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The strength of a bond is affected by the charge and distance for ionic bonds. The strength of a bond is affected by the electronegativity differences and the bond length. Generally, double bonds are stronger than single bonds and triple bonds are stronger than double bonds. We will probably need to know the energy of the bond, which is going to be the enthalpy of bonds broken minus the enthalpy of bonds formed
I think Professor Lavelle hasn't gone over it in class yet but there should be a formula or methodology to calculating bond length (primarily looking at single, double, and triple bonds in a lewis dot structure diagram) and thus will help determine bond strength.
I'm not quite sure if there is a value that we use to determine bond strength I think just remembering that as the number of bonds increase, so does its strength so the strongest bonds are triple bonds>double bonds>single bond with single bonds being the weakest.
Triple bonds are shorter than double bonds because there are more attraction forces and they tend to be stronger. Double bonds are shorter and stronger than single bonds because of the same reason.
Last edited by Junwei Sun 4I on Thu Oct 24, 2019 8:50 pm, edited 1 time in total.
PranaviKolla3G wrote:In terms of electrons, what is the difference between a triple bond, a double bond, and a single bond?
Triple bonds represent three pairs of electrons. Double bonds represent two pairs of electrons. Single bonds represent one pair of electrons.
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