Dichloromethane has highest dipole moment among CH₂​Cl₂​, CHCl₃​ and CCl₄​. The decreasing order of dipole moments is CH₂​Cl₂​>CHCl₃​>CCl₄​. These molecules have tetrahedral geometry due to sp3 hybridization of carbon atom.In CCl4​, the individual C−Cl bond dipoles cancel each other which results in zero dipole moment. 
Hence, CCl₄​ is non polar.

(i) 2-Chloro-3-methylpentane
 
(ii) p-Bromochlorobenzene
 
(iii)  1-Chloro-4-ethylcyclohexane
 
(iv)  2-(2-Chlorophenyl)-1-iodooctane
 
(v) 2-Bromobutane
 
(vi) 4-tert-Butyl-3-iodoheptane
 
(vii) 1-Bromo-4-sec-butyl-2-methylbenzene
 
(viii) 1,4-Dibromobut-2-ene

(i) Cyclopentanone reacts with hydroxyl amine to form oxime.
 
(ii) \(\text { a } \beta\)unsaturated aldehyde reacts with semicarbazide (H₂NCONHNH₂) to form semicarbazone. 

(iii) Cyclohexanone reacts with 2,4-dinitro phenyl hydrazine to form 2,4-dinitro phenyl hydrazone.

(iv) Acetophenone reacts with  ethyl amine to form an imine

The variability in oxidation states of transition metals is due to the incomplete filling of d-orbitals in such a way that their oxidation states differ from each other by unity, e.g., Fe⁺ and Fe³⁺, Cu⁺ and Cu²⁺ etc. In the case of non-transition elements, the oxidation states differ by units of two, e.g., Pb²⁺ and Pb⁴⁺, S²⁺ and S⁴⁺ etc. Moreover, in transition elements, the higher oxidation states are more stable for heavier elements in a group. For example, in group 6, Mo (VI) and W (VI) are more stable than Cr (VI). In P block elements, the lower oxidation states are more stable for heavier members due to inert pair effect, e.g., in group 16, Pb (II) is more stable than Pb (IV).

We know from Kohlrausch law that
\(A_{m\left(\mathrm{CaCl}_{2}\right)}^{\mathrm{o}}=\lambda_{\mathrm{Ca}^{2+}}^{0}+2 \lambda_{\mathrm{Cl}^{-}}^{0}=119.0 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}+2(76.3) \mathrm{S} \mathrm{cm}^{2} \mathrm{~mol}^{-1}\)
= (119.0 + 152.6) S cm² mol^–1
= 271.6 S cm² mol^–1
\(A_{n\left(\mathrm{MgSO}_{4}\right)}^{\mathrm{o}}=\lambda_{\mathrm{Mg}^{2+}}^{0}+\lambda_{\mathrm{so}_{4}^{2}}^{0}=106.0 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}+160.0 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}\)
= 266 S cm² mol^–1

(i) and (ii)
Eight isomers of C₄H₁₁N are
(a) \(\stackrel{4}{\mathrm{C}} \mathrm{H}_3-\stackrel{3}{\mathrm{C}} \mathrm{H}_2-\stackrel{2}{\mathrm{C}} \mathrm{H}_2-\stackrel{1}{\mathrm{C}} \mathrm{H}_2-\mathrm{NH}_2\)
                     Butan -1 -amine
                               (Primary)
(b)           CH₃
                    |
\(\stackrel{3}{CH}_3-{ }^2 \mathrm{CH}-\stackrel{1}{C} \mathrm{H}_2-\mathrm{NH}_2\)
            2-methyl propan -1-amine
                     (Primary)

(iii) Isomerism exhibited by different amines are:
(a) Chain isomers, i.e. have different carbon chains, (a) and (b), (c) and (d) (as discussed in part (i) and (ii)]
(b) Position isomers, i.e. functional group occupy different positions, (a) and (c), (b) and (d). 
(c) Metamers, i.e. different alkyl groups are attached to the same functional group, (e) and (f), (e) and (g).
(d) Functional isomers, i.e. they have different functional groups. All the three categories (1°, 2° and 3°) of amines are the functional isomers of each other.

\({ { \wedge }^{ ° } }_{ \left( HCOOH \right) }={ { \lambda }^{ ° } }_{ \left( { H }^{ + } \right) }+{ { \lambda }^{ ° } }_{ \left( { HCOO }^{ - } \right) }\)
\(=349.6+54.6\\=404.2S{ cm }^{ 2 }{ mol }^{ -1 }\)
\(\alpha =\frac { { { { \wedge } }^{ m } }_{ c } }{ { { { \wedge } }^{ m } }_{ 0 } } =\frac { 46.1 }{ 404.2 } =0.114\)
\({ K }_{ c }=\frac { c{ \alpha }^{ 2 } }{ 1-\alpha } =\frac { 0.025\times { \left( 0.114 \right) }^{ 2 } }{ 1-0.114 } =3.67\times { 10 }^{ -4 }\)

According to Raoult’s Law,
\(\frac{\mathrm{P}_{\mathrm{A}}^{\circ}-\mathrm{P}_{\mathrm{S}}}{\mathrm{P}_{\mathrm{S}}}=\frac{n_{\mathrm{B}}}{n_{\mathrm{A}}}=\frac{\mathrm{W}_{\mathrm{B}}}{\mathrm{M}_{\mathrm{B}}} \times \frac{\mathrm{M}_{\mathrm{A}}}{\mathrm{W}_{\mathrm{A}}}\)
\(\text { Let } \mathrm{P}_{\mathrm{A}}^{\circ}=1 \mathrm{~atm}, \mathrm{P}_{\mathrm{S}}=0 \cdot 8 \mathrm{~atm} ; \mathrm{P}_{\mathrm{A}}^{\circ}-\mathrm{P}_{\mathrm{S}}=0 \cdot 2 \mathrm{~atm} ; \mathrm{M}_{\mathrm{B}}=40 \mathrm{~g} \mathrm{~mol}^{-1} ; \mathrm{W}_{\mathrm{A}}=114 \mathrm{~g} \)
\(\mathrm{M}_{\mathrm{A}}\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)=114 \mathrm{~g} \mathrm{~mol}^{-1} \)
\(\mathrm{W}_{\mathrm{B}}=\frac{\left(\mathrm{P}_{\mathrm{A}}^{\circ}-\mathrm{P}_{\mathrm{S}}\right)}{\mathrm{P}_{\mathrm{S}}} \times \frac{\mathrm{M}_{\mathrm{B}} \times \mathrm{W}_{\mathrm{A}}}{\mathrm{M}_{\mathrm{A}}}\)
\(=\frac{(0 \cdot 2 \mathrm{~atm})}{(0 \cdot 8 \mathrm{~atm})} \times \frac{\left(40 \mathrm{~g} \mathrm{~mol}^{-1}\right) \times(114 \mathrm{~g})}{\left(114 \mathrm{~g} \mathrm{~mol}^{-1}\right)}=10 \cdot 0 \mathrm{~g}\)

(i)
 
(ii)
 
(iii)

(iv)

(v)
 
(vi)

(vii)

(viii)

(ix)

(x)
 
(xi)

\(\text { Average Rage } =\frac{1}{2}\left\{-\frac{\Delta\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]}{\Delta t}\right\} \)
\(=-\frac{1}{2}\left[\frac{(2.08-2.33) \mathrm{mol} \mathrm{L}^{-1}}{184 \mathrm{~min}}\right] \)
\(=6.79 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} / \mathrm{min}\)
\(=\left(6.79 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}\right) \times(60 \mathrm{~min} / 1 \mathrm{~h}) \)
\(=4.07 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} / \mathrm{h} \)
\(=6.79 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \times 1 \mathrm{~min} / 60 \mathrm{~s} \)
\( =1.13 \times 10^{-5} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
It may be remembered that
Rate \( =\frac{1}{4}\left\{\frac{\Delta\left[\mathrm{NO}_{2}\right]}{\Delta t}\right\} \)
\(\frac{\Delta\left[\mathrm{NO}_{2}\right]}{\Delta t} =6.79 \times 10^{-4} \times 4 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}\)
\(=2.72 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1} \)

(a) The high enthalpies of atomization are due to a large number of unpaired electrons in their atoms. Therefore, they have stronger interatomic interactions and hence, stronger bonding between atoms. Thus, they have high enthalpies of atomization.
(b) Most of the compounds of transition elements contain unpaired electrons in their (n-1) d-subshells. Therefore, they are paramagnetic in nature and are attracted by the magnetic field. The magnetic character is expressed in terms of magnetic moment. The larger the number of unpaired electrons in a substance, the greater is the paramagnetic character and larger is the magnetic moment. The magnetic moment is expressed in Bohr magneton abbreviated as B.M. For example, Ti²⁺ has 2 unpaired electrons and has less magnetic moment than Mn²⁺which has 3 unpaired electrons. Mn²⁺has 5 unpaired electrons and has maximum magnetic moment among the divalent transition metal ions because d-subshell can have a maximum of 5 unpaired electrons.
(c) Most of the transition metal ions are colored both in the solid state and in aqueous solutions.The color of these ions is attributed to the presence of incomplete (n - 1) d subshell. The electrons in these metal ions can be easily promoted from one energy level to another in the same d-subshell. The amount of energy required to excite the electrons to higher energy states within the same d-subshell corresponds to the energy of certain colors of visible light. Therefore, when white light falls on a transition metal compound, some of its energy corresponding to a certain color, is absorbed causing promotion of d-electrons. This is known as d-d transitions. The remaining colors of white light are transmitted and the compound appears colored. For example, hydrated cupric compounds absorb radiations corresponding to red light and the transmitted color is greenish blue (which is complementary color to red color). Thus, cupric compounds have greenish-blue color
(d) Some transition metals and their compounds act too good catalysts for various reactions. This is due to their ability to show multiple oxidation states. The common examples are Fe, Co, Ni, V, Cr, Mn, Pt, etc.The transition metals form reaction intermediates with the substrate by using empty d-orbitals. These intermediates give reaction paths of lower activation energy and therefore, increase the rate of reaction. 

2-Methyl propanal.

Methanol (CH₃OH). 

6

This is because colliding molecules may not be having proper orientation for collision to be effective.

In pure water, the entire surface is occupied by water are volatile. On adding glucose, some water molecules on the surface are replaced by glucose molecules which are non - volatile. Hence, vapour pressure is lowered.

Warming up of the solution means that the process of mixing is exothermic, i.e., \(\Delta H_{ mixing }=-ve\). This implies that the solution shows a negative deviation.

B) Assertion and reason both are correct statements but reason is not correct explanation for assertion.
Explanation:
Due to denaturation, a protein loses its biological activity. During denaturation the protein molecule uncoils from a more random conformation and precipitates from the solution.

(a) Assertion and reason both are correct statements and reason is correct explanation for assertion.

(b) Fe³⁺ is more stable than Fe²⁺. The electronic configuration of Fe³⁺ has half-filled 'd' orbitals and thus, becomes more stable.
₂₆Fe²⁺ : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶
₂₆Fe³⁺ : 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵

(c) Benzene diazonium salts are soluble in water because they are ionic in nature. Thus, (A) is correct and R is incorrect.

(a) \(\mathrm{Pb}+\mathrm{SO}_{4}^{2-} \longrightarrow \mathrm{PbSO}_{4}+2 \mathrm{e}^{-}\) (At anode)
(b) \(\mathrm{PbO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\mathrm{SO}_{4}^{2-} \longrightarrow \mathrm{PbSO}_{4}+2 \mathrm{H}_{2} \mathrm{O}\)
2 Faraday is required.
(c) \(\mathrm{M}=\frac{\text { percentage by mass } \times d \times 10}{\text { Molar mass }}\)
\(=\frac{38 \times 1.30 \times 10}{98}=\frac{494}{98}=5.041 \mathrm{M}\)
(d) Mass of solution after discharge = 3500 mL x 1.14 g mL^-1 = 3990 g
Mass of H₂ SO₄ present in solution (20%) = \(\frac{20}{100} \times 3990 \mathrm{~g}=798 \mathrm{~g}\)
(e) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{dil}) \longrightarrow 2 \mathrm{H}^{+}+\mathrm{SO}_{4}^{2-}\)
H₂O \(\rightarrow\) H⁺ + OH^-
At cathode: 2H⁺ + 2e^- \(\rightarrow\) H₂(g)
At anode: \(2 \mathrm{H}_{2} \mathrm{O} \longrightarrow 4 \mathrm{H}^{+}+4 \mathrm{e}^{-}+\mathrm{O}_{2}(g)\)
H₂ gas is liberated at cathode and O₂ gas is formed at anode.

(i) (d): Glycinate ion is an example of bidentate ligand. It contains Nand O as donor atoms.
(ii) (a)
(iii) (c) : H₂N - NH₂ does not act as chelating ligand.
The coordination by hydrazine leads to a three member highly unstable strained ring and thus it does not act as chelating agent.
(iv) (d): In Zeises salt, coordination no. of Pt is 4. Ethylene is a mono dentate ligand.