Strengths of H2S vs H2Se

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Madison Gil 3D
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Strengths of H2S vs H2Se

Postby Madison Gil 3D » Sat Dec 08, 2018 5:09 pm

In the final review session, Lyndon said that H2Se has a greater boiling point (and therefore stronger bonds) because it has greater London dispersion forces than H2S does. However, in the chemistry textbook version 6 p.484, H2Se is expected to be a stronger acid than H2S because H2Se has weaker bonds. Does having more london dispersion forces make a molecule stronger, or more likely to ionize? And which explanation would be correct?

Austin Clack
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Re: Strengths of H2S vs H2Se

Postby Austin Clack » Sat Dec 08, 2018 6:28 pm

LDS forces do contribute to a higher boiling point and therefore a stronger molecule. As for these conflicting explanations, stronger bonds make boiling point greater and conversely, pH higher (less acidic).

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Re: Strengths of H2S vs H2Se

Postby Rami_Z_AbuQubo_2K » Sun Dec 09, 2018 5:13 pm

Bigger london dispersion forces do lead to higher boiling points when a molecule exhibits no hydrogen bonds, is not polar or when the polarity is almost the same between two molecules. The bigger the atom, the greater the shift in electrons to create a temporary dipole and makes H2Se a stronger acid

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Re: Strengths of H2S vs H2Se

Postby Anjali_Kumar1F » Sun Dec 09, 2018 5:41 pm

Why is London Disperse Force in every bond?

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Re: Strengths of H2S vs H2Se

Postby 604656370 » Mon Dec 10, 2018 12:35 am

LDF is found in every bond because its the most basic form of molecular attraction. Since electrons are constantly moving, at any given time, one atom will be more electronegative than the other atom. Thus, there will always be some degree of induced dipole-induced dipole (also known as LDF).

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