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The length of the bond is the distance between the centers of the atoms. The dipole moment depends on the multiplicity of the bond, as the length of the bond decreases with multiplicity (i.e., a double bond between two elements is shorter than a single bond between them, a triple bond shorter than a double bond etc.).
Yes, the bond length does decrease if it is a single, double, or triple bond - its multiplicity. This can be sorted out intuitively, knowing that the higher the multiplicity, the stronger the bond and the pull, resulting in a shorter length between the connected atoms (the bond length).
Alissa Stanley 3G wrote:What is the bond length of a resonance structure? For example, if the resonance structure is NO3, would the bond lengths be in-between the length of a single and double bond?
Yes, the real bond lengths are in-between the length of a single and double bond.
I went through several examples of this in class. See your lecture notes for sulfate, benzene, etc.
You can also discuss this today (Thursday) in the many support hours I have organized:
Chemistry & Biochemistry, 4222 Young Hall
Victoria Ford 12-1 pm, Ronald Yang 12-1 pm, Karen Leung 1-2pm
STEM Learning Center, Boelter Science & Engineering Library 8251
Franklin Liu 2-4 pm
Five (physical) hours available today, in addition to Chemistry Community.
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