Bond Strength

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Bond Strength

Postby 304655635 » Fri Nov 03, 2017 1:04 pm

Quick question: I just don't get how a molecule with another electron can have a stronger bond than the same molecule with one less electron. Wouldn't the extra electron cause more repulsion and a longer bond?

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Joined: Fri Sep 29, 2017 7:07 am

Re: Bond Strength

Postby EveEmm3D » Fri Nov 03, 2017 6:14 pm

Can you give an example of a molecule you are referring to? Your question might be easier to answer when looking at a specific molecule.

ami patel
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Joined: Thu Jul 27, 2017 3:00 am

Re: Bond Strength

Postby ami patel » Fri Nov 03, 2017 9:58 pm

I am not sure what exactly you are referring to, but longer bonds are weaker and shorter bonds are stronger. That is why molecules with double bonds (shorter) are stronger than those with single bonds and thus have higher dissociation energies! Yay!

Katherine Jordak 1H
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Re: Bond Strength

Postby Katherine Jordak 1H » Sun Nov 19, 2017 10:06 pm

Also, the smaller the difference in electronegativity between the two bonded atoms, the shorter the bond. This usually happens closer to the right side of the periodic table amd creates covalent bonds. These bonds are stronger because the two atoms are "sharing" the electrons. Neither one will want to let them go.

Anthony Mercado 1K
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Re: Bond Strength

Postby Anthony Mercado 1K » Sun May 20, 2018 10:22 pm

Why do we even classify compounds with bonds lengths and strengths? I was led to believe that these are never a true depiction of such, in relation to concepts such as the average bond length of resonance structures

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Re: Bond Strength

Postby SamanthaGrohe1B » Sun May 20, 2018 11:15 pm

I don't believe you mean that it has a stronger bond but rather that it has the greater chance of dipole interactions or Van Der Waals forces between the atoms due to the extra charge of the atom. This can make a stronger interaction between the atoms or molecules of the compound.

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