The energy required to break an O ⋅ ⋅ ⋅ ⋅ ⋅ H hydrogen bond in vacuum and in water has to be calculated. Concept introduction: Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires a partial positive charge. This results in the formation of the dipole. The energy of interactions is calculated by the formula shown below. V = Q H Q O 4 π ε r

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Chapter 14, Problem 14B.2P

Interpretation Introduction

Interpretation:

The energy required to break an O⋅⋅⋅⋅⋅H hydrogen bond in vacuum and in water has to be calculated.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires a partial positive charge. This results in the formation of the dipole. The energy of interactions is calculated by the formula shown below.

V=QHQO4πεr

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