Question

explain all the effects with their application, examples and conditions ?
1. inductive effect
2. resonance
3. hyper conjugation ​

Answer 1

Explanation:

1 ) Inductive Effect

About

When an electron-releasing or an electron-withdrawing species is introduced to a chain of atoms , the corresponding negative or positive charge is due to the atoms belonging to it. This causes a permanent dipole to arise in the molecule and is referred to as the inductive effect.

Applications

• In deciding acidic strength of aliphatic carboxylic acids.
• Stability of alkyl carbocation, carbon free radicals and carboanions.

Examples

Cl is electron-withdrawing by inductive effect in phenylchloride as Cl is very electronegative.

2 ) Resonance

About

Resonance is a way of describing bonding in certain molecules or ions by the combination of several contributing structures ( canonical structures ) into a resonance hybrid ( hybrid structure) in valence bond theory.

Applications

• Resonance is that the more resonance structures a certain molecule has, the more stable

• The transition state in a chemical reaction

Example

Resonant bonds between the carbon atoms of benzene rings.

3 ) Hyper Conjugation

About

Hyperconjugation is the stabilising interaction that results from the interaction of the electrons in a σ-bond with an adjacent empty or partially filled p-orbital or a π-orbital to give an extended molecular orbital that increases the stability of the system.

Application

• Explains stability of carbocations
• Explains stability of free radicals
• Explains stability of carbonyl group

Example

CH3-CH=CH2 is more stable and having higher heat than CH2=CH2

Answer 2

Answer:

Inductive Effect

The inductive effect is a permanent state of polarization. The electron density in a \sigmaσ bond between two unlike atoms is not uniform. The electron density is more dense toward the more electronegative of the two atoms.

The inductive effect is a distance-dependent phenomenon:

C^{\delta+}-X^{\delta-}

C

δ+

−X

δ−

The atom XX above acquires a slightly negative charge (\delta-),(δ−), and the carbon atom a slightly positive charge (\delta+),(δ+), which means the bond is polarized:

If the electronegative atom XX is connected to a chain of carbon atoms, then the positive charge is relayed to the other carbon atoms. C_{1}C

1

, with its positive \deltaδ charge, exerts a pull on the electrons of C_2C

2

, but the pull is weaker than it is between XX on C_1C

1

. The effect rapidly dies out and is usually not significant after the 2^\text{nd}2

nd

carbon atom, or at most the 3^\text{rd}.3

rd

.

:

The +I effect is observed among the less electronegative atoms of the molecule by electron-releasing (or electron-donating) groups. The alkyl groups are usually considered electron-releasing (or electron-donating) groups.

Resonance

Sometimes, there are several correct Lewis structures for a given molecule. Ozone (O_3)(O

3

) is one example. The compound is a chain of three oxygen atoms, and minimizing the charges while giving each atom an octet of electrons requires that the central oxygen atom form a single bond with one terminal oxygen and a double bond with the other terminal oxygen.

When drawing the Lewis structure, the choice of placement for the double bond is arbitrary, and either choice is equally correct. The multiple correct ways of drawing the Lewis structure are called the resonance forms.

the greatest number of covalent bonds.

.

Hyperconjugation

Hyperconjugation helps explain the stability of alkyl radicals. It involves the delocalization of \sigma σ-electrons belonging to the C-H bond of the alkyl group attaching to an atom with an unshared pp orbital. The more the hyperconjugative hydrogen, the more is the stability.