- I etiect increases the acidity. If electronegativity is high, - I effect is also high.

BF₃ → electron deficient →  Lewis acid
PF₃ → electron rich →  Lewis base
CO → having lone pair of electron →  Lewis base
F → unshared pair of electron →  Lewis base

In 140days ⇒ initial concentration reduced to (1/2) g
In 280 days ⇒ initial concentration reduced to (1/4) g
In 420 days ⇒ initial concentration reduced to (1/8) g
In 560 days ⇒ initial concentration reduced to (1/16) g

a) Fe²⁺  b) Fe³⁺  c) Fe⁰

Glucose gets oxidized to gluconic acid with mild oxidizing agents like bromine water suggesting that the carbonyl group is an aldehyde group.

(i) Phenol are only sparingly soluble in water. Actually they form only negligible hydrogen bonding with water since the size of the phenyl group is large and it almost masks the polar character of -OH group. So, phenol has a smaller dipole moment.

(ii) But methanol is soluble in soluble in water due to the formation of hydrogen bonding with water and it results in higher dipole moment. In henol, there is +ve charge on oxygen, therefore it does not undergo protonation easily.

Other metals such as aluminium, copper and silver also undergo corrosion, but at a slower rate than iron. Let us consider the reduction of aluminium,
\({ Al }_{ (s) }\rightarrow { Al }_{ (aq) }^{ 3+ }+{ 3e }^{ - }\)
Al³⁺, which reacts with oxygen in air to form a protective coating of Al₂O₃. This coating act as a protective film for the inner surface. So, further corrosion is prevented.

(i) 2-methyl propan-2-o1 < Butan-2-ol < Butan-1-ol

(ii) propan-2-ol < propan-1-ol < propan -1,3- diol < propan-1,2,3-triol

i) Cr² + 2e^- ⟶ Cr
ii) Mn²⁺ + 2e^- ⟶ Mn
iii) Fe²⁺ + 2e^- ⟶ Fe
iv) CO²⁺ + 2e^- ⟶ Co

(i) Ionic solids have high melting points.
(ii) These solids do not conduct electricity, because the ions are fixed in their lattice positions.
(iii) They are hard so strong external force can change the relative positions of ions.

The main functions of the salt bridge are
(i) To complete the electrical circuit by the allowing only ions to flow from one solution to other without mixing the two solutions.
(ii) To maintain electrical neutrality of the solution in the two half cells.

\(\mathrm{Hg}_{2} \mathrm{Cl}_{2(\mathrm{~s})} \rightleftharpoons \mathrm{Hg}_{2}^{2+} \text { (aq) }+2 \mathrm{Cl^-}_{(\mathrm{aq})}\\ s \quad \quad \quad \quad \quad \quad s \quad \quad \quad \quad \quad 2s\)
\(\mathrm{K}_{\mathrm{sp}} =\left[\mathrm{Hg}_{2}^{2+}\right]{\left[\mathrm{Cl}^{-}\right]^{2}}  \)
\(=(\mathrm{s})(2 \mathrm{~s})^{2} \)
\(\mathrm{~K}_{\mathrm{sp}} =4 \mathrm{~s}^{3}\)

Conjugate Pairs:
\((a) \mathrm{HS}_{\text {(aq) }}^{-} \& \mathrm{H}_{2} \mathrm{~S}_{\text {(aq) }} \) \((b) \mathrm{HF}_{\text {(aq) }} \& \mathrm{~F}_{\text {(aq) }}^{-} \)
\((a) \mathrm{HPO}_{4}^{2-} \& \mathrm{PO}_{4}^{3-} \) \((b) \mathrm{SO}_{3}^{2-} \& \mathrm{HSO}_{3}^{-} \)
\((a) \mathrm{NH}_{4}^{+} \& \mathrm{NH}_{3} \) \((b) \mathrm{CO}_{3}^{2-} \& \mathrm{HCO}_{3}^{-}\)

The rate of a reaction is affected by the following factors.
(i) Nature and state of the reactant
(ii) Concentration of the reactant
(iii) Surface area of the reactant
(iv) Temperature of the reaction
(v) Presence of a catalyst

(i) The two O-O bond lengths are identical due to resonance.
(ii) Due to the strong bond formation with other elements.

The preliminary step in metallurgical process is removal of the impurities. This removal process is known as concentration of ore.

Diammine silver (I) Chloride.

(i) Let A = 100M, [A₀] - [A] = 20M,
For the zero order reaction
\(k=\left( \frac { \left[ { A }_{ 0 } \right] -\left[ A \right] }{ t } \right) \)
(i) 20% completion  \(k=\left( \frac { 20M }{ 20min } \right) \) = 1 mol L^-1 min^-1 
(ii) 80% completion
\(\mathrm{K}=1 \mathrm{~mol} \mathrm{~L}{ }^{-1} \mathrm{~s}^{-1} ;\left[\mathrm{A}_{0}\right]=100 \mathrm{M} ;\left[\mathrm{A}_{0}\right]-[\mathrm{A}]=80 \mathrm{M} ; \mathrm{t}=?\)
\(\therefore t=\left(\frac{\left[A_{O}\right]-[A]}{K}\right)=\frac{80}{1}=80 \mathrm{mins}\)

(i) Zeolites are three-dimensional crystalline solids containing Al, Si and O in their regular three dimensional framework.
(ii) They are hydrated sodium alumino silicates with general formula Na₂O(AI₂O₃).·x(SiO₂)·yH₂O
(x = 2 to 10; y = 2 to 6).
(iii) Zeolites have porous structure in which the monovalent sodium ions and water molecules are loosely held.
(iv) The Si and Al atoms are tetrahedrally coordinated with each other through shared oxygen atoms.
(v) Zeolites are similar to clay minerals but they differ in their crystalline structure.
(vi) Zeolites have a three dimensional crystalline structure looks like a honeycomb consisting of a network of interconnected tunnels and cages.
(vii) Water molecules moves freely in and out of these pores but the zeolite framework remains rigid
(viii) Another special aspect of this structure is that the pore/channel sizes are nearly uniform, allowing the crystal to act as a molecular sieve.

(i) (A) on oxidation with air and V₂O₅ gives (B).
\(\underset{(A)}{{ C }_{ 6 }{ H }_{ 5 }{ CH }_{ 3 }}\overset { \left( O \right) }{ \underset { { V }_{ 2 }{ O }_{ 5 } }{ \longrightarrow } } \underset{(B)}{{ C }_{ 6 }{ H }_{ 5 }CHO}\) 
(ii) (B) on reduction with LiAIH₄ gives C.
\({ C }_{ 6 }{ H }_{ 5 }CH\overset { \left[ H \right] }{ \underset { LiA/{ H }_{ 4 } }{ \longrightarrow } } \underset{(C)}{{ C }_{ 6 }{ H }_{ 5 }CHO}\)

(i) Effective and efficient conversion is the special characteristic of enzyme catalysed reactions. An enzyme may transform a million molecules of reactant in a minute 
For Eg: \({ 2H }_{ 2 }{ O }_{ 2 }\longrightarrow { 2H }_{ 2 }O+{ O }_{ 2 }\)
For this reaction, the activation energy is 18k cal/mole without a catalyst  With colloidal platinum as a, catalyst the activation energy is 11.7kcal /mole. But with the enzyme catalyst the activation energy of this reaction is less than 2kcal/ mole.
(ii) Enzyme catalysis is highly specific in nature.
(iii) Enzyme catalysed reaction has maximum rate at optimum temperature
(iv) The rate of enzyme catalysed reactions varies with the pH of the system. The rate is maximum at a pH called optimum pH.
(v) Enzymes can be inhibited i.e. poisoned activity of an enzyme is decreased and destroyed by a poison. The physiological action of drugs is related to their inhibiting action.
(vi) Catalytic activity of enzymes is increased by coenzymes or activators.

The heavier transition elements belong to fourth (4d), fifth (Sd) and sixth (6d) transition series. Their properties are expected to be different form the elements belonging to the first (3d) series due to the following reasons.
(i) Atomic radii: Size of the transition elements 94d and Sd series are larger than those of the corresponding elements of the first transition series though those of 4d and Sd series are very close to each other.
(ii) Ionisation enthalpy of Sd series are higher than the corresponding elements of 3d and 4d series.
(iii) Atomisation enthalpy of 4d and Sd series are higher than the corresponding elements of the first series.
(iv) Melting and boiling points of heavier transition elements are greater than those of the first transition series due to stronger intermetallic bonding.
(v) The elements of the first transition series generally form low or high spin complexes, depending upon the higher of ligand field. However, the heavier transition elements form low spin complexes irrespective of the strength of the ligand filed.

(i) When a solution of brine (NaCl) is electrolysed, Na⁺ and Cl ions are formed.
(ii) Na⁺ ion reacts with OH^- ions of water and forms sodium hydroxide. Hydrogen and chlorine are liberated as gases.
NaCI \(\longrightarrow \) Na⁺ + CI^-1
H₂O \(\longrightarrow \) H⁺ + OH^-
Na⁺ + OH^- \(\longrightarrow \) NaOH
At the cathode,
H⁺ + e^- \(\longrightarrow \) H
H + H\(\longrightarrow \)H₂
At the anode,
Cl^- \(\longrightarrow \) CI + e^-
CI + CI \(\longrightarrow \) Cl₂

Crystal defects are classified as follows
(i) Point defects
(ii) Line defects
(iii) Interstitial defects
(iv) Volume defects
Point defects are further classified as follows

The stability of a complex or co-ordination compound refers to the extent up to which it exists in a solution as co-ordination sphere.
(i) Change on the central metal ion: Greater the charge on the central metal ion, greater the stability of complex.
(ii) Nature of the metal ion: Group 3 and 6 and inner transition elements form stable complexes when donor atoms of the ligands are N, O and F. The elements after group 6 of the transition metals form stable complex when the donor atoms of the ligands are the heavier members of N, O and F family.
(iii) Basic nature of the ligands: Greater the basic strength, greater is the stability of the complex.
(iv) Presence of chelate rings: Its presence increases the stability of the complex. it is called chelate effect. It is maximum for the 5 and 6 membered rings.
(v) Effect of multidentate cyclic ligand: If the ligands are IT multidentate and cyclic without any steric effect the stability of the complex get increased.