U1-3-3 - Bonding and Attractions in Elements Flashcards

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

1
Q

Why do covalent networks have high m.p./b.p.?

A

Strong covalent bonds are broken to melt/boil them, this requires a lot of energy.

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2
Q

What are fullerenes?

A

Molecular forms of carbon, e.g. C60

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3
Q

Intermolecular forces/van der Waals forces

A

Forces (attractions) between molecules

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4
Q

Forces of attraction between
temporary dipoles and induced dipoles.

A

London dispersion forces

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5
Q

What causes temporary dipoles to form in atoms and molecules?

A

Any one of:

uneven distribution of electrons

electron cloud ‘wobble’

movement of electrons in the molecule

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6
Q

LDF strength increases as …

A

the no. of electrons increases.

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7
Q

London dispersion forces

A

Forces of attraction between
temporary dipoles and induced dipoles.

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8
Q

Oxygen atoms have 8 electrons, neon atoms have 10 electrons.

Neon atoms have more electrons, but LDFs are stronger in oxygen. Why?

A

Oxygen is diatomic (O2) and oxygen molecules have more electrons (16) than neon atoms (10).

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9
Q

In covalent molecular substances, the boiling and melting point depend on …

A

… the strength of intermolecular forces.

(stronger forces = higher b.p./m.p)

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10
Q

What is wrong with this statement?

“When water boils, covalent bonds are broken.”

A

Water is covalent molecular - only weak van der Waals forces are broken, not strong covalent bonds.

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11
Q

What is wrong with this statement?

“When boron boils, covalent bonds are broken.”

A

Nothing - boron is a covalent network, so covalent bonds are indeed broken.

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12
Q

Structure of noble gases

A

Monatomic

They exist as single atoms

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