Distinguish between bond enthalpy and dissociation enthalpy.

Explain enthalpy.

Enthalpy of dissociation is low for

Write the differences between ionisation enthalpy and electron gain enthalpy.

Considering the parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy, compare the oxidising power of F_(2) and Cl_(2) .

The chemical behaviour of dihydrogen is determined, to a large extent, by bond dissociation enthalpy. The H-H bond dissociation enthalpy is the highest for a single bond between two atoms of any element. What inferences would you draw from this fact? It is because of this factor that the dissociation of dihydrogen into its atoms is only 0.081% around 2000K which increases to 95.5% at 5000K. Also, it is relatively inert at room temperature due to the high H-H bond enthalpy. Thus the atomic hydrogen is produced at a high temperature in an electric arc or under ultraviolet radiations. Since its orbital is incomplete with Is' electronic configuration, it does combine with almost all the elements. Which of the following bond dissociation enthalpies is the highest for a single bond between two atoms of any element ?

Distinguish between a sigma bond and a pi bond.

The chemical behaviour of dihydrogen is determined, to a large extent, by bond dissociation enthalpy. The H-H bond dissociation enthalpy is the highest for a single bond between two atoms of any element. What inferences would you draw from this fact? It is because of this factor that the dissociation of dihydrogen into its atoms is only 0.081% around 2000K which increases to 95.5% at 5000K. Also, it is relatively inert at room temperature due to the high H-H bond enthalpy. Thus the atomic hydrogen is produced at a high temperature in an electric arc or under ultraviolet radiations. Since its orbital is incomplete with Is' electronic configuration, it does combine with almost all the elements. At which of the following temperatures, the dissociation of dihydrogen into its atoms will be maximum ?