why is bond dissociation enthalpy different for isotopes of hydrogen?
Dear Student,
The bond dissociation enthalpy is termed for computing energy in the molecules exhibiting bonds like covalent, ionic, van der waals, dipole-dipole, etc.., not for isotopes as bond dissociation is mostly depends on bonds formed from electron sharing but in hydrogen isotopes it is different.
Hydrogen is the third most abundant source available in the globe and the source of energy too, the isotopes are of three states namely Protium, Deuterium, Tritium, all these isotopes are directly under the influence of neutrons. Hence the normal enthalpy in bond dissociation is different with hydrogen isotopes by the presence of neutrons.
Regards.
The bond dissociation enthalpy is termed for computing energy in the molecules exhibiting bonds like covalent, ionic, van der waals, dipole-dipole, etc.., not for isotopes as bond dissociation is mostly depends on bonds formed from electron sharing but in hydrogen isotopes it is different.
Hydrogen is the third most abundant source available in the globe and the source of energy too, the isotopes are of three states namely Protium, Deuterium, Tritium, all these isotopes are directly under the influence of neutrons. Hence the normal enthalpy in bond dissociation is different with hydrogen isotopes by the presence of neutrons.
Regards.