Polarizability v. Electronegativity

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Seohyun Park 1L
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Joined: Fri Sep 28, 2018 12:29 am

Polarizability v. Electronegativity

Postby Seohyun Park 1L » Fri Nov 09, 2018 2:13 pm

What exactly is the difference between polarizability and electronegativity? I know electronegativity is the pull of electrons and is the cause of dipole moments, but is polarizability only relevant in the induced dipole-induced dipole intermolecular force?

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Joined: Fri Sep 28, 2018 12:24 am

Re: Polarizability v. Electronegativity

Postby annaspain » Fri Nov 09, 2018 2:41 pm

Electronegativity describes an element's ability to pull electrons closer towards its nucleus, which explains why electronegativity increases across a period (elements "want" electrons more to reach octet) and decreases down a group (atomic radius is larger so shielding causes a looser grip on electrons). Polarizability is basically how dipoles are formed. So, polarizable elements must be relatively flexible, so elements that are likely to have higher polarizability must also have a weaker pull on their electrons towards the central nucleus, therefore being less electronegative.

Jocelyne Milke 1G
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Joined: Fri Sep 28, 2018 12:25 am

Re: Polarizability v. Electronegativity

Postby Jocelyne Milke 1G » Sat Nov 10, 2018 6:15 pm

Polarizability is how easily electrons are distorted. Bigger molecules have higher polarizability because there are more electrons and they are more easily distorted.

Sarah Jeong 4F
Posts: 30
Joined: Fri Sep 28, 2018 12:27 am

Re: Polarizability v. Electronegativity

Postby Sarah Jeong 4F » Sat Nov 10, 2018 6:22 pm

Basically if a molecule has a great amount of electronegative difference, they are usually polar. For example, H20. The electronegative difference is large, therefore more electrons go toward oxygen, giving the oxygen a partial negative, and hydrogen a partial positive(polar molecule).

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