Question

\[{F_2}\] has lower bond dissociation enthalpy than \[C{l_2}\]. Why?

Answer 1

Hint: We have to know that in chemistry, chemical bonds are three types of classification. This classification is based on electron binding in the bond. There are covalent bonds, ionic bonds and coordinate bonds. The covalent bond is nothing but the mutually sharing of electrons between the two atoms in the molecule. The ionic bond is nothing but highly electronegativity pulls the electrons towards itself, least electronegativity atoms lose the electrons in the molecule. The coordinate bond is nothing but the pair of the electrons from one atom to another atom in the molecule. It is mainly seen in coordination chemistry.

Complete answer:
The molecular formula of fluorine molecules is \[{F_2}\].
The molecular formula of chlorine molecules is \[C{l_2}\].
We compare the bond dissociation enthalpy \[{F_2}\] and \[C{l_2}\], \[{F_2}\] has lower bond dissociation enthalpy than \[C{l_2}\]. Because fluorine molecule size is small and repulsive force will be more compared to the chlorine molecule. The size of the chlorine molecule is more than the size of the fluorine molecule. Hence, \[{F_2}\] has lower bond dissociation enthalpy than \[C{l_2}\].
According to the above discussion, we conclude \[{F_2}\] has lower bond dissociation enthalpy than \[C{l_2}\] because fluorine molecule size is small and repulsive force will be more compare to the chlorine molecule.

Note:
We have to know that all inorganic molecules are made up of ionic bonds. In ionic bonds cation and anion are important. The positive ion attracts negative ions due to this attraction ionic bond. One atom in the molecule has extra electrons in the outermost shell. Due to extra electrons in the shell, it is not able to attain stable electronic configuration. Another atom in the molecule is electron deficient atoms. It wants electrons to attain stable electronic configuration. One atom donates the electron to attain stability and positive charge cation. The other atom accepts the electron to attain stability and negative charge anion.