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AQA A Level Chemistry S4L > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is a dative covalent/co-ordinate bond?

A

A covalent bond where the pair of electrons originates from one atom.

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2
Q

What two conditions are there for a dative covalent/co-ordinate bond to occur?

A

The atom donating the pair must have a lone pair, and the atom accepting must have a vacant orbital

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3
Q

What are the 3 main types of bonding?

A

Ionic, metallic, covalent

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4
Q

An arrow can be used to show a dative bond. What does the direction the arrow is pointing show?

A

Points from the atom donating to the atom accepting

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5
Q

Between what type of atoms does metallic bonding occur?

A

metal + metal

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6
Q

What does metallic bonding involve?

A

Attraction between delocalised electrons and positive ions arranged in a lattice

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7
Q

‘Electrostatic forces between positive ions and delocalised outer electrons’ describes what type of bonding?

A

Metallic

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8
Q

‘Electrostatic forces of attraction between positively and negatively charged ions’ describes what type of bonding?

A

Ionic

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9
Q

What is a covalent bond?

A

Where two atoms share one pair of electrons

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10
Q

What type of bond occurs between a non-metal + metal?

A

Ionic

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11
Q

What type of bond occurs between two non-metals?

A

Covalent

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12
Q

What is electronegativity?

A

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

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13
Q

What happens to electronegativity as you go across the period?

A

Electronegativity would increase as atoms get bigger but similar shielding, therefore stronger nuclear charge and so stronger attraction b/w nucleus and shared pair of electrons

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14
Q

What happens to electronegativity as you go down a group?

A

As you go down a group, atom size increases and so nuclear charge does as well, but because there is increased shielding there is overall a weaker attraction (less electronegative)

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15
Q

A polar covalent bond occurs when_____?

A

One atom = more electronegative than the other

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16
Q

What are the 3 main types of intermolecular forces?

A

Van der Waal’s, dipole-dipole, hydrogen bonds

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17
Q

What is the strongest type of intermolecular force?

A

Hydrogen bonds

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18
Q

What affects electronegativity?

A

The size of the nuclear charge

The size of the atom

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19
Q

What is a polar covalent bond?

A

When one atom is more electronegative than the other

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20
Q

What is the difference between an induced dipole vs polar molecules?

A

The dipoles in polar molecules are permanent. These can attract other permanent molecules with dipole-dipole forces

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21
Q

Dipole-dipole bonds occur between what types of molecules?

A

Polar

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22
Q

State what is meant by a ‘hydrogen bond’

A

The attraction between a lone pair on a N, O, or F and the slightly positive H on a neighbouring molecule

23
Q

What type of bonding occurs in NaCl and what is the resulting structure?

A

Ionic

Giant ionic lattice

24
Q

What are the four kinds of crystal structure?

A

Ionic, metallic, macromolecular, molecular

25
Q

What kind of crystal structure occurs in iodine?

A

Simple molecular

26
Q

What kind of crystal structure occurs in diamond?

A

Giant covalent

27
Q

What kind of crystal structure occurs in graphite?

A

Giant covalent

28
Q

What kind of crystal structure occurs in ice?

A

Simple molecular

29
Q

What kind of crystal structure occurs in magnesium?

A

Giant metallic lattice

30
Q

Describe and explain the features of a giant ionic lattice

A

High melting point - oppositely charged ions held together by strong electrostatic attractions
Brittle - if a layer shifts, similarly charged ions are to close, repel and cause the structure to break open
Most can dissolve in water - +ve and -ve ions can interact with polar water molecules
Can enable a current if dissolved/melted - electrons free to move, can create flow of ions

31
Q

Describe and explain the features of a simple molecular crystal

A

Strong covalent bonds in molecules
Weak intermolecular forces between
Low melting points
Don’t conduct - no free moving electrons

32
Q

Describe and explain the features of a giant covalent diamond structure

A

Tetrahedral shape
Hard -v. strong covalent holding together
High mp - strong covalent
Can’t conduct - no free moving electrons

33
Q

Describe and explain the features of a giant covalent graphite structure

A

Each C covalently bonded to 3 Cs
Soft - weak VdW between planes, so able to slide past
Can conduct across a plane but not between layers (delocalised within plane)

34
Q

Describe and explain the features of a giant metallic lattice

A

High melting point - strong attraction between ions and delocalised electrons
Dense - same as above -pulls it close
Can conduct - delocalised electrons
Good heat conductors - same as above
Malleable - layers can slide over each other

35
Q

What does VSEPR stand for?

A

Valence Shell Electron Pair Repulsion Theory

36
Q

How many atoms are attached to a linear molecule?

A

2

37
Q

How many atoms are attached to the central atom in a trigonal planar molecule?

A

3

38
Q

How many atoms are attached to the central atom in a tetrahedral molecule?

A

4

39
Q

How many atoms are attached to the central atom in a trigonal bipyramid molecule?

A

5

40
Q

How many atoms are attached to the central atom in an octahedral molecule?

A

6

41
Q

What are the bond angles in a linear molecule?

A

180

42
Q

What are the bond angles in a trigonal planar molecule?

A

120

43
Q

What are the bond angles in a tetrahedral molecule?

A

109.5

44
Q

What are the bond angles in a trigonal bipyramid molecule?

A

90 and 120

45
Q

What are the bond angles in an octahedral molecule?

A

90

46
Q

A molecule has 4 pairs in total, 3 bonding and 1 lone. What is the shape of the molecule?

A

Trigonal pyramid

47
Q

A molecule has 4 pairs in total, 2 bonding and 2 lone. What is the shape of the molecule?

A

V-shaped

48
Q

A molecule has 5 pairs in total, 3 bonding and 2 lone. What is the shape of the molecule?

A

T-shaped

49
Q

A molecule has 6 pairs in total, 4 bonding and 2 lone. What is the shape of the molecule?

A

Square planar molecule

50
Q

What are the bond angles in a trigonal pyramid molecule?

A

107

51
Q

What are the bond angles in a v-shaped molecule?

A

104

52
Q

What are the bond angles in a T-shaped molecule?

A

90

53
Q

What are the bond angles in a square planar molecule?

A

90

54
Q

What are the bond angles in an octahedral based molecule?

A

87

AQA A Level Chemistry S4L (34 decks)

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