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A-Level Chemistry > Electrons, Bonding and Structure > Flashcards

Electrons, Bonding and Structure Flashcards

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1
Q

How many electrons can be in shell 1?

A

2

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2
Q

How many electrons can be in shell 2?

A

8

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3
Q

How many electrons can be in shell 3?

A

18

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4
Q

How many electrons can be in shell 4?

A

32

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5
Q

What is an electron shell?

A

Group of atomic orbitals with the same principle quantum number, n

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6
Q

What is n (principle quantum number)?

A

A number representing the overall energy level of the orbital.

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7
Q

What is an orbital?

A

A region of high probability within an atom that can hold up to 2 electrons with opposite spin

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8
Q

What does it mean if n (principle quantum number) is bigger?

A

The bigger the number, the further the distance between the energy level and atomic nucleus

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9
Q

How man electrons do orbitals hold?

A

2

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10
Q

What must electrons in the same orbital have?

A

Opposite spin

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11
Q

What are the 4 orbitals?

A

S-orbital
P-orbital
D-orbital
F-orbital

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12
Q

Where is s-orbital present?

A

n=1 upwards

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13
Q

Where is p-orbital present?

A

n=2 upwards

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14
Q

Where is d-orbital present?

A

n=3 upwards

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15
Q

Where is f-orbital present?

A

n=4 upwards

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16
Q

How many s-orbitals does a shell contain?

A

1

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17
Q

How many p-orbitals does a shell contain?

A

3

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18
Q

How many d-orbitals does a shell contain?

A

5

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19
Q

How many f-orbitals does a shell contain?

A

7

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20
Q

What is the shape of a s-orbital?

A

Sphere

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21
Q

What is the shape of a p-orbital?

A

Dumbbell

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22
Q

What is the order that you fill orbitals?

A

1s 2s 2p 3s 3p 4s 3d 4p

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23
Q

What are the two exceptions when it comes to filling orbitals?

A

Cu

Cr

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24
Q

What does Cu do?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

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25
Q

What does Cr do?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

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26
Q

What do CU and Cr do this?

A

Because they can become stable from full and half full 3d sub shells

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27
Q

How can you shorten filling orbitals?

A

By using the noble gases

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28
Q

What are the three noble gases that you can use?

A

He 1s2
Ne 1s2 2s2 2p6
Ar 1s2 2s2 2p6 3s2 3p6

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29
Q

What is a lattice?

A

A regular repeated three dimensional arrangement of atoms, ions or molecules in a metal or other crystalline solid

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30
Q

What is ionic bonding?

A

Ions of opposite charge held together by electrostatic attraction

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31
Q

What is ionic bonding between?

A

Metal and non metal

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32
Q

What are the properties of ionic bonding?

A

High melting and boiling points
Can conduct in liquid/aqueous state but not in a solid state
Soluble in polar solvents

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33
Q

Why does it have high meting and boiling points?

A

Because a large amount of energy is needed to overcome strong electrostatic attraction

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34
Q

Why is the melting point higher in certain ionic bonds?

A

Greater ionic charge in lattice = higher melting point

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35
Q

What must happen for ionic bonds to dissolve in polar solvents?

A

Ionic lattice must be broken down

Water molecules must attract and surround the lattice

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36
Q

What is an example of a polar solvent?

A

Water

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37
Q

What does solubility depend on in ionic bonding?

A

An attraction between the ions and water molecules

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38
Q

What happens as the ionic charge increases?

A

The solubility decreases

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39
Q

Why can ionic bonds conduct electricity when liquid or molten?

A

Because ions are free to move therefore there is charge carries so it can conduct electricity

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40
Q

Why can’t sometimes ionic bonds be dissolved in water?

A

Because the ionic attraction is too strong

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41
Q

What is covalent bonding?

A

Atoms that share a pair of electrons held together by intermolecular forces

42
Q

What is it called when a pair of electrons aren’t shared with the other element?

A

Lone pair

43
Q

What is it called when a covalent bond does that have a full amount of electrons?

A

Electron defieicent

44
Q

What is an example of an electron deficient covalent bond?

A

Borontrifluoride BF3

45
Q

What rule is broken when a covalent bond is electron deficient?

A

Octet rule

46
Q

When is it okay for the octet rule to be broken?

A

When there is more than 8 electrons in the covalent bond because the 3rd shell can hold 18

47
Q

What is a dative bond?

A

A bond formed when both electrons in the share are donated by one atom

48
Q

What is an example of a dative bond?

A

When ammonia acts as a base and reacts with H+ so donates both its electrons to the H+ to form ammonium

49
Q

When drawing covalent ions what do you represent the extra electron as?

A

A little triangle

50
Q

What are the properties of covalent bonding?

A

Low melting and boiling points
Insoluble in polar solvents
Doesn’t conduct electricity

51
Q

Why does covalent bonds have a low melting and boiling points?

A

Small covalent molecules

Weak intermolecular forces

52
Q

Why are covalent bonds insoluble in polar solvents but are in non-polar solvents?

A

Because london forces form between the solvent and the molecules

53
Q

Why does covalent bonds not conduct electricity?

A

Because there is no mobile charges so no charge carries so can’t conduct

54
Q

What is the VSEPR Theory?

A

The shape of a molecule/ion is determined by the no. of electron pairs in the outer shell of the central atom, repelling as far away as possible

55
Q

What does VSEPR stand for?

A 
Valence
Shell
Electron
Pair
Repulsion
56
Q

What shape is formed when there is two regions?

A

Linear

57
Q

What is the bond angle of a linear molecule?

A

180 degrees

58
Q

What is the shape formed when there is three regions>/

A

Trigonal planar

59
Q

What is the bond angle of a trigonal planar molecule?

A

120 degrees

60
Q

What shape is formed when there is four regions?

A

Tetrahedron

61
Q

What is the bond angle of a tetrahedron molecule?

A

109.5 degrees

62
Q

What shape is formed when there is six regions?

A

Octahedron

63
Q

What is the bond angle of an octahedron molecule?

A

90 degrees

64
Q

What is the shape formed when there is 5 regions?

A

Trigonal bi-pyramid

65
Q

What is the bond angles of a trigonal bi-pyramid?

A

90 and 120 degrees

66
Q

What shape is formed when there is 3 bonding pairs and 1 lone pair?

A

Pyramidal

67
Q

What shape would you think it would be there was 3 BP and 1 LP and why does this shape not form?

A

Tetrahedron as there is 4 electron pairs

But the lone pair aren’t attracted to the nuclei so they repel a further 2.5 degrees

68
Q

What is the bond angle of a pyramidal molecule?

A

107 degrees

69
Q

Why doe lone pairs have a greater repulsion?

A

Because there aren’t attracted to the nuclei

70
Q

How much does lone pairs reduce the bond angle by?

A

2.5 degrees

71
Q

What shape is formed when there is 2 bonding pairs and 2 lone pairs?

A

Non-linear

72
Q

What is the bond angle of a non-linear molecule?

A

104.5 degrees

73
Q

What is electronegativity?

A

A measure of the tendency of an atom to attract a bonding pair of electrons within a covalent bond

74
Q

What happens to electronegativity across a period?

A

It increases

75
Q

Why does electronegativity increase across a period?

A

Nuclear charge increases so there is a greater nuclear attraction so electronegativity increases

76
Q

What happens to electronegativity down a group?

A

It decreases

77
Q

Why does electronegativity decrease down a group?

A

The size of the atom increases so shielding of the outer shell increases so nuclear attraction reduces so electronegativity decreases

78
Q

What happens in a bond between different atoms when one element is more electronegative?

A

The electrons will attracts towards the more electronegative element
Will have a S- charge

79
Q

What happens to the other element in the bond when the other is more electronegative?

A

It will lose a small amount of electron density

Will have a S+ charge

80
Q

What is S-?

A

A (slight charge) delta

81
Q

When are molecules polar?

A

When the dipoles are in the same direction

82
Q

When are molecules non-polar?

A

When dipoles are symmetrical (opposite direction) so they cancel each other out

83
Q

What does it mean when there is no difference between electronegativity?

A

It is a non-polar covalent bond

84
Q

What does it mean when there is a small difference between electronegativity?

A

It is a polar covalent bond

85
Q

What does it mean when there is a large difference between electronegativity?

A

It is an ionic bond

86
Q

What is the size of a small difference?

A

0-1.8

87
Q

What is the size of a large difference?

A

> 1.8

88
Q

What are intra-molecular forces?

A

Strong bonds inside of molecules

89
Q

What are intermolecular forces?

A

Forces that act between different molecules and are much weaker than covalent bonds

90
Q

What are the three types of forces and their relative strength?

A

London forces - 1
Hydrogen forces - 50
Permanent dipole-dipole - 10

91
Q

What is a dipole-dipole force?

A

A weak attractive force between permanent dipoles in neighbouring polar molecules

92
Q

Where does dipole-dipole happen?

A

Attraction between two delta charges of elements

93
Q

How do london forces work?

A

Moving electrons = changing dipole
Instantaneous dipole induces dipole on neighbouring molecule
Induced dipole induces further dipole
They attract each other

94
Q

What happens to london forces as the no.of electrons increase?

A

Strength of london forces increase due to the larger instantaneous dipole created

95
Q

What are the anomalous properties of water?

A 
Elevated melting + boiling point
Ice floats (solid is less dense than the liquid)
96
Q

Why does water have an elevated boiling + melting point?

A

Because of strong hydrogen bonds

97
Q

Why does ice float?

A

Because when water freezes its molecules arrange themselves in a “more open, regular, lattice structure”

98
Q

Where does the hydrogen bond form?

A

Between the S+ and S- of two dipoles

99
Q

What are you doing when you’re boiling/melting water?

A

Breaking the hydrogen bonds

100
Q

When can hydrogen bonding only happen?

A

When hydrogen is covalently bonded to fluorine, nitrogen or oxygen

A-Level Chemistry (26 decks)

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