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Which member of the following pairs has the larger London dispersion forces?
H2O or H2S
CO2 or CO
CH4 or SiH4

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Answer:

H₂S; CO₂; SiH₄

Explanation:

London dispersion forces are larger in molecules that are large and have more atoms or electrons.

A. H₂O or H₂S

H₂S. S is below O in the Periodic Table, so it is the larger atom. Its electrons are more polarizable.

B. CO₂ or CO

CO₂. CO₂ has more atoms. It is also linear, so the molecules can get close to each other and maximize the attractive forces.

C. CH₄ or SiH₄

CH₄. Si is below C in the Periodic Table, so it is the larger atom. Its electrons are more polarizable.

Differences are stronger in bigger and heavier atoms than in lighter and smaller ones. Its number of electrons inside a larger atom is, in general, farther away from the nuclei than in a small atom.

  • The number of electrons that reasonable accommodations dipoles affect the intensity of the London dispersion forces.
  • [tex]H_2S[/tex] is indeed the bigger element since it is below O just on the Table Of the elements, and the electrons are polarizable to a greater extent.
  • [tex]CO_2[/tex]  has more atoms. It is also linear, allowing the molecules to get close to each other and optimize the attraction forces.
  • Because [tex]CH_4 \ Si[/tex] sits below C on the Periodic Table, it is the bigger atom. Its electrons are more polarizable.

Therefore, the answer is "[tex]\bold{H_2S\ , CO_2\ or \ SiH_4}[/tex]"

Learn more:

brainly.com/question/20514601

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