Match the ions given in Column I with their nature given in Column II. (More than one correlation is possible.

NCERT Exemplar · Q54

Q. Match the ions given in Column I with their nature given in Column II. (More than one correlation is possible.) Column I

(i) CH3—O—CH^+—CH3 (oxygen bears lone pairs)

(ii) F3C^+

(iii) (CH3)3C^-

(iv) CH3—CH^+—CH3
Column II

(a) Stable due to resonance

(b) Destabilised due to inductive effect

(d) A secondary carbocation

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Concept understanding — Inductive Effect

Inductive Effect on Acidity – From Intuition to Precision

Imagine you are holding a rope tied to a heavy box. If you pull the rope, the box moves toward you. Now imagine the rope is made of rubber bands — the pull still reaches the box, but it gets weaker the farther away you are. That is exactly how the inductive effect works inside a molecule.

The Core Intuition

An acid donates a proton ( $H^+$ ). After it does, the remaining part (the conjugate base) carries a negative charge. The stability of that negative charge determines how willing the molecule is to give up the proton. More stable conjugate base → stronger acid.

Now, some atoms or groups are electron-withdrawing — they pull electron density toward themselves through the sigma bonds. If such a group is attached near the acidic proton, it pulls some electron density away from the negative charge on the conjugate base. That spreads out (delocalises) the negative charge, making the conjugate base more stable. The acid becomes stronger.

Conversely, electron-donating groups push electron density toward the negative charge, concentrating it and making the conjugate base less stable. The acid becomes weaker.

Note

The inductive effect operates through sigma bonds only. It does not involve pi bonds or resonance. It is a permanent, through-bond polarisation.

The Precise Statement

Inductive effect on acidity: The acidity of a compound increases with the presence of electron-withdrawing groups (EWGs) near the acidic site, and decreases with electron-donating groups (EDGs). The effect is strongest when the group is closest to the acidic proton, and diminishes rapidly with distance.

Mathematically, for a series of substituted carboxylic acids:

\text{R-COOH} \quad \text{where R = substituent}

The acid dissociation constant $K_a$ changes as:

If R is electron-withdrawing (e.g., $-\text{Cl}$ , $-\text{NO}_2$ , $-\text{CF}_3$ ): $K_a$ increases → stronger acid.
If R is electron-donating (e.g., $-\text{CH}_3$ , $-\text{C}_2\text{H}_5$ ): $K_a$ decreases → weaker acid.

Why Distance Matters

The inductive effect falls off with distance because sigma bonds are localised. Each bond attenuates the effect by roughly a factor of 2–3. For example, compare:

Compound	$pK_a$	Explanation
$\text{CH}_3\text{COOH}$	4.76	Reference (no EWG)
$\text{ClCH}_2\text{COOH}$	2.86	Cl withdraws through one bond
$\text{Cl}_2\text{CHCOOH}$	1.29	Two Cl atoms, stronger withdrawal
$\text{Cl}_3\text{CCOOH}$	0.65	Three Cl atoms, strongest withdrawal
$\text{CH}_3\text{CH}_2\text{COOH}$	4.87	Ethyl group is electron-donating (slightly weaker acid)

Notice: $\text{ClCH}_2\text{COOH}$ is about 100 times stronger than acetic acid ( $\Delta pK_a \approx 1.9$ ). But if the Cl is moved further away:

Compound	$pK_a$
$\text{ClCH}_2\text{CH}_2\text{COOH}$	4.08
$\text{ClCH}_2\text{CH}_2\text{CH}_2\text{COOH}$	4.52

The effect fades as the chlorine moves farther from the carboxyl group. …

Why this formula?

Inductive Effect: Why the Key Ideas Hold

The inductive effect is a fundamental concept in organic chemistry that explains how electron density shifts along a sigma ( $\sigma$ ) bond due to differences in electronegativity. Let's break down why the key principles work — not just what they are.

1. The Core Idea: Polarization of $\sigma$ Bonds

What happens?

When two atoms with different electronegativities form a $\sigma$ bond, the bonding electrons are not shared equally. The more electronegative atom pulls electron density toward itself.

Why does this happen?

Electronegativity is a measure of an atom's ability to attract shared electrons.
The $\sigma$ bond is a region of high electron density between the nuclei.
The more electronegative atom's nucleus exerts a stronger electrostatic pull on these electrons.
Result: The bond becomes polarized — one end becomes slightly negative ( $\delta^-$ ), the other slightly positive ( $\delta^+$ ).

Key formula (conceptual):

$\delta^- \leftarrow \text{Atom A} \rightarrow \delta^+$

where A is more electronegative than B.

2. Why the Effect Transmits Along a Chain

The puzzle:

If the inductive effect is about a single bond, how does it affect atoms several bonds away?

The reasoning:

The $\delta^+$ on the less electronegative atom creates a partial positive charge.
This partial charge polarizes the next $\sigma$ bond in the chain.
The effect is relayed through successive bonds, like a chain of dominoes.

Why does it weaken with distance?

Each bond acts as a dielectric medium — it partially screens the charge.
The electrostatic influence falls off with distance according to Coulomb's law:

F \propto \frac{q_1 q_2}{r^2}

In a molecular chain, the effective distance $r$ increases, so the induced dipole in each subsequent bond is smaller.

Key result: Inductive effect is significant only up to 3–4 bonds away.

3. The Quantitative Measure: Inductive Effect Constant ( $\sigma_I$ )

What is $\sigma_I$ ?

It's a Hammett-type constant that quantifies the electron-withdrawing or electron-donating power of a substituent through sigma bonds only.

Why does it have this form?

The inductive effect is additive — each substituent contributes independently.
For a substituent X attached to a carbon chain:

\sigma_I = \log \left( \frac{K_a(\text{X-CH}_2\text{COOH})}{K_a(\text{CH}_3\text{COOH})} \right)

where $K_a$ is the acid dissociation constant.

Why use acid dissociation?

The carboxyl group ( $-\text{COOH}$ ) is a sensitive probe.
An electron-withdrawing group (EWG) stabilizes the conjugate base ( $\text{R-COO}^-$ ) by dispersing its negative charge.
This increases $K_a$ (stronger acid).
An electron-donating group (EDG) destabilizes the conjugate base, decreasing $K_a$ .

Key formula:

$\sigma_I > 0$ for EWGs (e.g., $-\text{Cl}$ , $-\text{NO}_2$ )

$\sigma_I < 0$ for EDGs (e.g., $-\text{CH}_3$ , $-\text{C(CH}_3)_3$ )

4. Why Inductive Effect is Not Resonance

Common confusion:

Students often mix inductive and resonance effects.

The critical difference:

Property	Inductive Effect	Resonance Effect
Electron movement	Through $\sigma$ bonds only	Through $\pi$ bonds or lone pairs
Distance dependence	Dies off after 3–4 bonds	Can transmit over long distances in conjugated systems
Permanent or temporary	Permanent polarization	Can be temporary (delocalization)

Why this matters for exam problems:

In alkyl halides, the inductive effect of $-\text{Cl}$ explains the $\delta^+$ on carbon.
In benzene derivatives, the combined inductive and resonance effects determine reactivity.

--- …

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Stability of carbocations and carbanions depends on electron donation (hyperconjugation, resonance) or withdrawal (inductive effect). The matches are: (i)→a,c;

(ii)→b;

(iii)→b;

(iv)→c,d.

Carbocations are electron-deficient and stabilised by electron-donating effects; carbanions are electron-rich and destabilised by electron-withdrawing groups. The two key stabilising mechanisms for carbocations are resonance (delocalisation of charge over multiple atoms) and hyperconjugation (donation from adjacent C–H or C–C σ-bonds). The inductive effect describes electron withdrawal or donation through σ-bonds: electron-withdrawing groups (like F) destabilise both cations and anions by pulling electron density away.

Let's analyze each ion systematically.

1. $\ce{CH3-O-CH^+-CH3}$ (oxygen with lone pairs)

This is a carbocation adjacent to oxygen. Oxygen's lone pairs can delocalise into the empty p-orbital on the positively charged carbon, creating resonance structures:

\ce{CH3-O^+-=CH-CH3 <-> CH3-O-CH^+-CH3}

The positive charge is shared between oxygen and carbon, spreading the charge over multiple atoms and lowering the energy significantly. This is resonance stabilisation (a).

Additionally, the C–H bonds on the methyl groups can participate in hyperconjugation with the empty p-orbital, though this is a weaker effect compared to the resonance with oxygen's lone pairs. Still, it contributes to stability (c).

Tip

Whenever a carbocation is adjacent to an atom with lone pairs (O, N, halogens), always check for resonance first—it's usually the dominant stabilising effect.

2. $\ce{F3C^+}$

This carbocation has three highly electronegative fluorine atoms directly attached to the positively charged carbon. Fluorine withdraws electron density through the inductive effect (−I effect), pulling electrons away from an already electron-deficient centre. This makes the carbocation extremely unstable—in fact, $\ce{CF3^+}$ is one of the least stable carbocations known.

The fluorines have lone pairs, but these are in orbitals (2p on F) that overlap very poorly with the empty 2p orbital on carbon due to the large electronegativity difference and size mismatch. Any resonance stabilisation is negligible compared to the strong destabilising inductive effect.

This ion is destabilised by inductive effect (b).

3. $\ce{(CH3)3C^-}$

This is a tertiary carbanion. Carbanions are electron-rich species (they have an extra electron pair). Alkyl groups are electron-donating through the inductive effect (+I effect), which pushes more electron density onto an already negative centre. This increases electron-electron repulsion and destabilises the carbanion. …

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Q.Match the ions given in Column I with their nature given in Column II. (More than one correlation is possible.)
Column I

Concept understanding — Inductive Effect

Inductive Effect on Acidity – From Intuition to Precision

The Core Intuition

The Precise Statement

Why Distance Matters

Why this formula?

Inductive Effect: Why the Key Ideas Hold

1. The Core Idea: Polarization of $\sigma$ Bonds

What happens?

Why does this happen?

2. Why the Effect Transmits Along a Chain

The puzzle:

The reasoning:

Why does it weaken with distance?

3. The Quantitative Measure: Inductive Effect Constant ( $\sigma_I$ )

What is $\sigma_I$ ?

Why does it have this form?

Why use acid dissociation?

4. Why Inductive Effect is Not Resonance

Common confusion:

The critical difference:

Why this matters for exam problems:

Matching Carbocations and Carbanions with Their Stability Factors

1. $\ce{CH3-O-CH^+-CH3}$ (oxygen with lone pairs)

2. $\ce{F3C^+}$

3. $\ce{(CH3)3C^-}$

Q.Match the ions given in Column I with their nature given in Column II. (More than one correlation is possible.) Column I

1. CHX3−O−CHX+−CHX3\ce{CH3-O-CH^+-CH3}CHX3​−O−CHX+−CHX3​ (oxygen with lone pairs)

2. FX3CX+\ce{F3C^+}FX3​CX+

3. (CHX3)X3CX−\ce{(CH3)3C^-}(CHX3​)X3​CX−

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Q.Match the ions given in Column I with their nature given in Column II. (More than one correlation is possible.)
Column I

1. $\ce{CH3-O-CH^+-CH3}$ (oxygen with lone pairs)

2. $\ce{F3C^+}$

3. $\ce{(CH3)3C^-}$

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