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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.
PranaviKolla2B wrote:In terms of electrons, what is the difference between a triple bond, a double bond, and a single bond?
A good rule of thumb is that typically the stronger the bond is, the shorter it will be in length.
Triple bonds are the shortest of the bond types and have 3 pairs of electrons. Due to the 3 electron pairs, they are also the strongest.
This is followed up by double bonds which have 2 pairs of electrons.
Single bonds are the weakest in strength of the 3 and only contain 1 electron pair; however, they are also the longest.
505106414 wrote:Does strength of bonds relate to its melting point?
Yes, it does! Since more energy is needed to break stronger bonds, bonds that break with higher melting points would suggest that more energy is required to break the bonds.
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