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A-Level Chemistry > Bonding > Flashcards

Bonding Flashcards

1
Q

What is ionic bonding?

A

The electrostatic force of attraction between oppositely charged ions

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2
Q

How are ions formed?

A

Ions are formed when atoms lose or gain electrons

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3
Q

What type of ions do metals form?

A

Positive ions because they lose electrons

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4
Q

What type of ions do non-metals form?

A

Negative ions because they gain electrons

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5
Q

What are compound ions?

A

Ions made up of a group of atoms with an overall charge

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6
Q

What is the structure of ions?

A

They have a giant ionic lattice

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7
Q

What are the properties of ionic compounds?

A

They have:

  • high melting points
  • conduct electricity when molten or dissolved
  • tend to dissolve in water
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8
Q

How would you prove if a substance is ionic?

A
  • dissolve the substance in water
  • add a cathode and anode into the solution with a bulb in the circuit
  • if the solution conducts electricity(bulb switches on), then it is ionic
  • if insoluble melt the substance
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9
Q

How would you determine which ionic compound has a higher melting point?

A

Charge determines which ionic compound has a higher melting point, not the size

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10
Q

What happens down the group as the ions become larger?

A

Charge density decreases

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11
Q

What is charge density?

A

The ratio of the charge of an ion to its volume

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12
Q

Which are the five common compound ions?

A 
sulfate-SO4^2-
hydroxide-OH-
nitrate-NO3-
carbonate-CO3^2-
ammonium-NH4+
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13
Q

What is a covalent bond?

A

A single shared pair of electrons

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14
Q

What is the structure of diamond?

A

Giant covalent
Tetrahedral
Carbon makes 4 covalent bonds

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15
Q

What are the properties of diamond?

A

Very high melting point
Hard
insoluble
Non-conductor of electricity(the outer electrons are held in localised bonds)

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16
Q

What is the structure of graphite?

A

Giant covalent
Planar- arranged in layers
Carbon makes 3 covalent bonds

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17
Q

What are the properties of graphite?

A

High melting point
Conducts electricity(each carbon has one delocalised electron)
Slippery-the layers can slide over each other easily
(used in pencils and as a dry lubricant)
Soft
Insoluble

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18
Q

Which forces bond together the layers of graphite?

A

Weak van der Waals forces

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19
Q

What is the structure of iodine?

A

Molecular covalent

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20
Q

What are the properties of iodine?

A

Low boiling and melting point

Poor conductor of electricity(no charged particles)

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21
Q

What is dative covalent bonding?

A

A covalent bond where both of the shared pair of electrons come from one atom

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22
Q

What are the common examples of dative covalent bonding?

A

NH4+
H3O+
NH3BF3

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23
Q

What is metallic bonding?

A

The electrostatic force of attraction between the positive metal ions and the delocalised electrons

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24
Q

What is the structure of metallic bonding?

A

A giant metallic lattice

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25
Q

What are the properties of metals?

A

High melting point
Good thermal and electrical conductors
Soft, ductile and malleable
Arranged in layers

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26
Q

How does the number of delocalised electrons per atom affect the melting point?

A

The more delocalised electrons there are per atom, the stronger the bonding and the higher the melting point

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27
Q

What happens to the metallic bonding strength going down a group?

A

Going down a group, the ions become larger, the charge density decreases and the weaker the metallic bonding

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28
Q

How many bonding and lone pairs are there in a LINEAR molecule and what is the bond angle of the molecule?

A

Bonding pairs - 2
Lone pairs - 0
Bond angle - 180

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29
Q

How many bonding and lone pairs are there in a TRIGONAL PLANAR molecule and what is the bond angle of the molecule?

A

Bonding pairs - 3
Lone pairs - 0
Bond angle - 120

30
Q

How many bonding and lone pairs are there in a TETRAHEDRAL molecule and what is the bond angle of the molecule?

A

Bonding pairs - 4
Lone pairs - 0
Bond angle - 109.5

31
Q

How many bonding and lone pairs are there in a TRIGONAL PYRAMID molecule and what is the bond angle of the molecule?

A

Bonding pairs - 3
Lone pairs - 1
Bond angle - 107

32
Q

How many bonding and lone pairs are there in a BENT(angular, V-shaped, non-linear) molecule and what is the bond angle of the molecule?

A

Bonding pairs - 2
Lone pairs - 2
Bond angle - 104.5

33
Q

How many bonding and lone pairs are there in a TRIGONAL BIPYRAMID molecule and what are the bond angles of the molecule?

A

Bonding pairs - 5
Lone pairs - 0
Bond angles - 120 and 90

34
Q

How many bonding and lone pairs are there in an OCTRAHEDRAL molecule and what is the bond angle of the molecule?

A

Bonding pairs - 6
Lone pairs - 0
Bond angle - 90

35
Q

How many bonding and lone pairs are there in a SEESAW molecule and what is the bond angle of the molecule?

A

Bonding pairs - 4
Lone pairs - 1
Bond angle - 117.5-120 and 87-88

36
Q

How many bonding and lone pairs are there in a T-SHAPED molecule and what is the bond angle of the molecule?

A

Bonding pairs - 3
Lone pairs - 2
Bond angle - 88

37
Q

How many bonding and lone pairs are there in a SQUARE PLANAR molecule and what is the bond angle of the molecule?

A

Bonding pairs - 4
Lone pairs -2
Bond angle 90

38
Q

What type of repulsion is the greatest creating the biggest bond angles?

A

Lone pair-lone pair repulsion

39
Q

What type of repulsion is the smallest creating the smallest bond angles?

A

Bonding pair-bonding pair repulsion

40
Q

By how much do lone pairs reduce bond angles?

A

2.5 degrees per lone pair

41
Q

What is electronegativity?

A

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

42
Q

Which is the most electronegative element?

A

Fluorine

43
Q

Why is fluorine the most electronegative element?

A

It is the smallest atom with the most need to fill its outer shell
it has the least number of shells and electrons

44
Q

What is a polar bond?

A

A bond where a bonding pair is shared unequally and there are partial charges on the atoms in the bond

45
Q

What is a dipole?

A

A difference in charge between two atoms caused by a shift in electron density in the bond

46
Q

Why are symmetrical molecules not polar?

A

The dipoles cancel out and there is no permanent dipole

47
Q

What is a permanent dipole?

A

It is the unequal sharing of electrons in a covalent bond leading to partial charged due to the difference in electronegativity

48
Q

What are intermolecular forces?

A

Forces between molecules

49
Q

What are the three intermolecular forces?

A

Van der Waals forces
Permanent dipole-dipole
Hydrogen bonding

50
Q

What are van der Waals forces?

A

They are found between all atoms and molecules
They cause atoms and molecules to be attracted to each other
Weakest intermolecular forces

51
Q

What affects the magnitude of the van der Waals forces?

A

The number of electrons

The shape of the molecule

52
Q

How does the number of electrons affect the size of the van der Waals forces?

A

As the number of electrons increases, the larger the molecule and therefore the stronger the van der Waals forces

53
Q

How does the shape of the molecule affect the van der Waals forces?

A

Long straight molecules have a larger surface area of contact and therefore the stronger the forces between them

54
Q

What are permanent dipole-dipole forces?

A

They occur between polar molecules which have a permanent dipole
They are stronger than van der Waals forces

55
Q

What would happen if you placed a charged rod next to a jet of a polar liquid?

A

The liquid will move towards the rod

56
Q

Why would the liquid move towards the rod?

A

The polar liquid contains molecules with permanent dipoles
It doesn’t matter if the rod is positively or negatively charged because the polar molecules can turn around so that the oppositely charged end is attracted towards the rod

57
Q

What is hydrogen bonding?

A

It occurs only when hydrogen is covalently bonded to nitrogen, oxygen and fluorine
It is the strongest intermolecular force

58
Q

Why does hydrogen bonding only occur when hydrogen is covalently bonded to nitrogen, oxygen and fluorine?

A

They are very electronegative compared to hydrogen

59
Q

What are the properties of substances with hydrogen bonding?

A

They have higher melting and boiling points compared to similar molecules because extra energy is needed to break the hydrogen bonds

60
Q

What happens as water cools to form ice?

A

The molecules make more hydrogen bonds and arrange themselves into a regular lattice

61
Q

Why does ice float?

A

In the regular structure, the molecules are further apart and therefore, ice is less dense than liquid water

62
Q

What determines the melting and boiling points of a substance?

A

The strength of the attraction between its particles

63
Q

What are the properties of ionic bonding?

A 
High melting and boiling points
Solid at room temperature
Don't conduct electricity when solid
Conduct electricity when molten or dissolved
Soluble in water
64
Q

What are the properties of simple covalent bonding?

A

Low melting and boiling points
Can be solid but usually liquid or gas at room temperature
Don’t conduct electricity when a solid or liquid
Solubility in water depends on the polarity of the molecule

65
Q

What are the properties of giant covalent bonding?

A

High melting and boiling points
Solid at room temperature
Don’t conduct electricity except graphite
Insoluble

66
Q

What are the properties of metallic bonding?

A

High melting and boiling points
Solid at room temperature
Conduct electricity as a solid and molten
Insoluble

67
Q

What are the physical properties of solids?

A

The particles are very close together
High density which makes solids incompressible
The particles vibrate about a fixed point as they can’t move freely

68
Q

What are the physical properties of liquids?

A

Similar density to a solid which makes liquids incompressible
The particles vibrate freely and randomly within the liquid allowing it to flow

69
Q

What are the physical properties of gases?

A

The particles have more energy and are further apart
The density is low which makes gases very compressible
The particles move freely and diffuse.

70
Q

Describe the bonding between hydrogen chloride molecules

A

The delta negative charge on the chlorine would be attracted to the delta positive charge on the hydrogen on the next molecule

A-Level Chemistry (30 decks)

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