Wolframite ore is separated from tinstone by the process of________.

(a)

Smelting

(b)

Calcination

(c)

Roasting

(d)

Electromagnetic separation

Zinc is obtained from ZnO by________.

(a)

Carbon reduction

(b)

Reduction using silver

(c)

Electrochemical process

(d)

Acid leaching

Among the following, one does not belong to calcination, Pick the odd one out.

(a)

\({ PBCO }_{ 3 }\overset { \Delta }{ \longrightarrow } PBO+{ CO }_{ 2 }\uparrow \)

(b)

\({ CaCo }_{ 3 }\overset { \Delta }{ \longrightarrow } Cao+{ CO }_{ 2 }\uparrow \)

(c)

\(PbS{ O }_{ 3 }\overset { \Delta }{ \rightarrow } PbO+{ 2SO }_{ 2 }\uparrow \)

(d)

\({ ZnCO }_{ 3 }\overset { \Delta }{ \rightarrow } ZnO+{ CO }_{ 2 }\uparrow \)

Zinc is extracted from Zinc blende by________.

(a)

Carbon reduction process

(b)

Nitrogen reduction process

(c)

Oxygen reduction process

(d)

All of these

Na[Ag(CN)₂] is _________.

(a)

Sodium aurocyanide

(b)

Sodium meta aluminate

(c)

Aluminosilicate

(d)

Sodium dicyano argentate

Boric acid is an acid because its molecule________.

(a)

contains replaceable H⁺ ion

(b)

gives up a proton

(c)

combines with proton to form water molecule

(d)

accepts OH^- from water, releasing proton.

The stability of +1 oxidation state increases in the sequence ________.

(a)

Al < Ga < In < Tl

(b)

Tl < In < Ga < Al

(c)

In < Tl < Ga < Al

(d)

Ga< In < Al < Tl

SiO₄^4- ion has ____ geometry.

(a)

Triangular

(b)

Tetrahedral

(c)

Linear

(d)

Pentagonal bipyramidal

In graphite electrons are _______.

(a)

localised on each C-atom

(b)

localised on every third C-atom

(c)

delocalised within the layer

(d)

present in anti-bonding orbital

Allotropy is due to ______.

(a)

difference in chemical properties

(b)

difference in the number of atoms in the molecules

(c)

difference in the arrangement of atoms in the molecules in the crystal

(d)

None of these

Solid (A) reacts with strong aqueous NaOH liberating a foul smelling gas(B) which spontaneously burn in air giving smoky rings. A and B are respectively_________.

(a)

P₄(red) & PH₃

(b)

P₄(white) & PH₃

(c)

S₈ & H₂S

(d)

P₄(white) & H₂S

When copper is heated with conc HNO₃ it produces ________.

(a)

Cu(NO₃)₂, NO and NO₂

(b)

Cu(NO₃)₂ and N₂O

(c)

Cu(NO₃)₂ and NO₂

(d)

Cu(NO₃)₂ and NO

Which of the following is correct?

(a)

H₃PO₃ is dibasic and reducing

(b)

H₃PO₃ is dibasic and non-reducing

(c)

H₃PO₄ is tribasic and reducing

(d)

H₃PO₃ is tribasic and non-reducing

The hybridisation and shape of SF₆ is respectively?

(a)

sp³d², square planar

(b)

sp³d², octahedral

(c)

sp³d see-saw

(d)

sp³d, trigonal bipyramindal

Pick the wrong one among the following

(a)

F₂ - Yellow

(b)

Br₂ - Red

(c)

Cl₂ - Colourless

(d)

I₂- Violet

Which of the following does not give oxygen on heating?

(a)

K₂Cr₂O₇

(b)

(NH₄)₂Cr₂O₇

(c)

KClO₃

(d)

Zn(ClO₃)₂

When a brown compound of Mn (A) is treated with HCl, it gives a gas (B). The gas (B) taken in excess reacts with NH₃ to give an explosive compound (C). The compound A, B and C are ________.

(a)

MnO₂, Cl₂, NCl₃

(b)

MnO, Cl₂, NH₄Cl

(c)

Mn₃O₄, Cl₂, NCl₃

(d)

MnO₃, Cl₂, NCl₂

Ce (Z=58) and Yb (Z=70) exhibits stable +4 and +2 oxidation states respectively. This is because_______.

(a)

Ce⁴⁺ and Yb²⁺acquire f⁷ configuration

(b)

Ce⁴⁺ and Yb²⁺ acquire f⁰ configuration

(c)

Ce⁴⁺ and Yb²⁺acquire f⁷ and f¹⁴ configuration

(d)

Ce⁴⁺and Yb²⁺ acquire f⁰ and f¹⁴ configuration

CrO₃ is coloured due to_______.

(a)

Low l.E

(b)

Crystal defects

(c)

Charge transfer spectra

(d)

Unpaired electrons

FeSO₄ on heating gives _______.

(a)

SO₂ and O₂

(b)

SO₂ and SO₃

(c)

SO₂

(d)

SO₃

How many geometrical isomers are possible for [Pt(Py)(NH₃)(Br)(Cl)]?

(a)

3

(b)

4

(c)

0

(d)

15

Which one of the following complexes is not expected to exhibit isomerism?

(a)

[Ni(NH₃)₄(H₂O)₂]²⁺

(b)

[Pt(NH₃)₂Cl₂]

(c)

[Co(NH₃)₅SO₄]Cl

(d)

[FeCl₆]^3-

A metal ion from the first transition series forms an octahedral complex with magnetic moment of 4.9 BM and another octahedral, complex which is diamagnetic. The metal ion is _______.

(a)

Fe²⁺

(b)

Co²⁺

(c)

Mn²⁺

(d)

Ni²⁺

Consider the following statements and identify the incorrect statement(s).
(i) CN^- is a powerful ligand.
(ii) Haemoglobin is a monomer and myoglobin is a tetramer.
(iii) Cis - Pt (NH₃)₂Cl₂ is an anti-tumor drug.

(a)

only (i)

(b)

only (ii) 

(c)

only (iii)

(d)

both (i) and (iii) 

Crystal field stabilization energy for high spin d⁴ octahedral complex is ______.

(a)

- 0. 6 \({ \triangle }_{ 0 }\)

(b)

- 1. 8 \({ \triangle }_{ 0 }\)

(c)

- 1. 6 \({ \triangle }_{ 0 }\)

(d)

- 1. 4 \({ \triangle }_{ 0 }\)

The cation leaves its normal position in the crystal and moves to some interstitial position, the defect in the crystal is known as _____.

(a)

Schottky defect

(b)

F center

(c)

Frenkel defect

(d)

non-stoichiometric defect

The crystal with a metal deficiency defect is ________.

(a)

NaCl

(b)

FeO

(c)

ZnO

(d)

KCl

A solid with formula ABC₃ would probably have, _______.

(a)

A at body centre, B at face centres and C at corners of the cube

(b)

A at corners of cube, B at body centre, C at face centre

(c)

A at corners of hexagon, B at centres of the hexagon and C inside the hexagonal unit cell

(d)

A at corner, B at face centre, C at body centre

The empty space between the shaded balls and hollow balls as shown in the diagram is called, _______.

(a)

Hexagonal void

(b)

Octahedral void

(c)

Tetrahedral void

(d)

Double triangular void

Iodine crystals are ________.

(a)

covalent

(b)

ionic

(c)

metallic

(d)

molecular

For a first order reaction A ⟶ product with initial concentration x mol L^-1, has a half life period of 2.5 hours. For the same reaction with initial concentration \(\left( \frac { x }{ 2 } \right) \) mol L^-1 the half life is

(a)

(2.5 x 2) hours

(b)

\(\left( \frac { 2.5 }{ 2 } \right) \) hours

(c)

2.5 hours

(d)

Without knowing the rate constant, t_1/2 cannot be determined from the given data

For a reaction Rate = k[acetone]^3/2 then unit of rate constant and rate of reaction respectively is _______.

(a)

(mol L^-1 S^-1),(mol^1/2 L^1/2 S^-1)

(b)

(mol^-1/2 L^1/2 s^-1),(mol L^-1 s^-1)

(c)

(mol^1/2 L^1/2 s^-1),(mol L^-1 s^-1)

(d)

(mol L s^-1),(mol^1/2 L^1/2 s)

For a reaction: aA ⟶ bB, the rate of reaction is doubled when the concentration of A is increased by four times. The rate of reaction is equal to _____.

(a)

k[A]^a

(b)

\(k{ \left[ A \right] }^{ \frac { 1 }{ 2 } }\)

(c)

\(k{ \left[ A \right] }^{ \frac { 1 }{ a } }\)

(d)

K[A]

For the reaction N_2(g) + 3H_2(g) ⟶ 2NH_3(g) the rate of the reaction in terms of ammonia is ______.

(a)

\(+\frac { 1 }{ 2 } \frac { -d\left[ { NH }_{ 3 } \right] }{ dt } \)

(b)

\(-\frac { 1 }{ 2 } \frac { d\left[ { NH }_{ 3 } \right] }{ dt } \)

(c)

\(\frac { -d\left[ { NH }_{ 3 } \right] }{ dt } \)

(d)

\(\frac { +d\left[ { NH }_{ 3 } \right] }{ dt } \)

The half-life period of a first order reaction is 69.3 seconds. Its rate constant is ________.

(a)

10^-2 s^-1

(b)

10^-4 s^-1

(c)

10 s^-1

(d)

10² s^-1

What is the decreasing order of strength of bases
OH, NH₂^- H - C ≡ C and CH₃ - CH₂^-

(a)

OH^->NH₂^- >H-C≡C >CH₃^-CH₂^-

(b)

NH₂^->OH^->CH₃^-CH₂^- >H-C≡C

(c)

CH₃^-CH₂^->NH₂^->H-C≡C^->OH^-

(d)

OH^->H-C ≡ C^->CH₃^-CH₂^- >NH₂^-

Using Gibb’s free energy change, ∆G^o=57.34 kJ mol^-1, for the reaction, X₂Y_(s)⇌2X⁺+Y^2- (aq), calculate the solubility product of X₂Y in water at 300 K_______. (R = 8.3 J K^-1Mol^-1)

(a)

10^-10

(b)

10^-12

(c)

10^-14

(d)

can not be calculated from the given dat

K_w represents _______.

(a)

ionic product constant of water

(b)

Solubility product of water

(c)

Equilibrium constant of water

(d)

Buffer index

For two acids A and B, K_a values at 25°C are 2 x 10⁶ and 1.8 x 10^-4 respectively. which among the following is true with respect to the above data _______.

(a)

A and B are equally acidic

(b)

A is stronger than B

(c)

B is stronger than A

(d)

K_a value is not a measure of acid strength

NH₄OH is a weak base because _______.

(a)

it has low vapour pressure

(b)

it is only partially ionised

(c)

it is completely ionised

(d)

it has low densit

In the electrochemical cell: Zn|ZnSO_{4 (0.01M)}|| CuSO_{4 (1.0M)}|Cu, the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0M and that CuSO₄ changed to 0.01M, the emf changes to E₂. From the above, which one is the relationship between E₁ and E₂?

(a)

E₁ < E₂

(b)

E₁ > E₂

(c)

E₂ ≥ E₁

(d)

E₁ = E₂

A gas X at 1 atm is bubbled through a solution containing a mixture of 1MY^- and 1MZ^- at 25^oC. If the reduction potential of Z>Y>X, then_____.

(a)

Y will oxidize X and not Z

(b)

Y will oxidize Z and not X

(c)

Y will oxidize both X and Z

(d)

Y will reduce both X and Z

The important use of Kohlrausch's law is deducing the ______.

(a)

λ_∞ value of weak electrolyte.

(b)

λ_∞ value of strong electrolyte.

(c)

λ_∞ value of weak electrolyte.

(d)

λ_∞ value of weak electrolyte

What is/are the factor(s) that govern the single electrode potential of a half cell?

(a)

concentration of ions in solution

(b)

tendency to form ions

(c)

temperature

(d)

all of these

In an electrochemical cell, the wrong statement is ______.

(a)

electrons move from cathode to anode

(b)

anode is negative charged

(c)

cathode is positive charged

(d)

chemical energy is converted to electrical energy.

The most effective electrolyte for the coagulation of As₂S₃Sol is _______.

(a)

NaCl

(b)

Ba(NO₃)₂

(c)

K₃[Fe(CN)₆]

(d)

Al₂(SO₄)₃

Adsorption of a gas on solid metal surface is spontaneous and exothermic, then ______.

(a)

ΔH increases

(b)

ΔS increases

(c)

ΔG increases

(d)

ΔS decreases

The impurity present in the colloidal particle is _______.

(a)

electrolytes

(b)

solute

(c)

both (a) and (b)

(d)

neither (a) or (b)

In W/O system, the dispersion medium is_______

(a)

water

(b)

benzene

(c)

alcohol

(d)

oil

Decomposition of hydrogen peroxide is retarded in the presence of________.

(a)

alcohol

(b)

glycerine

(c)

MnO₂

(d)

Mo

The X is _______.

(a)

(b)

(c)

(d)

None of these

Among the following ethers which one will produce methyl alcohol on treatment with hot HI?

(a)

(H₃C)₃C-O-CH₃

(b)

(CH₃-)₂-CH-CH₂-O-CH₃

(c)

CH₃-(CH₂)₃-O-CH₃

(d)

CH₃-CH₂-\(\underset { \overset { | }{ { CH }_{ 3 } } }{ CH } \)-O-CH₃

An example of trihydric alcohol is _________.

(a)

trimethyl carbinol

(b)

3-hexanol

(c)

propane-1,2,3-triol

(d)

tert-butylacohol

CH₃-CH₂-O-CH₂CH₃ and \({ CH }_{ 3 }-O-\overset { \underset { | }{ { CH }_{ 3 } } }{ CH } -{ CH }_{ 3 }\) are examples of _______ isomerism.

(a)

functional

(b)

chain

(c)

position

(d)

metamerism

_______ cannot be prepared by using Grignard reagent.

(a)

CH₃- OC₂H₅

(b)

CH₃-OCH₃

(c)

C₂H₅-O-C₂H₅

(d)

CH₃-OCH₂CH₂CH₃

In which case chiral carbon is not generated by reaction with HCN?

(a)

(b)

(c)

(d)

An alkene “A” on reaction with O₃ and Zn - H₂O gives propanone and ethanol in equimolar ratio. Addition of HCl to alkene “A” gives “B” as the major product. The structure of product “B” is ______.

(a)

\(Cl-{ CH }_{ 2 }-CH_{ 2 }-\overset { \overset { CH_{ 3 } }{ | } }{ \underset { \underset { CH_{ 3 } }{ | } }{ CH } } \)

(b)

\({ H }_{ 3 }C-{ CH }_{ 2 }-\overset { \overset { CH_{ 2 }Cl }{ | } }{ CH } -{ CH }_{ 3 }\)

(c)

\(\\ { H }_{ 3 }C-{ CH }_{ 2 }-\overset { \overset { CH_{ 3 } }{ | } }{ \underset { \underset { CL{ } }{ | } }{ C } } -{ CH }_{ 3 }\)

(d)

\({ H }_{ 3 }C-{ CH }-\overset { \overset { CH_{ 3 } }{ | } }{ \underset { \underset { Cl }{ | } }{ C } } \)

When propanoic acid is treated with aqueous sodium-bicarbonate, CO₂ is liberated. The "C" of CO comes from _______.

(a)

methyl group

(b)

carboxylic acid group

(c)

methylene group

(d)

bicarbonate

Chloroacetic acid is stronger than acetic acid due to _______.

(a)

+ I effect

(b)

- I effect

(c)

+ M effect

(d)

- M effect

Lower members of carboxylic acid family are _______.

(a)

waxy solids

(b)

pleasant smelling liquids

(c)

foul smelling liquids

(d)

inert gases

What are the differences between minerals and ores?

What is the role of quick lime in the extraction of Iron from its oxide Fe₂O₃?

Why should we have a ecofriendly metallurgical process?

What are the different methods of concentration of ores?

Write a short note on anamolous properties of the first element of p-block.

Describe briefly allotropism in p- block elements with specific reference to carbon.

What are alums?

Starting from SiCl₄, prepare the following in steps not exceeding the number given in parentheses.
(i) Silicon
(ii) Linear silicon containing methyl groups only
(iii) Na₂SiO₃

Give the oxidation state of halogen in the following.
a) OF₂
b) O₂F₂
c) Cl₂O₃
d) I₂O₄

Give the uses of helium.

What is the reaction of Phosphorous with alkali?

Acidic character increases from HF to HI. State whether the above statement is True or false and give reason for your answer.

What are actinides? Give three examples.

Why Gd³⁺ is colourles?

Which is the most common oxidation state of lanthanoides?

Comparing La(OH)₃ and Lu(OH)₃, which is more basic and explain why?

Calculate the ratio of \(\frac { \left[ { Ag }^{ + } \right] }{ \left[ Ag\left( NH_{ 3 } \right) _{ 2 } \right] ^{ + } } \) in 0.2 M solution of NH_3. If the stability constant for the complex \([Ag(NH_{ 3 })_{ 2 }]^{ + }\) is 1.7 x 10⁷

Based on VB theory explain why [Cr(NH₃)₆]³⁺ is paramagnetic, while [Ni(CN)₄]^2- is diamagnetic.

Write a neutral molecule in which the central atom is Sp³d² hybridised.

Write the IUPAC name of [Cu(NH₃)₄]SO₄

Why do solids have a definite volume?

What is the total number of atoms per unit cell in a face - centered cubic structure (fcc)?

Define average rate and instantaneous rate.

Explain the rate determining step with an example.

For a reaction A + B ⟶ C, the rate of the reaction is denoted \(\frac { -dA }{ dt } \) or \(\frac { -dB }{ dt } \) or \(\frac { +dC }{ dt } \). State the significance of plus and minus sign.

In a reaction, 2A \(\longrightarrow \) products, the concentration of A decreases from 0.5 mol L^-1 to 0.4 mol L^-1 in 10 minutes. Calculate the rate during this interval?

Account for the acidic nature of HClO₄ in terms of Bronsted – Lowry theory, identify its conjugate base.

Define solubility product.

Give a condition for a compound to be precipitated.

BF₃ is termed as an acid though it does not contain H⁺ ions. Explain.

Describe the construction of Daniel cell. Write the cell reaction.

The resistance of a conductivity cell is measured as 190 Ω using 0.1M KCl solution (specific conductance of 0.1M KCl is 1.3 Sm^-1). When the same cell is filled with 0.003 M sodium chloride solution, the measured resistance is 6.3KΩ. Both these measurements are made at a particular temperature. Calculate the specific and molar conductance of NaCl solution.

On dilution of 0.1 M of Na₂SO₄, what will happen to its
(a) Conductance (C)
(b) Conductivity K
(c) Molar conductance \({ \Lambda }_{ m }\)
(d) Equivalent conductance \({ \Lambda }\)

Why is the electrode potential of a single electrode cannot be determined?

What is Ultrafilteration?

What is difference between sol gel and emulsion?

Identify the product A and B.

Which of the following does not give iodoform reaction?

Complete the following reaction

Write a note on Claisen Condensation.

Explain zone refining process with an example.

What is cementation?

AlCl₃ behaves like a lewis acid. Substantiate this statement.

Describe the structure of diamond.

Give the balanced equation for the reaction between chlorine with cold NaOH and hot NaOH.

Explain the reaction of ammonia with chlorine and chlorides at different conditions.

Explain the variation in E⁰_{M³⁺/M²⁺}  3d series.

Explain why oxidation states of transition elements increases first from Sc to Mn and then decrease?

Give one test to differentiate [Co(NH₃)₅Cl]SO₄ and [Co(NH₃)₅SO₄]Cl.

Aqueous copper sulphate solution (blue) gives
(i) a green precipitate with aqueous potassium fluoride.
(ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.

Answer the following:
(I) Name the intermolecular force present in ice.
(II) What type of bond is present in network solid?

Explain briefly the collision theory of bimolecular reactions.

The energy of achivation for the formation of hydrogen iodide is 150 kJ mol^-1 The rate constant of this reaction at 673 K is 2.3 x 10^-3. Calculate the rate constant at 773 K.

Derive an expression for Ostwald’s dilution law.

What do you mean by buffer action?

Can Fe³⁺ oxidises Bromide to bromine under standard conditions?
Given: \({ E }_{ { Fe }^{ 3+ }|{ Fe }^{ 2+ } }^{ 0 }=0.771V\); \(\\ { E }^{0}_{ { Br }_{ 2 }|{ Br }^{ - } }=1.09V\).

What is the oxidation and reduction half cell in a Daniel cell?

What happens when a colloidal sol of Fe(OH)₃ and As₂S₃ are mixed?

What are the advantages of Brownian movement?

What happens when 1-phenyl ethanol is treated with acidified KMnO₄.

Ethers should not be heated to dryness. Why?

What is acidity constant? How is it expressed.

Write short note on the following:
(i) The process in which no external reducing agent is used.
(ii) The process which is used for highly electro positive metal.
(iii) Write the equation involved in the thermite process.

Distinguish between diamond and graphite.

An amorphous solid (A) burns in air to form a gas (B) which turns lime water milky. The gas is also produced as a byproduct during roasting of sulphide ore. This gas decolourises acidified aqueous KMnO₄ solution and reduces Fe³⁺ to Fe²⁺. Identify the solid 'A' and the gas 'B' and write the reactions involved.

Why is there a variation of atomic andionic size as we move from Sc to Zn?

Give the postulates and limitation of Werner's theory of co-ordination compounds.

What are the general characteristics of solids?

The initial rate of a first order reaction is 5.2 x 10^-6 mol lit^-1 S^-1 at 298 K. When the initial concentration of reactant is 2.6 x 10^-3 mol.lit^-1, calculate the first order rate constant of the reaction at the same temperature.

A 0.02 M solution of a weak mono basic acid is 5% ionised. Calculate the ionisation constant of the acid.

The equilibrium constant of cell reaction: Ag_(s) + Fe³⁺ ⇌ Fe²⁺ + Ag⁺ is 0.335 at 25°C. Calculate the standard emf of the cell AgI Ag⁺; Fe³⁺, Fe²⁺/Pt. Calculate E^o of the half cell Fe³⁺, Fe²⁺/Pt is 0.7791 V. Calculate E^o of Fe³⁺, Fe²⁺/ Pt half cell.

Write a note on phase transfer catalysis.

Compound (A) with molecular formula C₆H₆O gives violet colour with neutral FeCI₃ (A) reacts with CHCl₃ and NaOH gives two isomers (B) and (C) with molecular formula C₇H₆O₂ Compound (A) reacts with ammonia at 473 K in the presence of ZnCl₂ gives compound (D) with molecular formula C₆H₇N. Compound (D) undergoes carbylamine test. Identify (A), (B), (C) and (D) and explain the reactions.

An organic compound (A) of molecular formula C₇H₆O is not reduced by Fehling's solution but will undergo Cannizzaro reaction. Compound (A) reacts with aniline to give compound (B). Compound (A) also reacts with Cl₂ in the presence of catalyst to give compound (C). Identify (A) (B) and (C) and explain the reactions.