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A-Level Edexcel Chemistry Flashcards > 2:Bonding and Structure > Flashcards

2:Bonding and Structure Flashcards

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1
Q

What is ionic bonding?

A

The electrostatic attraction between oppositely charged ions

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2
Q

What is the formula for hydroxide ion?

A

OH−

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3
Q

What is the formula for nitrate ion?

A

NO3^-

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4
Q

What is the formula for ammonium ion?

A

NH4 ^+

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5
Q

What is the formula for sulphate ion?

A

SO4^2-

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6
Q

What is the formula for carbonate ion?

A

CO3^2-

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7
Q

What are the features of giant ionic structures?

A
  • regular structure
  • cubic shape
  • giant repeating patterns
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8
Q

Give an example of a giant ionic structure?

A

NaCl

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9
Q

Why can ionic compounds dissolve in water?

A

Water molecules are polar, so they attract the anions and cation which break up the structure

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10
Q

Why can ionic structures conduct electricity when molten or dissolved in a solution?

A

The ions are free to move around.

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11
Q

Why do ionic compounds have high melting points?

A

There are many strong electrostatic forces between oppositely charged ions
- therefore more energy is needed to overcome these forces

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12
Q

Why are ionic compounds brittle?

A

When struck with a hammer the layers slide - so the cations align with cations and anions align with anions. They repel each other and the structure breaks apart

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13
Q

Why does the size of the charge increase the strength of the ionic bond?

A

The bigger the charge of the ion the stronger the electrostatic attraction between ions.
- Therefore more energy is required to overcome these forces

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14
Q

Why does the size of the ion (ionic radius) affect the strength of the ionic bond?

A

The smaller the ion the stronger the electrostatic attraction between the ions
-> smaller ions can pack together more closely so more energy is required to overcome these strong forces

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15
Q

Which ions have the highest charge density?

A

Ions with smaller radius and higher charge

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16
Q

Why does ionic radius increase as you go down a group?

A

Number of electrons shell increases

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17
Q

Why does the ionic radius in isoelectric ions decrease as atomic number increases?

A

More protons for the same number of electrons so attractive force from nucleus increases

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18
Q

Describe the experiment to show evidence for charged particles?

A

Electrolysis of copper(II)chromate(VI) on wet filter paper

  • add a drop of green copper(II)chromate(VI) is placed on wet filter paper and electricity is passed through (to separate the ions)
  • Positive Blue Cu2+ ions move to cathode
  • Negative Yellow CrO4^2- ions move to anode
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19
Q

What is covalent bonding?

A

The electrostatic attraction between a shared pair of electrons of two non-metal atoms and their nuclei

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20
Q

What are dative bonds (co-ordinate bonds)?

A

Covalent bond where the shared pair of electrons comes from one atom

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21
Q

What happens to bond enthalpy the shorter the bond?

A

The bond enthalpy will be higher

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22
Q

What two forces are acting in a covalent bond?

A
  • attraction - between shared pair of electrons and positive nuclei
  • repulsion - between like charged electrons and like charged nuclei
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23
Q

What is bond length a result of?

A

The balance between the attraction and repulsion force in a covalent bond.

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24
Q

How does a greater electron density cause high bond enthalpy?

A

There is a stronger attraction force so atoms are pulled closer towards each other. This leads to shorter bond length which results in higher bond enthalpy.

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25
Q

Why does the C-C triple bond have a higher bond enthalpy than a C-C single bond?

A

C-C triple bond has a higher electron density shared, so there is a shorter bond
* - so there is a higher bond enthalpy*

26
Q

Why do molecules have specific shapes?

A
  • Bonds repel each other equally as they contain electrons so they will want to be as far apart as possible
27
Q

What is the shape of a molecule with 2 bond pairs and 0 lone pairs?

A

Linear

28
Q

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

A

Trigonal planar

29
Q

What is the shape of a molecule with 4 bond pairs and 0 lone pairs?

A

Tetrahedral

30
Q

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

A

Trigonal Bipyramidal

31
Q

What is the shape of a molecule with 6 bond pairs and 0 lone pairs?

A

Octahedral

32
Q

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

A

Trigonal pyramidal

33
Q

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

A

V-shaped

34
Q

What are the properties of graphite?

A

1) each carbon has 3 bonds with one delocalised electron
2) conduct electricity and thermal energy
3) layers slide over each other
4) lightweight
5) insoluble

35
Q

Why can graphite transfer thermal energy and conduct electricity?

A

Delocalised electrons

36
Q

Why can the layers of graphite slide over each other?

A

There are weak forces between the layers

37
Q

Why is graphite lightweight?

A

Layers are far apart compared to its covalent bond length. This means it has a low density and therefore lightweight

38
Q

Why is graphite insoluble?

A

Covalent bonds are too strong to break

39
Q

What are the properties of diamond?

A

1) each carbon atoms has 4 bonds
2) can conduct heat well
3) very high melting point
4) doesn’t conduct electricity
5) insoluble
6) same structure as SiO2

40
Q

Why can diamond conduct heat well?

A

It’s tightly packed, in a rigid arrangement

41
Q

Why can’t diamond conduct electricity but graphite and grapheme can?

A

Diamond doesn’t have any delocalised electrons to conduct or transfer energy

42
Q

Why is diamond insoluble?

A

Covalent bonds are too strong to break

43
Q

What are the properties of graphene?

A

1) it is a single layer of graphite (so it’s 1 atom thick)
2) made up of hexagonal carbon rings
3) lightweight and transparent
4) contains delocalised electrons which strengthen the covalent bonds

44
Q

Why is graphene lightweight and transparent?

A

Because it’s one atom thick

45
Q

What is metallic bonding?

A

The strong electrostatic attraction between the nuclei of metal cations and delocalised electrons

46
Q

What increases the melting point in metallic bonding?

A

More electrons being donated to the sea of delocalised electrons

47
Q

Why do metal compounds have a high melting point?

A

Due to strong electrostatic attraction between cations and delocalised electrons which require a high amount of energy to overcome

48
Q

Why are metal compounds insoluble?

A

Due to strong metallic bonds

49
Q

Why are metal compounds malleable and ductile?

A

Ion layers can slide across each other and still retain an attraction between cations and delocalised electrons

50
Q

What is electronegativity?

A

The ability for an atom to attract electrons towards itself in a covalent bond

51
Q

What is the most electronegative element, according to the Pauling Scale?

A

Fluorine

52
Q

What scale do we use to determine electronegativity?

A

The Pauling Scale

53
Q

What does a bigger difference in electronegativity between atoms mean?

A

The more ionic the compound will be

54
Q

What does it mean if a bond is polar?

A

There is a significant difference in electronegativity between atoms
- the bigger the difference in electronegativity the more polar the bond will be

55
Q

What makes a covalent bond non-polar?

A

When atoms have the same/similar levels of electronegativity.
- e.g. hydrocarbons are non-polar

56
Q

Order the intermolecular forces from strongest to weakest (1 being the strongest).

A

1) Hydrogen bonds
2) Permanent dipole - dipole
3) London forces

57
Q

When does hydrogen bonding occur?

A

When hydrogen on one molecule forms a bond with the lone pair of either oxygen,fluorine or nitrogen

58
Q

What is permanent dipole-dipole ?

A

The δ- of one permanent dipole molecule is attracted to the δ+ of another

59
Q

What are London forces?

A

Forces that occur when the δ+ of a temporary dipole molecule is attracted to the δ- of another

60
Q

What is the difference between bonds and forces?

A

Forces occur between molecules
Bonds occur between atoms

A-Level Edexcel Chemistry Flashcards (4 decks)

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