---
title: "Electronic Effects and Reactive Intermediates"
book: "University Chemistry — Year 1"
subject: chemistry
language: en
chapter: 18
exercises: 12
source: https://one-course.com/books/chemistry/2/en/chapter/18-electronic-effects-and-reactive-intermediates
license: CC-BY-NC-SA-4.0
credit: "One Chemistry Book, One Course (one-course.com)"
---

# Chapter 18 — Electronic Effects and Reactive Intermediates

Trifluoroethanoic acid, $\ce{CF3COOH}$, is about ten thousand times stronger an acid than ethanoic acid, $\ce{CH3COOH}$, although the acidic O–H bond is three bonds away from the fluorine atoms. Phenol is a million times more acidic than ethanol, and an ammonia molecule bound to a benzene ring — aniline — is a million times less basic than one bound to a methyl group. Organic chemistry is full of such contrasts, and two effects explain most of them: the pull of electronegative atoms along the $\sigma$ bonds, and the spreading of electron pairs over $\pi$ systems. The same two effects decide which bonds break, which intermediates form and where reagents attack: they are the grammar of the [reaction mechanisms](https://one-course.com/books/chemistry/2/en/chapter/9-reaction-mechanisms-elementary-steps-and-approximations#def-b1-elementary-steps-elementary-step) of the next chapters.

**You already know.**

[Electronegativity](https://one-course.com/books/chemistry/2/en/chapter/2-periodicity#def-b1-periodicity-electronegativity) and its trends ([Chapter 2](https://one-course.com/books/chemistry/2/en/chapter/2-periodicity#ch-b1-periodicity)); [Lewis structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis), [formal charges](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-formal-charge) and resonance ([Chapter 3](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#ch-b1-lewis-resonance-vsepr)); $\mathrm{p}K_a$ and the strength of acids and bases ([Chapter 10](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#ch-b1-predominant-reaction)). The school volume (grade 12) drew [curly arrows](#def-b1-electronic-effects-curly-arrow) from a [nucleophile](#def-b1-electronic-effects-nucleophile) to an [electrophile](#def-b1-electronic-effects-nucleophile).

## 18.1 Inductive effects

**Definition 18.1 (Inductive effect).**

The *inductive effect* is the shift of electron density along $\sigma$ bonds towards an electronegative atom or group. An attracting group (F, Cl, O, $\ce{NO2}$, $\ce{CF3}$) has a $-I$ effect; alkyl groups and negatively charged atoms push electrons, a $+I$ effect. The effect weakens quickly with the number of bonds in between.

**Proposition 18.2 (Inductive effect and acidity).**

An attracting group near the acidic site of a carboxylic acid stabilises the carboxylate ion by spreading its negative charge, and lowers the $\mathrm{p}K_a$: the more attracting groups, the closer, the stronger the acid.

**Proof.** $\mathrm{p}K_a$ measures the position of $\mathrm{RCOOH} \rightleftharpoons
\mathrm{RCOO^-} + \ce{H+}$. A group that draws electron density away from the carboxylate spreads its charge over more atoms, which lowers its energy more than that of the neutral acid; the equilibrium moves to the right and $K_a$ increases. The measured series confirms it. ∎

![The halogenated ethanoic acids. Each chlorine lowers the pK_a; with three, the acid is about ten thousand times stronger than ethanoic acid. Trifluoro- and trichloroethanoic acids are equally strong within the uncertainty of measurements on such strong acids.](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-236f1a9ce5f5.svg)

*The halogenated ethanoic acids. Each chlorine lowers the $\mathrm{p}K_a$; with three, the acid is about ten thousand times stronger than ethanoic acid. Trifluoro- and trichloroethanoic acids are equally strong within the uncertainty of measurements on such [strong acids](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid).*

Alkyl groups work the other way, a little: propanoic acid ($\mathrm{p}K_a
= 4.89$) is slightly weaker than ethanoic acid (4.76), and methanoic acid (3.74), with no alkyl group, is stronger than both.

## 18.2 Mesomeric effects

When an atom bearing a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis), or a charge, is bound to a $\pi$ system, its electrons can be shared with that system; [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) ([Chapter 3](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#ch-b1-lewis-resonance-vsepr)) describe the sharing.

**Definition 18.3 (Mesomeric effect, donor and acceptor groups).**

The *mesomeric effect* is the shift of electron density through a conjugated $\pi$ system, shown by [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance). A *donor group* gives a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) to the system, a $+M$ effect ($\ce{-OH}$, $\ce{-O^-}$, $\ce{-NH2}$, $\ce{-OR}$); an *acceptor group* draws electrons from it through a $\pi$ bond to an electronegative atom, a $-M$ effect ($\ce{-NO2}$, $\ce{-C=O}$, $\ce{-C#N}$).

![Resonance structures of the ethanoate ion (the charge shared by two equivalent oxygens), of the phenoxide ion (the charge spread into the ring; one of the three ring structures shown), and of an amide (the nitrogen lone pair shared with the C=O, which makes amides poor bases).](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-834f7dd77379.svg)

![Resonance structures of the ethanoate ion (the charge shared by two equivalent oxygens), of the phenoxide ion (the charge spread into the ring; one of the three ring structures shown), and of an amide (the nitrogen lone pair shared with the C=O, which makes amides poor bases).](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-dcd5c802548d.svg)

![Resonance structures of the ethanoate ion (the charge shared by two equivalent oxygens), of the phenoxide ion (the charge spread into the ring; one of the three ring structures shown), and of an amide (the nitrogen lone pair shared with the C=O, which makes amides poor bases).](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-17a40bb89020.svg)

*[Resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) of the ethanoate ion (the charge shared by two equivalent oxygens), of the phenoxide ion (the charge spread into the ring; one of the three ring structures shown), and of an amide (the nitrogen [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) shared with the C=O, which makes amides poor bases).*

**Proposition 18.4 (Mesomeric effect and acidity).**

An acid whose conjugate base spreads its charge by resonance is stronger than one whose base cannot: carboxylic acids ($\mathrm{p}K_a$ about 4–5) are far stronger than alcohols (about 16), and phenol (10.0) lies between. An [acceptor group](#def-b1-electronic-effects-mesomeric) in the position *ortho* or *para* to the OH of a phenol strengthens it more than in the position *meta*.

**Proof.** In an alkoxide the charge sits on one oxygen; in a carboxylate it is shared by two oxygens; in a phenoxide it is shared by the oxygen and three ring carbons, less electronegative than oxygen, a smaller gain. A $\ce{NO2}$ group at the *ortho* or *para* carbon can take the charge itself through a [resonance structure](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) with $\ce{C=N+(-O^-)-O^-}$; at *meta*, no [resonance structure](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) brings the charge onto the carbon that carries $\ce{NO2}$, and only the [inductive effect](#def-b1-electronic-effects-inductive) remains. The measured values: 2-nitrophenol 7.23, 4-nitrophenol 7.16, 3-nitrophenol 8.36, against 9.99 for phenol and 15.9 for ethanol. ∎

The same reasoning applies to bases. Methylamine ($\mathrm{p}K_a$ of its ammonium 10.66) is a stronger base than ammonia (9.25, [Chapter 10](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#ch-b1-predominant-reaction)), the methyl group pushing electrons onto nitrogen; in aniline the [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) is shared with the ring and the ammonium is far more acidic (4.60). Pyridine (5.23) keeps its [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis), but on a nitrogen held in a planar ring with more *s* character, less available than in an amine.

## 18.3 Breaking a bond: reactive intermediates

**Definition 18.5 (Homolysis and heterolysis).**

A [covalent bond](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) breaks by *homolysis* when each atom keeps one of the two bonding electrons, giving two [radicals](#def-b1-electronic-effects-intermediates), and by *heterolysis* when one atom keeps both, giving a cation and an anion.

**Definition 18.6 (Reactive intermediates).**

A *reactive intermediate* is a species formed in one step of a mechanism and consumed in a later one, too reactive to accumulate ([Chapter 9](https://one-course.com/books/chemistry/2/en/chapter/9-reaction-mechanisms-elementary-steps-and-approximations#ch-b1-elementary-steps)). A *carbocation* has a carbon with three bonds and a positive charge (six [valence electrons](https://one-course.com/books/chemistry/2/en/chapter/1-quantum-numbers-and-electron-configurations#def-b1-quantum-numbers-configuration)); a *carbanion* a carbon with three bonds, a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) and a negative charge; a *radical* an atom with an [unpaired electron](https://one-course.com/books/chemistry/2/en/chapter/1-quantum-numbers-and-electron-configurations#def-b1-quantum-numbers-unpaired).

**Definition 18.7 (Class of a carbon).**

A carbon bound to one other carbon is a *primary carbon*, to two a *secondary carbon*, to three a *tertiary carbon*. A [carbocation](#def-b1-electronic-effects-intermediates), a [radical](#def-b1-electronic-effects-intermediates) or a halogenoalkane takes the class of the carbon concerned.

![Geometries of the three reactive intermediates of carbon (R: H or an alkyl group). The flat carbocation can be attacked on either face, a point that matters for the stereochemistry of .](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-bd3d00e31753.svg)

*Geometries of the three [reactive intermediates](#def-b1-electronic-effects-intermediates) of carbon (R: H or an alkyl group). The flat [carbocation](#def-b1-electronic-effects-intermediates) can be attacked on either face, a point that matters for the stereochemistry of [Chapter 19](https://one-course.com/books/chemistry/2/en/chapter/19-nucleophilic-substitution#ch-b1-nucleophilic-substitution).*

**Proposition 18.8 (Stability of carbocations).**

[Carbocations](#def-b1-electronic-effects-intermediates) are stabilised by groups that give them electrons: tertiary $>$ secondary $>$ primary $>$ methyl; a [carbocation](#def-b1-electronic-effects-intermediates) next to a double bond (allylic) or a benzene ring (benzylic) is further stabilised by resonance, and one next to an atom with a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) ($\ce{R-O-CH2+}$) even more.

**Proof.** Each alkyl group pushes electron density towards the electron-poor carbon ($+I$ effect, and a related interaction of its C–H bonds with the empty orbital, described in the Year 2 volume). An allylic cation has two [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) putting the charge on either end carbon; a benzylic cation has four, three in the ring; an oxygen [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) forms a fourth bond to the cationic carbon, $\ce{R-O+=CH2}$, in which every atom has an octet. ∎

[Carbanions](#def-b1-electronic-effects-intermediates) follow the opposite order (methyl $>$ primary $>$ secondary $>$ tertiary) and are stabilised by [acceptor groups](#def-b1-electronic-effects-mesomeric); [radicals](#def-b1-electronic-effects-intermediates) follow the same order as [carbocations](#def-b1-electronic-effects-intermediates), less markedly.

## 18.4 Curly arrows, nucleophiles and electrophiles

**Definition 18.9 (Curly arrows).**

In a mechanism, a *curly arrow* shows the movement of an electron pair: it starts on a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) or a bond and ends on an atom (where a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) or a new bond forms) or between two atoms (a new bond). A *half-headed arrow* shows the movement of a single electron, in [radical](#def-b1-electronic-effects-intermediates) reactions.

**Method 18.10 (Drawing curly arrows).**

1. Start from electrons: a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) , a $\pi$ bond or a $\sigma$ bond, never from a positive charge or an atom without electrons.
2. End where the pair goes: a new bond between the two atoms, or a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) on the more electronegative atom when a bond breaks.
3. Count charges after each step: the atom giving a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) to a new bond gains $+1$ , the atom receiving a pair as a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) gains $-1$ ; the total charge is conserved.
4. Never exceed an octet on C, N, O: when a pair arrives, another must leave.

![Curly arrows. Top: heterolysis of the C–Br bond, the pair going to bromine. Bottom: a proton transfer from water to hydroxide, written as the attack of a lone pair of the base on the hydrogen (the bond O–H of water then breaks, its pair staying on oxygen; the second arrow is left for ).](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-db1d977ceaa3.svg)

![Curly arrows. Top: heterolysis of the C–Br bond, the pair going to bromine. Bottom: a proton transfer from water to hydroxide, written as the attack of a lone pair of the base on the hydrogen (the bond O–H of water then breaks, its pair staying on oxygen; the second arrow is left for ).](https://one-course.com/images/onecourse/chapters/chemistry-2/b1-electronic-effects/fig-c34c68302d4b.svg)

*[Curly arrows](#def-b1-electronic-effects-curly-arrow). Top: [heterolysis](#def-b1-electronic-effects-cleavage) of the C–Br bond, the pair going to bromine. Bottom: a proton transfer from water to hydroxide, written as the attack of a [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) of the base on the hydrogen (the bond O–H of water then breaks, its pair staying on oxygen; the second arrow is left for [Exercise 18.4](#exo-b1-electronic-effects-4)).*

**Definition 18.11 (Nucleophile, electrophile, leaving group).**

A *nucleophile* is a species that gives an electron pair to an atom other than hydrogen to form a bond (a [Lewis base](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis-acid)); an *electrophile* is a species that accepts such a pair (a [Lewis acid](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis-acid), often a carbon bearing a partial positive charge). The *nucleophilicity* of a species is its reactivity as a nucleophile, measured by [rate constants](https://one-course.com/books/chemistry/2/en/chapter/8-chemical-kinetics-rate-laws#def-b1-rate-laws-order). A *leaving group* is the group that departs with the [bonding pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) when a bond to carbon breaks heterolytically.

**Proposition 18.12 (Nucleophilicity and basicity).**

For [nucleophiles](#def-b1-electronic-effects-nucleophile) that attack through the same atom, [nucleophilicity](#def-b1-electronic-effects-nucleophile) follows basicity: $\ce{CH3O-}$ $>$ $\ce{OH-}$ $>$ $\ce{CH3COO-}$ $>$ $\ce{H2O}$. It fails across a column of the periodic table in [protic solvents](https://one-course.com/books/chemistry/2/en/chapter/4-intermolecular-forces-and-solvents#def-b1-intermolecular-forces-solvents-solvent-classes), where large, polarisable, weakly solvated [nucleophiles](#def-b1-electronic-effects-nucleophile) react faster although they are weaker bases ($\ce{I-}$ $>$ $\ce{Br-}$ $>$ $\ce{Cl-}$ $>$ $\ce{F-}$), and for bulky bases, which are poor [nucleophiles](#def-b1-electronic-effects-nucleophile).

**Proof.** Basicity measures the equilibrium of the attack on a proton, [nucleophilicity](#def-b1-electronic-effects-nucleophile) the rate of attack on a carbon; both increase with the availability of the electron pair, hence the parallel within one atom. The rate also depends on the energy needed to strip the solvent from the [nucleophile](#def-b1-electronic-effects-nucleophile) and on the distortion of its electron cloud towards a crowded carbon: small anions such as $\ce{F-}$ are strongly bound to [protic solvent](https://one-course.com/books/chemistry/2/en/chapter/4-intermolecular-forces-and-solvents#def-b1-intermolecular-forces-solvents-solvent-classes) molecules ([Chapter 4](https://one-course.com/books/chemistry/2/en/chapter/4-intermolecular-forces-and-solvents#ch-b1-intermolecular-forces-solvents)), and bulky groups hinder the approach to carbon but not to a proton. ∎

A good [leaving group](#def-b1-electronic-effects-nucleophile) is a [weak base](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid), stable once it carries the pair: $\ce{I-}$, $\ce{Br-}$, $\ce{Cl-}$, water, sulfonates; $\ce{OH-}$ and $\ce{RO-}$, [strong bases](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid), are poor [leaving groups](#def-b1-electronic-effects-nucleophile) — the reason why alcohols must be activated before substitution ([Chapter 22](https://one-course.com/books/chemistry/2/en/chapter/22-alcohols-activating-the-oh-group#ch-b1-alcohol-activation)).

## 18.5 Exercises

**Exercise 18.1 ★.**

Classify each carbon of 2-methylbutane and of 2-bromo-2-methylpropane as primary, secondary, tertiary or quaternary (bound to four carbons). Which [carbocation](#def-b1-electronic-effects-intermediates) forms most easily from each bromide of formula $\ce{C4H9Br}$?

**Solution of Exercise 18.1.**

2-Methylbutane, $\ce{CH3-CH(CH3)-CH2-CH3}$: the three $\ce{CH3}$ are primary, the $\ce{CH2}$ secondary, the CH tertiary. 2-Bromo-2-methylpropane: the three $\ce{CH3}$ are primary, the central carbon tertiary. Of the four bromides $\ce{C4H9Br}$ (1-bromobutane, 2-bromobutane, 1-bromo-2-methylpropane, 2-bromo-2-methylpropane), the last gives the tertiary [carbocation](#def-b1-electronic-effects-intermediates), the most stable.

**Exercise 18.2 ★.**

From the $\mathrm{p}K_a$ values, compute the ratio of the [acidity constants](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-acidity-constant) of chloroethanoic and ethanoic acids, and of trifluoroethanoic and ethanoic acids.

**Solution of Exercise 18.2.**

$10^{4.76 - 2.87} = 10^{1.89} = 78$; $10^{4.76 - 0.52} = 10^{4.24} =
1.7 \times 10^{4}$.

**Exercise 18.3 ★.**

Draw the [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) of the ethanoate ion, of the 4-nitrophenoxide ion (with the charge on an oxygen of the nitro group) and of the allyl cation $\ce{CH2=CH-CH2+}$.

**Solution of Exercise 18.3.**

Ethanoate: the C=O and $\ce{C-O^-}$ exchanged between the two oxygens. 4-Nitrophenoxide: the oxygen [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) forms a C=O, the ring double bonds shift, the carbon bearing $\ce{NO2}$ forms a C=N bond, and an N=O pair goes to oxygen: a structure with C=O at one end of the ring, C=N at the other and both nitro oxygens negative (a quinoid structure). Allyl cation: $\ce{CH2=CH-CH2+}$ $\leftrightarrow$ $\ce{+CH2-CH=CH2}$.

**Exercise 18.4 ★.**

Complete the [curly arrows](#def-b1-electronic-effects-curly-arrow) of the proton transfer of the figure and of $\ce{NH3 + H3O+ -> NH4+ + H2O}$. Check the charges.

**Solution of Exercise 18.4.**

Second arrow: from the O–H bond of water to its oxygen; products $\ce{H2O}$ (from $\ce{OH-}$, now neutral) and $\ce{OH-}$ (the oxygen of the former water keeps the pair, charge $-1$). For ammonia: an arrow from the N [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) to an H of $\ce{H3O+}$, and one from that O–H bond to the oxygen: N becomes $+1$, O becomes 0.

**Exercise 18.5 ★★.**

Rank by increasing acidity: ethanol, phenol, ethanoic acid, 4-nitrophenol, trichloroethanoic acid, water ($\mathrm{p}K_a$ of the couple $\ce{H2O}$/$\ce{OH-}$, 14.0). Justify each step with an inductive or mesomeric argument.

**Solution of Exercise 18.5.**

Ethanol (15.9) $<$ water (14.0) $<$ phenol (9.99, ring delocalisation) $<$ 4-nitrophenol (7.16, $\ce{NO2}$ takes the charge) $<$ ethanoic acid (4.76, two equivalent oxygens) $<$ trichloroethanoic acid (0.51, three $-I$ chlorines).

**Exercise 18.6 ★★.**

Rank by increasing basicity: aniline, methylamine, ammonia, pyridine. Explain the position of aniline with a [resonance structure](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance).

**Solution of Exercise 18.6.**

Aniline (4.60) $<$ pyridine (5.23) $<$ ammonia (9.25) $<$ methylamine (10.66). In aniline the [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) is shared with the ring (structures with C=N$^+$ and the negative charge *ortho* and *para*); protonating N would cost that delocalisation.

**Exercise 18.7 ★★.**

Why is 3-nitrophenol weaker than 4-nitrophenol but still stronger than phenol? Draw the [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) that justify both statements.

**Solution of Exercise 18.7.**

In 3-nitrophenoxide, the [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) place the charge on the carbons *ortho* and *para* to the oxygen, never on the carbon bearing $\ce{NO2}$: no mesomeric help, hence weaker than the 4-isomer. The nitro group still pulls electrons through the $\sigma$ bonds ($-I$), hence stronger than phenol.

**Exercise 18.8 ★★.**

Rank the [carbocations](#def-b1-electronic-effects-intermediates) $\ce{CH3+}$, $\ce{(CH3)3C+}$, $\ce{CH2=CH-CH2+}$, $\ce{CH3CH2+}$, $\ce{C6H5CH2+}$, $\ce{CH3OCH2+}$, and justify.

**Solution of Exercise 18.8.**

$\ce{CH3+}$ $<$ $\ce{CH3CH2+}$ $<$ $\ce{CH2=CH-CH2+}$ $<$ $\ce{C6H5CH2+}$ $\approx$ $\ce{(CH3)3C+}$ $<$ $\ce{CH3OCH2+}$: alkyl groups give electrons; allyl and benzyl delocalise the charge (two and four structures); the oxygen [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) gives a structure with a full octet everywhere. The order in the middle of the list depends on the medium.

**Exercise 18.9 ★★.**

Identify the [nucleophile](#def-b1-electronic-effects-nucleophile) and the [electrophile](#def-b1-electronic-effects-nucleophile) in: $\ce{CH3Br + OH-}$; $\ce{H2O + H+}$; ethanal with a cyanide ion; $\ce{BF3 + NH3}$. Draw the [curly arrows](#def-b1-electronic-effects-curly-arrow).

**Solution of Exercise 18.9.**

$\ce{OH-}$ ([nucleophile](#def-b1-electronic-effects-nucleophile)) attacks the carbon of $\ce{CH3Br}$ ([electrophile](#def-b1-electronic-effects-nucleophile)), the C–Br pair leaving on Br. $\ce{H2O}$ gives a pair to $\ce{H+}$ (here acid and base are the names used). $\ce{CN-}$ attacks the carbonyl carbon of ethanal, the C=O $\pi$ pair moving to oxygen. $\ce{NH3}$ gives its [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) to the empty orbital of boron in $\ce{BF3}$.

**Exercise 18.10 ★★★.**

A solution contains $0.010\,\mathrm{mol}/\mathrm{L}$ of trichloroethanoic acid. Is the weak-acid formula $\mathrm{pH} = \frac12(\mathrm{p}K_a - \log C)$ valid? Compute the pH properly and the [degree of dissociation](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-dissociation).

**Solution of Exercise 18.10.**

No: $K_a = 10^{-0.51} = 0.31$ is much larger than $C$; the acid is almost totally dissociated. $x^2/(0.010 - x) = 0.31$ gives $x = 9.7 \times 10^{-3}\,\mathrm{mol}/\mathrm{L}$, $\mathrm{pH} = 2.01$, [degree of dissociation](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-dissociation) $97\,\%$.

**Exercise 18.11 ★★★.**

The $\mathrm{p}K_a$ of alcohols measured in water increase from methanol (15.5) to ethanol (15.9), propan-2-ol (17.1) and 2-methylpropan-2-ol (19.2). Give two explanations, one through the [inductive effect](#def-b1-electronic-effects-inductive) of the alkyl groups on the alkoxide, one through the [solvation](https://one-course.com/books/chemistry/2/en/chapter/4-intermolecular-forces-and-solvents#def-b1-intermolecular-forces-solvents-dissolution) of the alkoxide.

**Solution of Exercise 18.11.**

Alkyl groups push electrons ($+I$) onto the alkoxide oxygen and make its charge less stable, the more so the more groups. Larger alkoxides are also less well solvated by water, which stabilises a small charged oxygen better than one buried among alkyl groups. Both raise the $\mathrm{p}K_a$.

**Exercise 18.12 ★★★.**

Explain why amides are neither basic on nitrogen nor nucleophilic, whereas amines are both, using the [resonance structure](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) of the amide. Which atom of an amide is protonated in [strong acid](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid)?

**Solution of Exercise 18.12.**

In an amide the nitrogen [lone pair](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-lewis) is shared with the C=O ($\ce{N+=C-O^-}$ structure); taking it for a proton or an [electrophile](#def-b1-electronic-effects-nucleophile) would destroy that stabilisation. In [strong acid](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid) the amide is protonated on the oxygen, which carries the partial negative charge.

## 18.6 Problem: Why Trifluoroethanoic Acid Is So Strong

**Problem 18.1.**

Weekend problem — the inductive series of the halogenated acids, carboxylates against alkoxides, the three nitrophenols, a predominant-reaction calculation, and the ratio of the acidity constants of trifluoroethanoic and ethanoic acids

Data ($\mathrm{p}K_a$ at $25\,{}^{\circ}\mathrm{C}$): ethanoic acid 4.76, chloroethanoic 2.87, dichloroethanoic 1.35, trichloroethanoic 0.51, trifluoroethanoic 0.52, ethanol 15.9, phenol 9.99, 2-nitrophenol 7.23, 3-nitrophenol 8.36, 4-nitrophenol 7.16; $\mathrm{p}K_e = 14.00$.

**Part I — The inductive series.**

1. Compute the ratio of $K_a$ for each step from ethanoic to trichloroethanoic acid.
2. Is the effect of each chlorine the same? Comment.
3. Explain the trend with the [inductive effect](#def-b1-electronic-effects-inductive) .
4. Why would a chlorine on the carbon of a longer chain farthest from COOH have almost no effect?
5. Fluorine is more electronegative than chlorine. What does the comparison of the trifluoro- and trichloro- acids show, and why is it hard to measure such $\mathrm{p}K_a$ precisely?
6. In which form is each of these acids at pH 3?

**Part II — Carboxylates and alkoxides.**

7. Draw the two [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) of the ethanoate ion.
8. What do they predict for the two C–O bond lengths of the ion?
9. Why has the ethoxide ion no equivalent structures?
10. Compute the ratio of the $K_a$ of ethanoic acid and ethanol.
11. Place phenol between the two and justify with the phenoxide [resonance structures](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) .
12. Which of ethanol, phenol and ethanoic acid react almost totally with a hydrogencarbonate solution ( $\mathrm{p}K_a$ 6.37 for $\ce{CO2,H2O}$ / $\ce{HCO3-}$ )?

**Part III — The nitrophenols.**

13. Rank the three nitrophenols and phenol by acidity.
14. Draw a [resonance structure](https://one-course.com/books/chemistry/2/en/chapter/3-lewis-structures-resonance-and-vsepr#def-b1-lewis-resonance-vsepr-resonance) of 4-nitrophenoxide with the charge on the nitro group.
15. Show that no such structure exists for 3-nitrophenoxide.
16. Why is 3-nitrophenol still more acidic than phenol?
17. 2-Nitrophenol is slightly weaker than 4-nitrophenol although both have the [mesomeric effect](#def-b1-electronic-effects-mesomeric) ; propose an explanation involving its OH and the nearby nitro group.
18. At pH 7.5, which nitrophenols are mostly in the anion form? Why does that make 4-nitrophenol a [colour indicator](https://one-course.com/books/chemistry/2/en/chapter/15-titration-methods-and-curves#def-b1-titration-methods-indicator) ?

**Part IV — Trifluoroethanoic acid in water.**

19. Compute the pH of trifluoroethanoic acid at $0.010\,\mathrm{mol}/\mathrm{L}$ (do not assume weak dissociation).
20. Compute the pH of ethanoic acid at $0.010\,\mathrm{mol}/\mathrm{L}$ .
21. Write the reaction of trifluoroethanoic acid with sodium ethanoate and compute its constant.
22. State the ratio $K_a(\ce{CF3COOH})/K_a(\ce{CH3COOH})$ , as a power of ten and as a number.

**Solution of Problem 18.1.**

**1.** $10^{1.89} = 78$; $10^{1.52} = 33$; $10^{0.84} = 6.9$. **2.** No: each further chlorine helps less. The charge of the carboxylate is already well spread, and the measurements become less precise as the acid approaches total dissociation. **3.** Each Cl attracts electron density through the C–C and C–O bonds and stabilises the carboxylate ($-I$). **4.** The [inductive effect](#def-b1-electronic-effects-inductive) fades within two or three bonds. **5.** The two acids appear equally strong (0.52 and 0.51). In water, both are almost totally dissociated at usual concentrations ([Chapter 10](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#ch-b1-predominant-reaction), levelling): a $\mathrm{p}K_a$ near 0 is the limit of what water can distinguish, and the two values carry uncertainties of a few tenths. **6.** Ethanoic acid: acid form ($98\,\%$); chloroethanoic: both, the anion slightly predominant ($10^{3 - 2.87} = 1.3$); the three others: anion. **7.** $\ce{CH3-C(=O)-O^-}$ $\leftrightarrow$ $\ce{CH3-C(-O^-)=O}$. **8.** Two equal C–O bonds, between a double and a single bond. **9.** The charge is on the single oxygen, with no $\pi$ bond to share it. **10.** $10^{15.9 - 4.76} = 10^{11.1}$, about $10^{11}$. **11.** The phenoxide charge spreads to three ring carbons, less electronegative than oxygen: a gain, smaller than in a carboxylate: $\mathrm{p}K_a$ 9.99 between 4.76 and 15.9. **12.** $K = 10^{6.37 - \mathrm{p}K_a}$: ethanoic acid $10^{1.61} = 41$, favoured (carbon dioxide is released with excess hydrogencarbonate); phenol $10^{-3.62}$ and ethanol $10^{-9.5}$: no reaction. **13.** 4-Nitrophenol (7.16) $>$ 2-nitrophenol (7.23) $>$ 3-nitrophenol (8.36) $>$ phenol (9.99). **14.** The quinoid structure of [Exercise 18.3](#exo-b1-electronic-effects-3), with the charge on an oxygen of the nitro group. **15.** The charge reaches only the carbons *ortho* and *para* to the oxygen; the nitro carbon is *meta*. **16.** The $-I$ effect of $\ce{NO2}$. **17.** In 2-nitrophenol the OH forms a [hydrogen bond](https://one-course.com/books/chemistry/2/en/chapter/4-intermolecular-forces-and-solvents#def-b1-intermolecular-forces-solvents-hbond) with an oxygen of the neighbouring nitro group, which stabilises the acid form and makes the proton slightly harder to remove. **18.** Anion fractions $1/(1 + 10^{\mathrm{p}K_a - 7.5})$: 4-nitro $69\,\%$, 2-nitro $65\,\%$, 3-nitro $12\,\%$. Acid and anion of 4-nitrophenol absorb differently, the anion in the visible: its colour appears around its $\mathrm{p}K_a$. **19.** $x^2/(0.010 - x) = 10^{-0.52} = 0.30$: $x = 9.7 \times 10^{-3}\,\mathrm{mol}/\mathrm{L}$, $\mathrm{pH} = 2.01$: almost a [strong acid](https://one-course.com/books/chemistry/2/en/chapter/10-acidbase-equilibria-and-the-predominant-reaction-method#def-b1-predominant-reaction-strong-acid). **20.** $\frac12(4.76 + 2.00) = 3.38$. **21.** $\ce{CF3COOH + CH3COO- -> CF3COO- + CH3COOH}$, $K = 10^{4.76 -
0.52} = 10^{4.24}$: [quantitative](https://one-course.com/books/chemistry/2/en/chapter/7-describing-a-chemical-system-extent-activities-q-and-k#def-b1-extent-q-and-k-quantitative). **22.** $K_a(\ce{CF3COOH})/K_a(\ce{CH3COOH}) =$ **$10^{4.24} =
1.7 \times 10^{4}$**, about ten thousand.