The concept of electronegativity (EN) is mainly to discuss the nature of chemical bonding, EN of an atom is the measure of its capacity to attract the shared electron pair towards itself. Linus Pauling compiled the values of EN that are most widely used, and that are displayed for a few elements in Table - 1. These values are based on bond energy differences between atoms bonded to themselves (e.g. A-A) and to other atoms (e.g. A-B), and an arbitary value of 4 to fluorine (most electronegative element)

Mulliken regarded electronegativity as the average value of ionization energy and electron affinity of an atom EN=`1/2`(IE+EA). Both IE and EA are expressed in electron volts. In the Table-2, values of IE and EA for several elements are listed Table-3 shows the values of dipole moments and bond energies for simple molecules.

Which of the following best describes the relationship of electronegativity, bond energy moment in a diatomic molecule ?

Options

A. As electronegativity increases, both bond energy and bond moment increases
B. As electronegativity increases, bond energy decreases but bond moment increases
C. As electronegativity increases, bond energy increases but bond moment decreases
D. As electronegativity increases, both bond energy and bond moment decreases

Answer

A