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Chemistry A Level > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

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1
Q

What is ionic bonding?

A

The electrostatic attraction between oppositely charged ions in a lattice

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2
Q

What is a covalent bond?

A

A shared pair of electrons

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3
Q

What is a coordinate bond?

A

A shared pair of electrons with both electrons supplied by one atom

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4
Q

How is a covalent bond represented?

A

A line

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5
Q

How is a coordinate bond represented?

A

An arrow

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6
Q

What is metallic bonding?

A

The attraction between delocalised electrons and positive ions arranged in a lattice

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7
Q

What are bonding and lone pairs? (3)

A

Charge clouds that repel each other
Bonding pairs - shared pair of electrons
Lone pairs - unshared pair of electrons

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8
Q

How do electrons in an outer shell arrange themselves?

A

As far apart as possible to minimise repulsion

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9
Q

Which sort of repulsion is greatest?

A

Lone pair - lone pair

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10
Q

Which repulsion causes the greatest bond angles?

A

Lone pair - lone pair

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11
Q

Bond angles - Linear

A

180°

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12
Q

Bond angles - Trigonal Planar

A

120°

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13
Q

Bond angles - Tetrahedral

A

109.5°

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14
Q

Bond angles - Trigonal Pyramidial

A

107°

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15
Q

Bond angles - Bent (2 lone pairs)

A

104.5°

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16
Q

Bond angles - Bent (1 lone pair)

A

Slightly less than 120°

17
Q

Bond angles - Trigonal Bipyramidial

A

120° / 90°

18
Q

Bond angles - Seesaw

A

102° / 86.5°

19
Q

Bond angles - T-shaped

A

87.5°

20
Q

Bond angles - Octahedral

A

90°

21
Q

Bond angles - Square Pyramidial

A

90°

22
Q

Bond angles - Square Planar

A

90°

23
Q

What is electronegativity?

A

The ability of an atom to attract the bonding pair of electrons in a covalent bond

24
Q

How does a polar bond form?

A

When two atoms of different electronegativities are covalently bonded, the electron distribution is unsymmetrical

25
Q

How do polar bonds produce polar molecules?

A

If charge s distributed unevenly across a whole molecule, the molecule will have a permanent dipole

26
Q

Why do some molecules with polar bonds not have a permanent dipole?

A

The partial charges in the molecule cancel out

27
Q

What are Van der Waals forces? (4)

A

Electrons in charge clouds are constantly moving
They are more likely to be in one position at any one time, forming a temporary dipole
This induces a dipole in nearby molecules, creating an attraction between them
As the electrons are constantly moving, dipoles are being created and destroyed all the time

28
Q

What makes Van der Waals forces stronger? (2)

A 
Larger molecules (larger electron clouds)
Long, straight molecules
29
Q

What is hydrogen bonding? (4)

A

Strongest intermolecular force
Happens when hydrogen is covalently bonded to oxygen, fluorine or nitrogen
F, N and O are very electronegative so bonding electrons are attracted away from hydrogen
Due to polarity of bond and high charge density in hydrogen (small molecule), the H atoms form weak bonds with lone pairs of electrons on F, N or O atoms in other molecules

30
Q

How does hydrogen bonding affect properties of substances?

A

High melting and boiling points as extra energy is needed to break the hydrogen bonds

31
Q

Why is ice less dense than water? (2)

A

When liquid water cools to form ice, the molecules make more hydrogen bonds as they arrange themselves into a regular lattice
As hydrogen bonds are relatively long, the distance between molecules is greater, on average, in ice so ice is less dense

32
Q

Why are metals malleable?

A

There are no bonds holding specific ions together so they can slide over each other and be shaped easily

33
Q

How do simple covalent structures melt or boil?

A

The weak intermolecular forces are overcome

34
Q

How are macromolecules melted or boiled?

A

The strong covalent bonds are broken

35
Q

How can the type of structure of an unknown substance be determined?

A

Carry out experiments to test its physical properties (electrical conductivity, melting/boiling point, solubility in water)

Chemistry A Level (32 decks)

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