, +5,

+6, +7 also

3 4f electrons have greater shielding

effect

5f electrons have poor shielding effect

4 They have less tendency towards

complex formation

They have greater tendency towards complex

formation

5 Except promethium, they are non-

radioactive.

All of them are radioactive.

6 Lanthanoid compounds are less

basic

Actinoid compounds are more basic

7 They do not form oxocations They form oxocations. Ex: UO22+

, PuO2+

17) Write any four similarities between lanthanoids and actinoids

1) Both show mainly an oxidation state of +3

2) Both are electropositive and are very reactive.

3) Both exhibit magnetic and spectral properties.

4) Ionic radius and atomic radius of the elements in both the series decrease with the

increase in atomic no. (lanthanoid and actinoid contraction)

5) The electronegativity of all the elements in both the series is low and are highly reactive.

9. COORDINATION COMPOUNDS

1) Define coordination number

Coordination no is defined as the number of coordinate bonds formed with the central metal

atom/ion by the ligands.

2) Give an example for a polydentate ligand.

EDTA

3) Give an example for a cationic complex.

[Cu(NH3)4]SO4

4) Give an example for an anionic complex.

K4[Fe(CN)6]

5) Give an example for a neutral monodentate ligand.

H2O or NH3

6) Give an example for a bidentate ligand.

Oxalato or ethane-1,2-diammine.

7) Write the IUPAC names for the following complexes

1) K3[Fe(C2O4)3] : Potassium trioxalatoferrate(III)

2) [Cr(H2O)4Cl2]Cl : tetraaquadichloridochromium(III)chloride

3) K3[Fe(CN)6]: Potassium haxacyanidoferrate(III)

4) [Cu(NH3)4]SO4 : tetraamminecopper(II) sulphate

5) [Ni(CO)4] : tetracarbonylnickel(0)

8) What is crystal field splitting energy(CFSE)?

The difference of energy between two sets of d-orbitals (t2g &eg) after splitting is called

crystal field splitting energy.

9) What is spectrochemical series?

The arrangement of ligands in order of their crystal field splitting energy values

or The arrangement of the ligands in the increasing order of the field strength is called

spectrochemical series.

10) What are ambidentate ligands? Give an example.

The ligands which contain more than one donor atoms but ligate through only one donor

atom are called ambidentate ligands.

Examples: NO2-, CN

-, SCN

- etc.,

11) Define ionization isomerism? Give an example.

Two or more complexes having same molecular formula but differs in the mode of ionization to

give different ions in solution.

Example: [Pt(NH3)4(OH)2]SO4 and [Pt(NH3)4(SO4)](OH)2

[Pt(NH3)4Cl2]Br2 and Pt(NH3)4Br2]Cl2

12) What is linkage isomerism? Give an example.

Two or more complexes having same molecular formula but it differs in the mode of attachment of

the ligating atom of an ambidentate ligand.

Example: [Co(NH3)5(ONO)]2+

and [Co(NH3)5(NO2)]2+

13) What is geometrical isomerism? Give an example.

Two or more complexes having same molecular formula and structural formula but differs in the

arrangement of the ligands either towards same side or opposite side around the central metal.

atom/ion. Cl NH3 2+ Cl NH3 2+

Ex:

Pt Pt

Cl NH3 NH3 Cl

14) What are homoleptic complexes? Give an example.

Homoleptic complexes are those in which the central metal atom/ion is bonded to only one type of

ligands.

Example : [Co(NH3)6]3+

, [PtCl4]2-

etc.,

15) What are heteroleptic complexes? Give an example.

Heteroleptic complexes are those in which the central metal atom/ion is bonded to more than one

type of ligands.

Example: [Co(NH3)4Cl2]+, [Cr(SO4)(NH3)5]

+ etc.,

16) Write any two limitations of Valence bond theory

a)VBT doesn’t offer any explanation for the colour and the spectral properties of the coordination

compounds.

b) It fails to explain exact magnetic moment value satisfactorily.

c) It doesn’t distinguish between weak and strong ligands.

17) What are metal carbonyls? Give an example.

Metal carbonyl are the organometallic compounds in which carbon monoxide (CO) acts as the

ligand.

Example: [Ni(CO)4], [Fe(CO)4], [Mo(CO)6] etc.,

18) On the basis of Valence bond theory, explain hybridization & predict the geometry

and magnetic property of hexaamminecobalt(III) ion, [Co(NH3)6]3+

Co atom (Z=27):

in ground state

Co3+

ion :

When strong ligand NH3 approaches the cental metal ion Co3+

, the unpaired electron gets paired

up and six empty d2sp

3 hybrid orbitals are obtained.

↑↓ ↑↓ ↑↓ xx Xx

xx

xx xx xx

Six d2sp3 hybrid orbitals

Each NH3 molecule donates a pair of electron to all the six d2sp

3 hybrid orbitals.

The geometry is octahedral and magnetic property is diamagnetic due to the absence of unpaired

electrons.

19) Using VBT, explain the hybridization, magnetic property and geometry of

hexafluoridocobaltate(III) ion, [CoF6]3-

3d

4s

4p

4d

↑↓ ↑↓ ↑ ↑ ↑

↑↓

↑↓ ↑ ↑ ↑ ↑

Co atom (Z=27):

in ground state

Co3+

ion :

↑↓ ↑ ↑ ↑ ↑

six sp3d2 hybrid orbitals

Since F- is a weak ligand, pairing of electron doesn’t take place. Six electron pairs are donated by

six F- ion to each empty sp

3d

2 hybrid orbital.

↑↓ ↑ ↑ ↑ ↑

xx

xx xx xx

xx xx

six sp3d2 hybrid orbitals

Geometry: Octahedral

Magnetic property: Highly paramagnetic due to the presence of four unpaired electrons.

20) Explain the hybridization of the complex ion [Ni(CN)4]2-

(tetracyanidonickelate(II)

ion) on the basis of VBT and predict the geometry and its magnetic property.

Ni atom(Z=28) in ground state:

Ni2+

ion

When CN- a strong ligand approaches the cental metal ion Ni

2+, pairing up of unpaired electron

takes place and dsp2 hybridisation takes place.

dsp2 hybrid orbitals

of Ni2+

dsp2 hybrid orbitals

Formation of [Ni(CN)4]2-

4 e- pairs donated by 4 CN- ion

3d

4s

4p

4d

↑↓ ↑↓ ↑ ↑ ↑

↑↓

↑↓ ↑ ↑ ↑ ↑

3d

4s

4p

4d

↑↓ ↑↓ ↑↓ ↑ ↑

↑↓

3d

4s

4p

4d

↑↓ ↑↓ ↑↓ ↑ ↑

↑↓ ↑↓ ↑↓ ↑↓

↑↓ ↑↓ ↑↓ ↑↓ xx

xx

xx xx

Geometry : Square planar

Magnetic property: Diamagnetic

21) Predict the hybridization, magnetic property and geometry of the complex ion

[NiCl4]2-

on the basis of VBT.

Ni atom(Z=28) in ground state:

Ni2+

ion

When Cl- a weak ligand approaches the central metal ion Ni

2+, pairing up of unpaired electron does

not takes place and sp3 hybridisation take place.

↑↓ ↑↓ ↑↓ ↑ ↑

sp3 hybrid orbitals

Formation of [NiCl4]2-

↑↓ ↑↓ ↑↓ ↑ ↑

xx

xx xx xx

sp3 hybrid orbitals

Geometry : Tetrahedral

Magnetic property: Paramagnetic due to the presence of unpaired electron.

22) Write the postulates of Werner’s theory of coordination compounds.

i)The central metal atom/ion in a complex contains 2 types of valency i.e., primary and secondary

valency.

ii)Primary valency is the number of charge present on the central metal atom/ion in a complex.

Secondary valency represents coordination number.

iii)Primary valency is satisfied by the –ve ions which may be ligand or counter ion where

secondary valency is satisfied by only ligands.

iv)Primary valency is non directional whereas secondary valency is directional in nature.

10. HALOALKANES AND HALOARENES

3d

4s

4p

4d

↑↓ ↑↓ ↑↓ ↑ ↑

↑↓

↑↓ ↑↓ ↑↓ ↑ ↑

1) Give an example for vinylic, allylic and benzylic halide.

vinylic halide: CH2=CH-Cl allylic halide: CH2=CH-CH2-Cl

benzylic halide:C6H5CH2Cl

2) What is racemization?

The process of conversion of enantiomers into a racemic mixture is called racemization.

3) What are enantiomers?

Optically active isomers which are non-super imposable on their mirror images are called

enantiomers.

4) Give one use for each of the following.

(i) Chloroform –Anaesthetics , solvent.

(ii) Freons -aerosol propellants, refrigeration and air conditioning purposes

(iii) DDT- insecticide

(iv) CCl4-aerosol propellants, refrigerants

(v) CHI3-antiseptic

5) Discuss the mechanism of SN1

I Step: (Slow step): Tertiary butyl bromide ionizes slowly to give tertiary butyl carbocation and

bromide ion.

C+

CH3

CH3CH3

+ Br-

C

CH3

CH3

CH3 Br

II Step: (Fast step): the nucleophile OH- from aq.NaOH attacks planar carbocation on either side

to give tertiary butyl alcohol, a racemic mixture.

C+

CH3

CH3CH3

+ OH-

C

CH3

CH3

CH3 OH

6) Discuss the mechanism of SN2

Primary alkyl halides react with aq.NaOH to give alkyl alcohol. The nucleophile OH- attacks

electron deficient carbon atom from the back side to form a transition state. It is unstable. In the

transition state a partial C-OH bond is formed and a C-Cl bond is broken. The product methyl

alcohol obtained has inversion in configuration.

OH-

+H

C

H

Cl

H

H

C

H

H

Cl

H

C

H

OH

H

HO----- ------- + Cl-

methyl chloridetransition state

methyl alcohol with inversion in configuration

7) Explain Finkelstein’s reaction.

Chloroalkane or bromoalkane on heating with sodium iodide in dry acetone gives alkyl iodide.

Dry acetone

C2H5-Cl +NaI -------------------> C2H5-I + NaCl

8) Explain Swart’s reaction.

Chloroalkane or bromoalkane on heating with metallic fluoride like AgF gives alkyl fluoride.

C2H5-Cl +AgF ---------> C2H5-F + AgBr

9) Explain β-elimination/dehydrohalogenation(Zaitsev’s rule) reactions of alkyl

halide.

Zaitsev’s rule states that “ during dehydrohalogenation reaction of an unsymmetrical alkyl halide,

the more substituted alkene is the most preferred product.“

CH3-CH2-CH2-CHBr-CH3 + KOH --->CH3-CH2-CH=CH-CH3+CH3-CH2-CH2-CH=CH2 +

KBr + H2O

2-Bromo pentane pent-2-ene(major) pent-1-ene(minor)

10) Explain the following reactions.

1) Wurtz reaction: When an alkyl halide is treated with metallic sodium in dry ether,

higher alkane is formed.CH3-Cl +2Na + Cl-CH3 ------> CH3-CH3+ 2NaCl

Methyl chloride ethane

2) Fittig reaction: When an aryl halide is treated with metallic sodium in dry ether,

biphenyl is formed. C6H5-Cl +2Na + Cl-C6H5 ------> C6H5-C6H5 + 2NaCl

chlorobenzene biphenyl

3) Wurtz-Fittig reaction: When an alkyl halide is coupled with an aryl halide with

metallic sodium in dry etheralkylarenes are formed.

CH3-Cl +2Na + Cl-C6H5---------> CH3-C6H5+ 2NaCl

11) Why is chloroform stored on dark coloured bottle?

Ans: because chloroform is slowly oxidized by air in the presence of light to a highly poisonous

gas, carbonyl chloride, also known as phosgene. 2CHCl3 + O2 --> 2COCl2 + 2HCl

11.ALCOHOLS, PHENOLS AND ETHERS

1) Complete the following equation .

OH

Zn+ ZnO

heat

2) What is Lucas reagent? Between primary & tertiary alcohols, which one of these

will react faster with Lucas reagent?

1. Lucas reagent is a mixture of Anhyd. ZnCl2 + Conc HCl

2. Tertiary alcohol reacts faster

3) A Carboxylic acid is treated with alcohol in the presence of Conc H2SO4. Name

the reaction . Give its general equation/ Explain esterification reaction with an

example.

Esterification .

Con H2SO4 RCOOH + HOR

I -----------------> RCOOR

I

-H2O Con H2SO4

Ex: CH3COOH + HOC2H5 --------------> CH3COOC2H5 Acetic acid ethanol -H2O ethyl acetate

4) Name the organic compound formed when vapours of tertiary butyl alcohol is

passed over heated copper at 573 K. Write the equation.

C OH

CH3

CH3

CH3

-H2O

CH3 C CH2

CH3

Cu/heat

2-Methyl-1-propene

5) How is Anisole converted into 2-Methoxy toluene & 4-Methoxy toluene? Give the

equation.

(Friedel crafts reaction) .

Anisole reacts with methyl chloride in the presence of Anhy.AlCl3 catalyst to give a

mixture of 2- & 4- methoxy toluenes.

OCH3

+2 2CH3ClAnhyd.AlCl3

-2HCl

OCH3

CH3

+

OCH3

CH3anisole2 Methoxy toluene

4 Methoxy toluene

6) How do you convert propene into propan-2-ol?

Alkenes when subjected to acid hydrolysis by heating with water in the presence of

dil.H2SO4 give alcohols.

CH3 CH CH2 + H2O CH3 CH CH3

OH

dil.H2SO4

propenepropan-2-ol

heat

7) Name the major product formed when sodium phenoxide is heated with CO2 at

400 K(140oC) and at 4-7 atm. pressure. What is the name of the reaction./ Explain

Kolbe’s reaction.

Sodium salicylate is formed which on acidification gives salicylic acid.

ONa

+ CO2

140oC

6 to 7 atm

OH

COONa

HCl

OH

COOH

8) Explain Williamson’s ether synthesis with an example.

When an alkyl haide is heated with sodium alkoxide, an ether is obtained.

R-O-Na + X-R’ → R-O-R’ + NaX . R/R’ -CH3, -C2H5 X-Cl, Br

9) How is phenol manufactured from cumene?

Air is bubbled through cumene at 130oC to form cumene hydroperoxide which on heating

with dil.H2SO4 at 100oC gives phenol and acetone.

CH

CH3

CH3

+ O2

130oC COOH

CH3

CH3

dil.H2SO4

100oC

OH

+ CH3COCH 3

cumene or isopropyl benzenecumene hydroperoxide Phenol

10) Write equation for

(i) Reimer Tiemann reaction.

ONa

+ CHCl3-HCl

ONa

CHCl22NaOH

-2NaCl

ONa

CHO

sodium phenate

HCl

-NaCl

OH

CHO

salicylaldehyde

(ii) Dehydration of primary alcohols

Primary alcohol when heated with con.H2SO4, dehydration takes place to form an

alkene.

CH3-CH2-OH -------------> CH2=CH2 Ethanol con.H2SO4 ethene

11) Complete the following reactions

CH3 C

CH3

CH3

O CH3 + HI +

(i)

+CH3 C

CH3

CH3

I CH3OHAns.

tert.alkyl halide

COOH

OH

+ (CH 3CO) 2O H+

---------- + --------

(ii)

COOH

OCOCH3

+ CH3COOHAns:

acetyl salicylic ac id

12. ALDEHYDES, KETONES AND CARBOXYLIC ACIDS

1) Give the name of the product X (Gattermann Koch reaction)

CO, HCl

Anhyd.AlCl 3 / CuClX

Ans.

CHO

Benzaldehyde

2) Name the product obtained when acetaldehyde reacts with hydroxylamine.

3) CH3 CH O NH2 OH+ CH3 CH N OH

acetaldoxime

COCH3 COONa

+ XNaOH

I2

Give the IUPAC name of X .

X= CHI3 Triiodomethane

4)

+ CH3COClAnhyd.AlCl3 X + HCl

Write the structure of X in the above.

COCH3

5) COCl

H2

Pd/BaSO4X

What is X?

CHO

6) What is the oxidizing agent used in Etards reaction?

Chromyl chloride vapours

7) Give reason: Electron withdrawing group increases the acidic strength of

Carboxylic acid.

Electron withdrawing group stabilizes the carboxylate anion.

8) Complete the following reaction

COOC2H5

H3O+

+ C2H5OH----------

COOH

Ans:

9) Explain Aldol condensation by taking acetaldehyde .

Acetaldehyde reacts with dil.NaOH to form β-hydroxy aldehyde. The aldol readily looses

water to form α,β-unsaturated aldehydes .

CH3 C

O

H

+ HCH2 C

CH3

Odil.NaOH

CH3 C

OH

CH2

H

CO CH3 -H2O

CH3 CH CH CO CH3

pent-3-en-2-one

10) Explain with equation , the addition reaction of (a) aldehyde (b) ketone with (i)

HCN (ii) NaHSO3

R C O

H

+ HCN R C OH

H

CN

cyanohydrinR=( -CH3)

a) i)

R C O

R

+ HCN R C OH

R

CN

cyanohydrinR=( -CH3)

b) i)

R C O

H

+ NaHSO3R C OH

H

SO3Na

bisulphite addition productR=( -CH3)

a) i i)

R C O

R

+ NaHSO3R C OH

R

SO3Na

bisulphite addition productR=( -CH3)

b) i i)

11) How is propanenitrile converted into propanal? Write the equation.

12) CH3 CH2 C N + 2[H] CH3 CH2 CH NH

SnCl2/HCl

Ether

H2OCH3 CH2 CHO

CH3

CCH3

ONH2

-NH2

H2OP Q + N2 .

heat

NaOH/glycol

What are P and Q. Name the reaction/Explain Wolf Kishner reduction with an

example.

CH3

CCH3

O + NH2 NH2-H2O

CH3

CCH3

N NH2

NaOH/glycolCH3 CH2

CH3 + N2

acetone hydrazine propaneheat

13) Explain Clemmensen’s reduction with an example ./ What happens when

aldehydes & ketones are treated with Zn-Hg & Conc HCl. Name the reaction.

Aldehydes & ketones when treated with Zn-Hg and con.HCl, >C=O group is reduced

to >CH2.

CH3 CHO + 4[H] Zn

-Hg/con.HCl

CH3 CH3 + H2O

acetaldehyde ethane

14) Mention 2- tests to distinguish aldehydes from ketones.

Silver mirror test and Fehlings solution test.

15) Mention any two uses of carboxylic acid.

(i) acetic acid is used as vinegar in food industry.

(ii) it is used as solvent.

16) α- hydrogen atom of aldehydes & ketones are acidic. Why?

Due to strong electron with drawing nature of C=O group & resonance stabilization of

conjugate base.

17) Complete the following equations

(i) R COONaNaOH/CaO

heat------------ + Na2CO3

(ii) CH3 COOH ------------ + HCl ( HVZ reaction)(i) Cl 2/Red P

(ii) H2O

Ans: (i) RH (ii) CH2(Cl)- COOH (chloroacetic acid)

18) Explain Cannizzaro’s reaction with an example.

Aldehydes having no α-hydrogen atom (HCHO,C6H5CHO)when treated with strong

solution of NaOH/KOH undergo self oxidation & reduction to give salt of a carboxylic

acid & an alcohol.

2C6H5CHO + NaOH C6H5COONa + C 6H5CH2OHbenzaldehyde Sodium benzoate

Benzyl alcohol 19. Explain HVZ (Hell- Volhard- Zelinskii )reaction with example.

CH3CH2COOHX2/Red P

CH3 CH

X

COOH

monohalo propanoic acid

13. AMINES

1) Explain diazotization reaction of aniline(aniline to benzene diazonium

chloride)

Aromatic primary amines(aniline) react with HNO2 (NaNO2 + HCl) at 0-5oC to form

diazonium salt.

NH2

+ NaNO2 + 2HCl

N2Cl

+ NaCl + 2H2O

0 - 5 oC

aniline

benzene diazonium chloride

2) What is Hinsberg’s reagent? How is it used to distinguish 10, 2

0 & 3

0 amine?

/Test to distinguish between 10,2

0 & 3

0 amines

Hinsberg’s reagent is benzene sulphonyl chloride ,C6H5SO2Cl.

10 amines react with Hinsberg’s reagent to give N-alkyl benzene sulphonamides which

dissolve in excess of NaOH.

20 Amines react with Hinsberg’s reagent to give N,N-dialkyl benzene sulphonamides

which are insoluble in excess of NaOH.

30 Amines do not react with benzene sulphonyl chloride.

3) Complete the following reactions

R C NH2/Ni

(i) -----------

R CH2 NH2Ans. (amine)

CH3NH2 + CHCl3 + 3KOH -------- + 3KCl + 3H2O(alc)

Ans. CH3NC

(ii)

(isocyanide)

(carbylamine reaction)

C6H5NH2 + 3Br2

Br2/H2O

+ 3HBr--------(ii i)

Br Br

Br

NH2

Ans.(2,4,6 tribromoaniline)

4) Give equation to synthesis methanamine by Gabriel Phthalimide synthesis.

NH

O

O

NK

O

O

KOHalc

-H2O

CH3INCH3

O

O

H2O/H+

COOH

COOH

+ CH3NH2

phthalimide potass ium phthalimide

N Methyl phthalimide

phthalic acid

methanamine

heat

NH2 + HNO2 + HCl N N Cl

-2H2O

0 to 5oC

Aniline

benzene diazonium chloride

5) Identify the major product of the following.

(i) Explain coupling reaction with an example.

N N Cl + OHH N N OHOH

-

-HCl

p Hy droxy azobenzene

NO2

Sn/HCl(i i)

Give the IUPAC name of the compound formed when nitrobenzene is treated with Sn/con.HCl.

NH2

aniline

Ans.

6) Explain with an example Hoffmann Bromamide reaction.

When an amide is heated with Br2 and KOH, primary amine is obtained.

CH3CONH2 + Br2 + 4KOH CH3NH2 + 2KBr + 2H2O + K2CO3acetamide Methanamine

14. BIOMOLECULES

1) Glucose on oxidation with water gives gluconic acid. What does this

reaction indicates about the structure of glucose?

This indicates that carbonyl group in glucose is present as an aldehydic group.

2) Why cellulose cannot be digested by human being? Cellulose cannot be digested by human beings due to the absence of the enzyme

cellulase.

2 - MARKS

3) Write the Haworth Structure of Maltose?

Maltose_- Its disaccharide consisting of two alpha D( +) glucose units.

Glycosidic linkage: - C1-C4 of alpha -D (+) glucopyranose units.

4) Write the Haworth structure of Sucrose.

Sucrose- It’s a disaccharide consisting of glucose and fructose unit.

Glycosidic Linkage: - C1 of alpha D (+)-glucopyranose-C2 of -D(-)

Fructofuranose

5) Write the Haworth structure of Lactose.

Lactose-It is disaccharide containing -D(+) Galactose and -D(+)glucose

Glycosidic Linkage:-C1--D (+) galactopyranose-C4--D (+) glucopyranose

6) What are hormones? Give one biological function of Insulin?

Hormones are the chemical substances produced by endocrine glands, which act

as biochemical messengers.Insulin- is a hormone which maintains blood sugar level in the

body.

7) Why is sucrose a Non- reducing sugar?

In sucrose, the aldehydicgroup of glucose and keto group of fructose are involved

in glycosidic linkage. Hence neither aldehydeic nor ketonic group are free therefore

does not reduce.Fehling’s and Tollens reagent.

8) What is a peptide bond? How many peptide bonds are present in tetra peptide?

Peptide bond is an amide bond or linkage formed by the reaction between amino group

of one amino acid molecule with carboxylic group of another amino acid molecule

by elimination of water. There are 4 amino acid residues and 3 peptide bonds.

9) Give differences between essential and non essential amino acids?

Essential amino acids- These are amino acids which cannot be synthesized in the

body and must be supplied through protein diet.

Ex: Lysine

Non -essential amino acids-These are amino acids which can be synthesized in the

body, not essential to supply through the diet. Ex: Glycine

10) Name a) sugar mostly present in DNA, b) N-base present in DNA but not in RNA?

A) -D-2-Deoxyribose

B) Thymine.

11) How will you prove the presence of five hydroxyl group in glucose?

Acetylation of glucose with acetic anhydride gives glucose penta acetate which

confirms the presence of five -OH groups attached to different c-atoms Reaction incomplete -

12) Mention any 2 importance of nucleic acids?

A) DNA is chemical basis of heredity and reserve of genetic information?

B) For protein synthesis in the cell.

13) Name the Hormone that contains Iodine?

Thyroxine

14) Name the storage Polysaccharide present in animals?

Glycogen

15) Deficiency of which vitamin leads to night blindness?

Vitamin-A

16) Which Hormone is responsible for hyperthyroidism?

Thyroxin

17) What is a Nucleotide? Phosphoric acid esters of nucleosides

[Nucleoside-sugar + base + phophoric acid]

18) Name the water insoluble component present in starch?

Amylopectin

19) Name a naturally occurring alpha-amino acid that is opticallyinactive?

Glycine

20) Why vitamin- C cannot be stored in the body?

Vitamin-C is soluble in water, hence can be easily excreted out, and so must be supplied

through the diet.

21) Name the heterocyclic nitrogen containing base present only in DNA but not in

RNA?

Thymine

22) Among the following, which is a fat soluble vitamin-Vit B-12,Vit-C, and Vit-D?

Vit-D

23) What are nucleosides?

It is a compound containing nitrogen base and pentose sugar

24) Name the nitrogenous base present in RNA only?

Uracil

25) What is zwitter ion?

In aqueous solution, the carboxyl group can lose a proton and

amino group can accept a proton giving rise to a dipolar ion

26) Define isoelectric pH?

It is the pH at which the ammonia acid does not move either to the cathode or to

the anode

27) Give an example for each of the following?

(1) Aromatic amino acid -Tryptophan

(2) Heterocyclic amino acid-Proline

(3) Acid amino acid-Aspartic acid

(4) Basic amino acid-Lysine

28) What is denaturation of protein?

Coagulation of protein or loss of biological activity of protein by change.

29) Name the growth hormone?

Thyroxin

30) Name a Sulphur containing amino acid?

Cysteine

31) Name a vitamin that is stored in liver and adipose tissues.

Vitamin A/D/E/K (Any one of these)

32) What does the Primary structure specify about structure of protein?

It represents the number and sequence of amino acid in the

33) Name a hormone which regulates the blood sugar level in the body?

Name the metal present in insulin.

Insulin. The metal present in insulin is Zinc

15. Polymers

a. Write the partial structure of Bakelite.

OH

2nOH

OH OH

n

2CH OH 2CH

2CH

Bakelite

b. Which among the following is a homopolymer and copolymer?

a) Nylon 6, 6 -copolymer

b) PVC- Homopolymer.

c. How is Buna-N prepared? Write an equation.

It is obtained by the copolymerization of 1, 3-butadiene and acrylonitrile in the

presence of a peroxide catalyst.

d. How is Neoprene prepared? Give equation.

It is formed by polymerization of chloroprene.

e. Give any 2 differences thermosetting and thermoplastics.

SL.NO. Thermosetting Thermoplastics

1 polymers that become hard

and insoluble on heating.

Polymers that soften on heating and harden on

cooling

2 3-D cross linking polymer chain held by intermolecular forces which

are in between those of elastomers and fibres

3. cannot be remoulded Can be remoulded

Ex: Bakelite, Urea-

formaldehyde

Ex : Polythene, PVC

f. What are condensation polymers? Give an example.

These are the polymers obtained by the combination of two different bi-functional

or trifunctional monomeric units with the elimination of simple molecules like water, NH3,alcohol

etc. Ex. Nylon -6, 6, Terylene, Bakelite.

g. What are addition polymers? Give an example.

These polymers formed by the repeated addition monomer molecules possessing

double or triple bonds.Ex: Polythene, PVC

h. With respect to natural rubber,

(a) Name its Monomer

(b) Name the element used for Vulcanization.

Ans: (a)Isoprene (2 Methyl-1, 3-Butadiene) (b) Sulphur

i. What is a biodegradable synthetic polymer? Give an example.

These polymers undergo environmental degradation.

Ex: PHBV, Nylon-2-nylon-6

j. Give an example for a non-biodegradable polymer.

Polythene, PVC

k. Give an example for thermoplastic polymer.

PVC, Polythene

l. Name the monomer of Nylon-6.

Caprolactum

m. Name the monomer of Nylon-6, 6.

Adipic acid and hexamethylenediamine

n. Give the IUPAC name of the monomer of natural rubber

Isoprene (2-methyl-1,3-butadiene)

o. Name the dicarboxylic acid used as one of the monomer in the manufacture of

Terylene.

Terephthalic acid

16. CHEMISTRY IN EVERYDAY LIFE

1) Name some antioxidant

Vitamin-E, Butylated hydroxyl toluene (BHT),

2) What are Antibiotics?

These are chemicals which are produced by micro organisms and

are capable of inhibiting the growth and Metabolism of other micro organisms.

3) Name two commonly used food preservatives

Table salt, Sugar

4) What are Tranquilizers?

The chemicals which provides soothing effect on mind.

5) What are Analgesics?

These are chemicals used to relieve pain

6) What is Chemotherapy?

It is the treatment of diseases using chemicals without affecting the host tissues

7) What are Antiseptics?

Antiseptics are chemicals applied to cuts, wounds, scratches to kill or prevent the

growth of microorganisms

8) What are disinfectants?

The drugs which are used to kill bacteria and used for sterilization of inanimate

objects like floors, clothes, etc

9) What is artificial sweetener?

These are non-nutritive sweetening agents used as substitutes for

sugar in foods and beverages

10) Give two examples for artificial sweetening agents.

Aspartame, Saccharin

11) Give one examples for Tranquilizer.

Equanil, Chlordiazepoxide

12) What are antifertility drugs? Give an example.

Drugs which are used in birth control or which prevents pregnancy.

Ex. Norethindrone, Novestrol.