Chapter 6, Problem 6.99QP

(a)

Interpretation Introduction

Interpretation: The electronegativity for given elements such as $\text{O, F and Cl}$ should be calculated and the calculated values should be compared with the values in Mulliken and Pauling scales.

Concept Introduction:

• Electronegativity is a property of an atom where it tends to attract the electrons shared in the bond to itself.
• $\text{Electronegativity, }\left(\text{EN}\right)\text{=}\frac{\text{First ionization energy}\left({\text{IE}}_{\text{1}}\right)\text{+}\text{Electron affinity}\left(\text{EA}\right)}{\text{2}}$
• Where, ${\text{IE}}_{\text{1}}$ is the amount of energy required to lose one mole of electron whereas $\text{EA}$ is the amount of energy released to gain one electron by an atom.

(b)

Interpretation Introduction

Interpretation: The electronegativity for given elements such as $\text{O, F and Cl}$ should be calculated and the calculated values should be compared with the values in Mulliken and Pauling scales.

Concept Introduction:

• Electronegativity is a property of an atom where it tends to attract the electrons shared in the bond to itself.
• $\text{Electronegativity, }\left(\text{EN}\right)\text{=}\frac{\text{First ionization energy}\left({\text{IE}}_{\text{1}}\right)\text{+}\text{Electron affinity}\left(\text{EA}\right)}{\text{2}}$
• Where, ${\text{IE}}_{\text{1}}$ is the amount of energy required to lose one mole of electron whereas $\text{EA}$ is the amount of energy released to gain one electron by an atom.

(c)

Interpretation Introduction

Interpretation: The electronegativity for given elements such as $\text{O, F and Cl}$ should be calculated and the calculated values should be compared with the values in Mulliken and Pauling scales.

Concept Introduction:

• Electronegativity is a property of an atom where it tends to attract the electrons shared in the bond to itself.
• $\text{Electronegativity, }\left(\text{EN}\right)\text{=}\frac{\text{First ionization energy}\left({\text{IE}}_{\text{1}}\right)\text{+}\text{Electron affinity}\left(\text{EA}\right)}{\text{2}}$
• Where, ${\text{IE}}_{\text{1}}$ is the amount of energy required to lose one mole of electron whereas $\text{EA}$ is the amount of energy released to gain one electron by an atom.