Given that compound X has stronger intermolecular force and has no dipole-dipole forces, compound Y has Hydrogen bonding, the relative solubility of the compounds X and Y in water and non-polar solvent has to be predicted and the same has to be explained. Concept Introduction: The intermolecular forces are the attractive forces between the molecules of a compound. The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. Among these London dispersion force is the weakest one and dipole-dipole force is the strongest one. London dispersion forces exist in non-polar covalent compounds . Dipole-dipole forces present in polar covalent compounds . This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature. Hydrogen bonding is formed in polar covalent compounds containing direct bond between Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen . The order of strength of intermolecular force is, London dispersion force < Dipole-dipole force < Hydrogen bonding. However London dispersion forces become stronger in case of larger molecules.

Question

6. A solution (0.0004 M) of Fe(S2CNEt2)3 (see the structural drawing below) in chloroform has absorption bands at: 350 nm (absorbance A = 2.34); 514 nm(absorbance A = 0.0532); Calculate the molar absorptivity values for these bands. Comment on their possible nature (charge transfer transitions or d-d S N- transitions?). (4 points)

Answer 1

Question

Chapter 12.2, Problem 12.2CC

Interpretation Introduction

Interpretation:

Given that compound X has stronger intermolecular force and has no dipole-dipole forces, compound Y has Hydrogen bonding, the relative solubility of the compounds X and Y in water and non-polar solvent has to be predicted and the same has to be explained.

Concept Introduction:

The intermolecular forces are the attractive forces between the molecules of a compound.

The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. Among these London dispersion force is the weakest one and dipole-dipole force is the strongest one.

London dispersion forces exist in non-polar covalent compounds. Dipole-dipole forces present in polar covalent compounds. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.

Hydrogen bonding is formed in polar covalent compounds containing direct bond between Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen.

The order of strength of intermolecular force is,

London dispersion force < Dipole-dipole force < Hydrogen bonding.

However London dispersion forces become stronger in case of larger molecules.

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6. A solution (0.0004 M) of Fe(S2CNEt2)3 (see the structural drawing below) in chloroform has absorption bands at: 350 nm (absorbance A = 2.34); 514 nm(absorbance A = 0.0532); Calculate the molar absorptivity values for these bands. Comment on their possible nature (charge transfer transitions or d-d S N- transitions?). (4 points)

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