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Chemistry > P1: 3 Bonding > Flashcards

P1: 3 Bonding Flashcards

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1
Q

What does ionic bonding involve?

A

Strong electrostatic attraction between oppositely charged ions in a lattice.

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2
Q

What does a single covalent bond contain?

A

A shared pair of electrons.

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3
Q

What do multiple covalent bonds contain?

A

Multiple shared pairs of electrons.

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4
Q

What does a co-ordinate (dative covalent) bond contain?

A

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

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5
Q

What does metallic bonding involve?

A

Attraction between delocalised electrons and positive ions arranged in a lattice.

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6
Q

What are the four types of crystal structure?

A

Ionic.
Metallic.
Macromolecular (giant covalent).
Molecular.

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7
Q

What are bonding and lone pairs of electrons?

A

Charge clouds that repel each other.

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8
Q

What do pairs of electrons in the outer shell do?

A

Arrange themselves as far apart as possible to minimise repulsion.

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9
Q

What type of repulsion is greater in pairs of electrons?

A

Lone pair - lone pair. (greatest)
Lone pair - bond pair.
Bond pair - bond pair (weakest)

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10
Q

What is electronegativity?

A

The power of an atom to attract the pair of electrons in a covalent bond.

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11
Q

What produces a polar covalent bond?

A

The electron distribution in a covalent bond between elements with different electronegativities will be asymmetrical.

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12
Q

What shape and bond angle does 2 bonding pairs and 0 lone pairs make?

A

Linear, 180

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13
Q

What shape and bond angle does 3 bonding pairs and 0 lone pairs make?

A

Trigonal planar, 120

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14
Q

What shape and bond angle does 2 bonding pairs and 1 lone pair make?

A

Bent (V-shape), 118

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15
Q

What shape and bond angle does 4 bonding pairs and 0 lone pairs make?

A

Tetrahedral, 109.5

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16
Q

What shape and bond angle does 3 bonding pairs and 1 lone pair make?

A

Trigonal pyramidal, 107

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17
Q

What shape and bond angle does 2 bonding pairs and 2 lone pairs make?

A

Bent V-shape, 104.5

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18
Q

What shape and bond angle does 5 bonding pairs and 0 lone pairs make?

A

Trigonal bipyramidal, 120 and 90

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19
Q

What shape and bond angle does 4 bonding pairs and 1 lone pair make?

A

Trigonal pyramidal, 119 and 89
Or
See-saw, 119, 89

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20
Q

What shapes and bond angles does 3 bonding pairs and 2 lone pairs make?

A

Trigonal planar, 120
Or
T-shape, 89

21
Q

What shape and bond angle does 6 bonding pairs and 0 lone pairs make?

A

Octahedral, 90

22
Q

What shape and bond angle does 5 bonding pairs and 1 lone pair make?

A

Square pyramid, 89

23
Q

What shape and bond angle does 4 bonding pairs and 2 lone pairs make?

A

Square planar, 90

24
Q

What are the rules for working out the shape of molecules and ions?

A
  1. How many electrons are around the central atom?
  2. Add 1 electron for each bond.
  3. Add 1 electron for a negative charge, deduct 1 electron for a positive charge.
  4. Divide total by 2 to give number of pairs.
  5. How many bonding pairs and lone pairs?
  6. Arrange electrons in space to minimise repulsion.
  7. Treat double bonds as a single unit.
25
Q

What is the formula of the compound ion sulfate?

A

SO4 2-

26
Q

What is the formula of the compound ion hydroxide?

A

OH -

27
Q

What is the formula for the compound ion nitrate?

A

NO3 -

28
Q

What is the formula for the compound ion carbonate?

A

CO3 2-

29
Q

What is the formula for the compound ion ammonium?

A

NH4 +

30
Q

What are the melting and boiling points of molecular substances influenced by?

A

The strength of the intermolecular forces.

31
Q

What are the intermolecular forces in order of strength?

A

Van der Waals
Permanent dipole-dipole forces
Hydrogen bonding

32
Q

Where are van der Waal’s forces present?

A

In all molecular substances.

33
Q

Why do van der Waal’s forces occur?

A

Electrons are constantly moving around so there will always be an uneven electron distribution (partly due to electronegativity).
This causes a temporary dipole within a molecule.
This induces a temporary dipole in a neighbouring molecule.
There is an attraction between these molecules - temporary induced dipole-dipole attraction.

34
Q

What affects the power of van der Waal’s forces?

A

The bigger the molecule, the greater the van der Waal’s forces.

35
Q

Where does permanent dipole-dipole attraction occur?

A

Between polar molecules.

36
Q

Where does hydrogen bonding occur?

A

Where an H atom is bonded to a very electronegative atom.
Only fluorine, oxygen and nitrogen.

37
Q

How does a hydrogen bond occur?

A

The polar bond between the H and F/O/N atom leaves the H nucleus exposed.
Therefore, there is a strong attraction from the lone pair on the F/O/N of one molecule to the exposed H nucleus of another molecule.
This is the strongest intermolecular force.

38
Q

What are the properties of substances with ionic bonding?

A

High melting/ boiling points.
Typically solid at rtp.
Doesn’t conduct electricity except when liquid.
Soluble in water.

39
Q

What are the properties of substances with molecular bonding?

A

(Simple covalent)
Low melting and boiling points.
Typically solid at rtp (except for I2 which is solid).
Doesn’t conduct electricity.
Solubility depends on how polarised the molecule is.

40
Q

What are the properties of substances with macromolecular bonding?

A

High melting and boiling points.
Typically solid at rtp.
Doesn’t conduct electricity (except graphite)
Sublimes rather than melts.
Not soluble in water.

41
Q

What are the properties of substances with metallic bonding?

A

High melting/ boiling points.
Typically solid at rtp.
Does conduct electricity.
Not soluble in water.

42
Q

What is the structure of diamond?

A

A macromolecular allotrope of carbon.
There is covalent bonding between every carbon atom.

43
Q

What is the structure of graphite?

A

A macromolecular allotrope of carbon.
Has strong covalent bonds between carbon atoms but weak van der Waals forces between layers.

44
Q

What is the structure of iodine?

A

A molecular crystal.
There is a strong covalent bond that holds two iodine molecules together.
Since iodine molecules have a large number of electrons, the van der Waals forces are strong enough to hold the molecules together as a solid.
But van der Waals are much weaker than covalent bonds.

45
Q

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

A

Overall, the molecule isn’t polar.

46
Q

What is the structure of sodium chloride?

A

Giant ionic lattice.

47
Q

What is the structure of magnesium?

A

Giant metallic lattice.

48
Q

What is the structure of ice?

A

Lattice.
Less dense than water.

Chemistry (33 decks)

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