FC10 Intermolecular forces Flashcards

1
Q

What are the 3 main categories of intermolecular forces

A
  • Induced dipole-dipole interactions (London forces)
  • Permanent dipole-dipole interactions
  • Hydrogen bonding
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2
Q

What is the strongest intermolecular forces

A

Hydrogen bonding

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3
Q

Do London forces exist between polar or non-polar molecules

A

Both

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4
Q

How are induced dipole-dipole forces created

A
  • Movement of electrons produces a changing dipole in a molecule
  • This instantaneous dipole induces a dipole on a neighbouring molecule
  • This induced dipole induces further dipoles on neighbouring molecules
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5
Q

Are London forces stronger in molecules with more electrons or less electrons

A

More electrons

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6
Q

Do permanent dipole-dipole interactions act between polar or non-polar molecule

A

Polar molecules

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7
Q

Explain why simple molecular compounds have low melting and boiling points

A

Weak intermolecular forces are broken by the energy present at low temperatures

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8
Q

Explain why simple molecular compounds do not usually dissolve readily in water

A

There is little interaction between the molecules in the lattice and the polar solvent molecules

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9
Q

Explain why simple molecular compounds have poor electrical conductivity

A

There are no mobile charged particles

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10
Q

What is a hydrogen bond

A

A special type of permanent dipole-dipole interaction found between molecules containing H-O, H-N, H-F

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11
Q

How do you draw/ show a hydrogen bond

A

dotted/ dashed line

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12
Q

What are the anomalous properties caused by hydrogen bonding

A
  • The solid (ice) is less dense than the liquid (water)
  • The relatively high melting and boiling points
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13
Q

Why is ice less dense than water

A
  • Hydrogen bonds hold water molecules apart in an open lattice structure
  • The water molecules in ice are further apart than in water
  • Solid ice is less dense than liquid water so floats
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14
Q

How many hydrogen bonds can one molecule of water form, and where will they form

A

4 bonds
- 2 on the 2 hydrogen atoms
- 2 of the 2 lone pairs of electrons on the oxygen

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15
Q

Why does water have a relatively high melting and boiling point

A
  • Hydrogen bonds are extra forces, over and above the London forces
  • Hydrogen bonds require a vast amount of energy to break, far more energy than just London forces
  • So it has a much higher melting and boiling point than expected
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16
Q

State which of the following have hydrogen bonding, H20, H2S, CH4, CH3OH, NO2

A
  • H20
  • CH3OH