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Chemistry > 1.3 Bonding > Flashcards

1.3 Bonding Flashcards

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1
Q

Metallic bonding

A

The attraction between delocalised outer shell electrons and positive metal ions in a lattice

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2
Q

How are the metal ions arranged

A

Packed close together in layers in a regular way

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3
Q

What are the metal ions surrounded by

A

Mobile electrons

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4
Q

What do mobile electrons do

A

Move freely within structure

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5
Q

What does delocalised mean

A

Displaced from where it’s expected to be

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6
Q

What does giant mean

A

A huge structure- consisting of millions and millions of atoms

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7
Q

What does the number of delocalised electrons depend on

A

How many electrons are lost from each metal atom

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8
Q

What is ionic bonding

A

The electrostatic attraction between oppositely charged ions in a lattice

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9
Q

Where does ionic bonding occur

A

Between metals and non metals

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10
Q

What happens in ionic bonding

A

Electrons are transferred from a metal to a non metal

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11
Q

What is formed as a result of ionic bonding

A

Positive and negative ions

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12
Q

What do metal atoms do

A

Lose electrons and become positively charged

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13
Q

What do non metals do

A

Gain electrons and become negatively charged

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14
Q

What is the charge on a simple ion related to

A

It’s position in the periodic table

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15
Q

What ion is formed from group 1 elements

A

+1

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16
Q

What ion is formed from group 2 elements

A

+2

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17
Q

What ion is formed from group 3 elements

A

+3

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18
Q

What ion is formed from group 5 elements

A

-3

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19
Q

What ion is formed from group 6 elements

A

-2

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20
Q

What ion is formed from group 7 elements

A

-1

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21
Q

What does boron not do

A

Form ions (covalently bonds)

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22
Q

Do carbon and silicon usually form ions?

A

No

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23
Q

What can transition elements do

A

Form more than one stable ion

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24
Q

What are compound ions

A

Covalently bonded species carrying a charge

Eg. Hydroxide and carbonate

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25
Q

Covalent bond

A

Shared pair of electrons

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26
Q

Where does covalent bonding occur

A

Between atoms of non- metals

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27
Q

What is a pair of electrons which is not bonded called

A

A lone pair

28
Q

When is a double bond formed

A

When 2 pairs of electrons are shared

29
Q

When is a triple bond formed

A

When 3 pairs of electrons are shared

30
Q

What is a non- octet molecule

A

A molecule where the central atom doesn’t have a noble gas electron arrangement (8 electrons in a full shell)

31
Q

Coordinate/dative bonding

A

A covalent bond in which both electrons of the shared pair come from the same atom

32
Q

The atom that donates the electrons has a…

A

Lone pair

33
Q

The atom that accepts the electron pair does not have a full outer shell of electrons. It is…

A

Electron deficient

34
Q

How can coordinate bonds be shown

A

Using an arrow. The arrow points from the atom donating the electrons

35
Q

What happens once the coordinate bond is formed

A

It behaves like a normal covalent bond

36
Q

What 3 things is the shape of a molecule determined by

A

The total number of electron pairs around the central atom

The number of bonding pairs of electrons

The number of lone pairs of electrons

37
Q

What can the shape of molecules be predicted by

A

The electron pair repulsion theory

38
Q

What does the electron pair repulsion theory state

A
  • pairs of electrons repel each other so they they are as far apart as possible
  • lone pairs repel slightly more than bonded pairs because they’re more compact
  • the molecule or ion takes up a shape which minimises these repulsions
  • each lone pair reduces the bond angle by 2.5 degrees
39
Q

How to draw a bond in the plain of the paper

A

A line

40
Q

How to draw a bond coming out of the paper

A

A wedge

41
Q

How to draw a bond going into the paper

A

A dotted line

42
Q

What are compound ions

A

Covalently bonded species carrying a charge

43
Q

What shape is a molecule with 2 bond pairs and no lone pairs

A

Linear

44
Q

What is the bond angle of a linear structure

A

180

45
Q

What is the shape of a molecule with 3 bond pairs and 0 lone pairs

A

Trigonal planar

46
Q

What is the bond angle of a trigonal planar

A

120

47
Q

What is the name of the molecule with 4 bond pairs and 0 lone pairs

A

Tetrahedral

48
Q

What is the bond angle of a tetrahedral structure

A

109.5

49
Q

What shape is the molecule with 5 bond pairs and 0 lone pairs

A

Trigonal bipyramidal

50
Q

What are the bond angles for a trigonal bipyramidal structure

A

90 and 120

51
Q

What is the shape of a molecule with 6 bond pairs and no lone pairs

A

Octahedral

52
Q

What is the bond angle for an octahedral structure

A

90

53
Q

What is the bond angle in an octahedral structure

A

90

54
Q

Do bonding pairs of electrons in double/triple bonds repel in the same way

A

Yes so the shape and bond angle are the same

55
Q

What is the shape of a molecule with 2 bond pairs and 1 lone pairs

A

Bent v-shaped

56
Q

What is the bond angle of a bent v shaped molecule with 1 lone pair

A

118

57
Q

What is the shape of the molecule with 3 bond pairs and 1 lone pair

A

Pyramidal

58
Q

What is the bond angle of a pyramidal structure

A

107

59
Q

What is the shape of the molecule with 2 bond pairs and 2 lone pairs

A

V shaped

60
Q

What is the bond angle of a v shaped molecule with 2 lone pairs

A

104.5

61
Q

Why is the bond angle smaller for a v shaped molecule with 2 lone pairs than a v shaped molecule with 1 lone pair

A

More repulsion

62
Q

What is the shape of a molecule with 3 bond pairs and 2 lone pairs

A

Trigonal planar

63
Q

What is the bond angle of a trigonal planar

A

120

64
Q

What is the shape of a molecule with 4 bond pairs and 2 lone pairs

A

Square planar

65
Q

What is the bond angle in a square planar

A

90

66
Q

What happens when an atom forms a coordinate bond

A

The shape changes as the number of bonding and lone pairs change

67
Q

Why does the shape of a molecule change when a coordinate bond forms

A

Bond pairs repel less than lone pairs so bond angle increases slightly

Chemistry (42 decks)

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