U1-3-4 - Bonding and Attractions in Compounds Flashcards

Part of the Structure and Bonding topic from Unit 1 of Higher Chemistry, Chemical Changes and Structure

1
Q

To fairly compare the m.p./b.p. of two molecules, they should have _______________ so that they have similar LDF strength.

A

To fairly compare the m.p./b.p. of two molecules, they should have the same no. of electrons so that they have similar LDF strength.

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2
Q

Additional electrostatic forces of attraction between polar molecules.

(Additional = on top of LDFs)

A

Permanent dipole-permanent dipole interactions

PD-PDIs for short

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3
Q

To fairly compare the m.p./b.p. of two molecules, they should have the same no. of electrons so that they have ___________.

A

To fairly compare the m.p./b.p. of two molecules, they should have the same no. of electrons so that they have similar LDF strength.

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4
Q

Permanent dipole-permanent dipole interactions

A

Additional electrostatic forces of attraction between polar molecules.

(Additional = on top of LDFs)

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5
Q

Electrostatic forces of attraction between molecules that contain the highly polar N-H, F-H or O-H bonds.

A

Hydrogen bonds

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6
Q

Weakest type of van der Waals force

A

London dispersion forces

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7
Q

Hydrogen bonds

A

Electrostatic forces of attraction between molecules that contain the highly polar N-H, F-H or O-H bonds.

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8
Q

NH3, H2O and HF have unusually high boiling points. Why?

A

They have hydrogen bonds between their molecules. These require more energy to break than other van der Waals forces.

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9
Q

Both molecules have the same no. of electrons.

Which one has the higher b.p. and why?

A

Ethane-1,2-diol - more H-bonds per molecule

or per mole

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10
Q

Both have the same no. of electrons. Why does propan-1-ol have the higher b.p.? (2)

A

Ethanethiol only has weaker PD-PDIs, propan-1-ol has hydrogen bonds (1)

Hydrogen bonds take more energy to break (1)

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11
Q

Why is ice less dense than liquid water?

A

Hydrogen bonding between molecules (creates a less dense structure in ice than in liquid water)

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12
Q

Strongest type of van der Waals force

A

Hydrogen bonding

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