1.12 Predict/rank the relative London Dispersion Forces between atoms and molecules of different sizes

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What are London Dispersion Forces (LDF)?

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LDF’s are weak intermolecular forces caused by temporary shifts in electron distribution, creating temporary dipoles.

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How does molecular size affect LDF strength?

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Larger molecules/atoms have stronger LDF’s because their electron clouds are more polarizable (easier to distort).

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5 Terms

1
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What are London Dispersion Forces (LDF)?

LDF’s are weak intermolecular forces caused by temporary shifts in electron distribution, creating temporary dipoles.

2
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How does molecular size affect LDF strength?

Larger molecules/atoms have stronger LDF’s because their electron clouds are more polarizable (easier to distort).

3
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Rank the following from weakest to strongest LDF’s: I2, Ne, CH4, C6H6, He

  • He (weakest LDF, smallest atom)

  • Ne (slightly stronger LDF, larger atom)

  • CH4 (weak LDF, small molecule)

  • C6H6 (stronger LDF, larger molecule)

  • I2 (strongest LDF, largest molecule)

4
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Why do larger molecules have stronger LDF’s?

They have more electrons, leading to greater temporary dipoles and stronger intermolecular attractions?

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What happens to boiling points as LDF strength increases?

Boiling points increase because stronger LDF requires more energy to break intermolecular attractions.