Synthesis Topic 2 Flashcards

1
Q

What is the general tendency of acid?

A

To lose a proton.

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2
Q

What is the general tendency of base?

A

To accept a proton.

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3
Q

What is pKa?

A

The measure of acidity and basicity.

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4
Q

What pKa tells about an acid?

A

It describes how much of the acid has been deprotonated and exists in its conjugate base form: it is a quantitative measure of acid strength in solution.

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5
Q

What are the main factors that affect strength of an acid?

A
  1. Stability of the conjugate base A-: electronegative A and inductively and mesomerically electron withdrawing substituents stabilise A- and make HA a strongger acid
  2. The H-A bond strength: the weaker the bond the stronger the acid
  3. The solvent: the better the solvent is at solvating/stabilising ions, the easier it is for the acid to be deprotonated.
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6
Q

What pKaH tells about an base?

A

The lower the pKaH the weaker the base.

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7
Q

What is pKaH?

A

The pKa of conjugate acid

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8
Q

What affects the strength of the base?

A

Any factor that increases the strength of an acid usually decreases the strength of the corresponding conjugate base.

The main factor that affects the strength of a base is the availability of its lone pair of electrons: electronegative B and inductively and measomerically electron-withdrawing substituents make lone pair less available for reaction with H+, making B a weaker base

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9
Q

Why aromatic amines are weaker bases than aliphatic amines?

A

It is because in aromatic amines lone pair on N can be delocalised in aromatic ring. However, the N lone pair is in an sp3 orbital. Therefore, orbital overlap with the aromatic π-system is not optimal and delocalisation is only partial.

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10
Q

What is the meaning of aliphatic compound?

A

Any chemical compound belonging to the organic class in which the atoms are connected by single, double, or triple bonds to form nonaromatic structures.

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11
Q

What is mesomeric effect?

A

It is defined as the polarity produced in the molecule by the interaction of two π bonds or between a π bond and lone pair of electrons present on an adjacent atom.

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12
Q

Why aromatic rings are more acidic than aliphatic ones?

A

Due to resonance stabilisation of the conjugate base.

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13
Q

What is the effect of aromatic rings on radicals?

A

Aromatic rings stabilises radicals as radical can be delocalised to the aromatic ring.

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14
Q

Why electron donating groups makes acid weaker?

A

Inductively electron donating group destabilises conjugate base.

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15
Q

Why electron withdrawing groups makes acid stronger?

A

It stabilises conjugate base.

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16
Q

Which compound is stronger base and why?

A

Oxygen is more electronegative than nitrogen, the lone pair on oxygen is held closer to the nucleus and thus less available for reaction with H+ making phenol a weaker base than aniline.

17
Q

What is formula for substituent constant?

A
18
Q

What positive σ means?

A

It indicates an electron-withdrawing substituent.

19
Q

What negative σ means?

A

It indicates an electron-donating substituent.

20
Q

What is the Hammett equation?

A
21
Q

What reaction constant tells us?

A

It tells us how the reaction responds to substituent effects and gives us an idea about the mechanism of the reaction.

22
Q

What positive ρ value means?

A

It means there are more electrons in the transition state than in the starting material: electron-withdrawing substituents increase rate of reaction

23
Q

Why Hammett effect does not work for ortho- substituents?

A

Because para and meta substituents have electronic effect and otrtho substituents have steric effects.

24
Q

What negative ρ value tells us?

A

It means fewer electrons are present in the transition state than in the starting material: electron-donating substituents increase reaction rate.

25
Q
A

Negative ρ means electron-donating substituents increase reaction rate. As a result RDS must involve a positively charged transition state as electron-donating substituent will stabilise positive charge.