Bond enthalpy is defined as the amount of energy required to break one mole of bonds of a particular type in gaseous state.

False

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True

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The correct option is B True

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Q. Bond enthalpy is defined as the amount of energy required to break one mole of bonds of a particular type in gaseous state.

Bond enthalpy is defined as the amount of energy required to break one mole of bonds of a particular type between two atoms in a gasesous state (True/False)

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

Q. The energy required to break one mole of hydrogen-hydrogen bonds in

H_{2}

436 k J

. What is the longest wavelength of light required to break a single hydrogen-hydrogen bond?

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