Lewis Acids and Bases

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Kaleb Tesfaye 1I
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Lewis Acids and Bases

Postby Kaleb Tesfaye 1I » Wed May 16, 2018 9:02 am

Is there any correlation between a molecule's bond and whether or not that determines if will be an acid or a base. For example, HCl is a strong acid that is a covalent bond. Does the fact that it is a covalent bond play any role in determining it's characteristic as a strong acid?

Isabelle De Rego 1A
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Re: Lewis Acids and Bases

Postby Isabelle De Rego 1A » Wed May 16, 2018 10:08 am

I do not think so, since all compounds have ionic and covalent properties. The difference between acids and bases is their tendency to give up or accept electrons. Those who give up electrons are a base and those who accept electrons are an acid.

NabilaNizam-1K
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Re: Lewis Acids and Bases

Postby NabilaNizam-1K » Wed May 16, 2018 12:31 pm

In order to determine the strength (bond strength) of an acid, it depends on the size of the 'A' atom: the smaller the 'A' atom, the stronger the H-A bond. When going down a row in the Periodic Table, the atoms get larger so the strength of the bonds get weaker, which means the acids get stronger. For the halogen-containing acids above, HF has the strongest bond and is the weakest acid. The strong bond between the more similarly-sized 'H' and 'F' atoms doesn't want to break and allow the 'H' to transfer. The type of bond does not determine how easy it is for the acid to dissociate in water, thus does not influence the strength of the acid.

Steven Luong 1E
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Re: Lewis Acids and Bases

Postby Steven Luong 1E » Fri May 18, 2018 3:23 pm

That does not seem to be the case because all compounds both have ionic and covalent properties. The main differences so far is that acids accept electrons and bases give up electrons.

OrAmar-1L
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Re: Lewis Acids and Bases

Postby OrAmar-1L » Fri May 18, 2018 4:27 pm

The charge of the molecule/ atoms in it can effect the acidity, but not so much the bond itself. However, ionic bonds are made up of charged particles, but they are opposites and usually cancel each other out. Hope this helps!


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