A diatomic molecule XY has a measured dipole moment of $2.5\ \text{D}$ and a bond length of $150\ \text{pm}$. Assuming the dipole arises solely from partial ionic charge transfer, calculate the percentage ionic character of the XY bond. (Use $1\ \text{D}=3.336\times10^{-30}\ \text{C·m}$ and elementary charge $e=1.602\times10^{-19}\ \text{C}$. Based on the percentage, state whether the bond is predominantly ionic or covalent (consider 50 % ionic as predominantly ionic).

Question

A diatomic molecule XY has a measured dipole moment of $2.5\ \text{D}$ and a bond length of $150\ \text{pm}$. Assuming the dipole arises solely from partial ionic charge transfer, calculate the percentage ionic character of the XY bond. (Use $1\ \text{D}=3.336\times10^{-30}\ \text{C·m}$ and elementary charge $e=1.602\times10^{-19}\ \text{C}$. Based on the percentage, state whether the bond is predominantly ionic or covalent (consider >50 % ionic as predominantly ionic).

Accepted Answer

34.7 % ionic character; the bond is predominantly covalent

Gce Model Questions Vol1 2021 Chemistry Question 1

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