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Introduction to Alkenes

Amount of ene...

Question

Amount of energy required to break a specific covalent bond is called:

A

Bond dissociation energy

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B

Bond energy

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C

Bond enthalpy

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D

All of the above

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Solution

The correct option is D All of the above
The energy required to break a specific covalent bond in one mole of gaseous molecules is called the bond energy or the bond dissociation energy or bond enthalpy.

Hence, the correct option is $D$

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Q. The amount of energy required to break a covalent bond is known as bond energy.

Q. Bond energy is the energy required to break a covalent bond between two atoms in its __________ state.

Q. The amount of energy required to break a bond is same as the amount of energy released when the same bond is formed. In gaseous state, the energy required for homolytic cleavage of a bond is called Bond Dissociation Energy (BDE) or Bond Strength. BDE is affected by s-character of the bond and the stability of the radicals formed. Shorter bonds are typically stronger bonds. BDEs for some bonds are given below:

For the following reaction

C H_{4} (g) + C l_{2} (g) light - - \to C H_{3} C l (g) + H C l (g)

The correct statement is

Q. Bond dissociation energy of a bond (A - B) is

165 k J^{- 1}

. Calculate the minimum frequency of photon required to break this bond.

Q. The amount of energy required to break a bond is same as the amount of energy released when the same bond is formed. In gaseous state, the energy required for homolytic cleavage of a bond is called Bond Dissociation Energy (BDE) or Bond Strength. BDE is affected by s-character of the bond and the stability of the radicals formed. Shorter bonds are typically stronger bonds. BDEs for some bonds are given below:

Correct match of the

C-H

bonds (shown in bold) in Column J with their

BDE

K

Column $J$ Molecule	Column $K$ $B D E (k c a l m o l^{- 1})$
(P) $H - C H (C H_{3})_{2}$	(i) $132$
(Q) $H - C H_{2} P h$	(ii) $110$
(R) $H - C H = C H_{2}$	(iii) $95$
(S) $H - C \equiv C H$	(iv) $88$

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