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AQA A Level Chemistry > Physical Chapter 3: Bonding > Flashcards

Physical Chapter 3: Bonding Flashcards

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1
Q

What is a compound?

A

A molecule made up of different elements bonded together.

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2
Q

What are the two types of bonding in compounds?

A

Covalent and ionic.

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3
Q

What is an ionic bond?

A

A bond formed when one or more electrons are transferred from one atom to another.

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4
Q

What holds ionic bonds together?

A

Electrostatic attraction

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5
Q

What is the formula of a sulfate ion?

A

SO42-

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6
Q

What is the formula of a hydroxide ion?

A

OH-

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7
Q

What is the formula of a nitrate ion?

A

NO3-

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8
Q

What is the formula of a Carbonate ion?

A

CO32-

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9
Q

What is the formula of an Ammonium ion?

A

NH4+

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10
Q

What is the overall charge of any compound?

A

zero

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11
Q

What is the structure of Sodium Chloride?

A

Giant Ionic Lattice

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12
Q

How does Ionic structure explain coductivity of compounds when dissolved?

A

Ions in a solid are held in place by strong bonds, whereas they are free to move in liquids.

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13
Q

How does Ionic structure explain high melting point of ionic compounds?

A

Giant ionic lattices are held together by strong electrostatic forces.

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14
Q

How does Ionic structure explain solubility in water?

A

Water molecules are polar - these can pull ions away from the lattice, causing dissolution.

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15
Q

What is a covalent bond?

A

A bond that contains at least one shared pair of electrons.

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16
Q

What is another name for a giant covalent structure?

A

Macromolecular structure

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17
Q

What is a giant covalent structure?

A

A molecule made up of a huge network of covalently bonded atoms

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18
Q

What is the structure of graphite?

A

Sheets of hexagons with delocalised electrons

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19
Q

What are the properties of graphite?

A

Sheets can slide over each other - it’s a dry lubricant
electrically conductive
Low density - layers are far apart
High melting point - strong covalent bonds
Insoluble - bonds are too strong to break

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20
Q

What is the hardest known substance?

A

Diamond

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21
Q

What are properties of Diamond?

A

High Melting Point
It’s very hard
Good thermal conductor
Can’t conduct electricity
Insoluble in all solvents
Refracts light a lot

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22
Q

What is a dative covalent bond?

A

A bond where both electrons in a pair are donated from one molecule.

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23
Q

What does molecular shape depend on?

A

Electron pairs around the central atom

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24
Q

What is a charge cloud?

A

An area where an electron could be - electrons do not stay still

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25
Q

How do Charge clouds interact with each other?

A

They repel each other, forming the molecule shape

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26
Q

What atom shape will be formed when the central atom has 2 electron pairs?
What is its bond angle?

A

Linear - 180 degrees

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27
Q

What atom shape will be formed when the central atom has 3 electron pairs?
What is its bond angle?

A

Trigonal planar - 120 degrees

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28
Q

What atom shape will be formed when the central atom has 4 electron pairs & 0 lone pairs?
What is its bond angle?

A

Tetrahedral - 109.5 degrees

29
Q

What atom shape will be formed when the central atom has 4 electron pairs & a lone pair?
What is its bond angle?

A

Trigonal Pyramidal - 107 degrees

30
Q

What atom shape will be formed when the central atom has 4 electron pairs & two lone pairs?
What is its bond angle?

A

Bent/V-Shaped - 104.5 degrees

31
Q

What atom shape will be formed when the central atom has 5 electron pairs & no lone pairs?
What is its bond angle?

A

Trigonal Bipyramidal - 90 & 120 degrees

32
Q

What atom shape will be formed when the central atom has 5 electron pairs & 1 lone pair?
What is its bond angle?

A

Seesaw - 102 degrees

33
Q

What atom shape will be formed when the central atom has 5 electron pairs & 2 lone pairs?
What is its bond angle?

A

T-shaped: 88 degrees

34
Q

What atom shape will be formed when the central atom has 6 electron pairs & no lone pairs?
What is its bond angle?

A

Octahedral - 90 degrees

35
Q

What atom shape will be formed when the central atom has 6 electron pairs & two lone pairs?
What is its bond angle?

A

Square planar - 90 degrees

36
Q

What is electronegativity?

A

The ability of an element to pull the bonding pair of electrons towards itself.

37
Q

What is the effect of elctronegativity on covalent bonds?

A

They will become polar

38
Q

What intermolecular forces occur in substances with polar bonds?

A

Dipole-dipole forces

39
Q

What are the three types of IMFs?

A

Dipole-Dipole forces
VdW forces
Hydrogen bonding

40
Q

What are Van der Walls’ forces?

A

Electron movement causes temporary dipoles, causing attraction between molecules.

41
Q

What causes VdW force strength to increase?

A

Larger electron clouds
Shape of molecule - longer straight chains are better

42
Q

What IMFs hold together ionic lattices such as Iodine?

A

Covalent bonds keep the I2 together, while VdW forces keep the molecules together.

43
Q

What is the order of strength of IMFs?

A

Hydrogen bonds > Dipole-dipole > VdW forces

44
Q

When does Hydrogen bonding occur?

A

When hydrogen is covalently bonded to flourine, nitrogen, or oxygen.

45
Q

How does Hydrogen bonding occur?

A

The hydrogen has its electrons pulled away by the F/N/O and the bond becomes polar.
These polar bonds will then form intermolecular bonds with lone pairs on other polar molecules.

46
Q

What effect does hydrogen bonding have on properties of substances?

A

They will have higher boiling & melting points
H-bonding can cause the solid to be less dense than the liquid - H2 and ice.

47
Q

What structure do metal elements exist as?

A

Giant metallic lattice structures

48
Q

How does Metallic bonding explain high melting point of metals?

A

Strong electrostatic attraction between positive metal ions & delocalised electrons
More delocalised electrons - higher M.P. (Na has lower mp than Mg)

49
Q

How does metallic bonding explain conductivity of metals?

A

Dolecalised electrons can move to carry charge or heat

50
Q

How does metallic bonding explain their insolubility?

A

The bonds are strong, so the metal is insoluble.

51
Q

Which bonds are broken during melting & boiling?

A

IMFs - not covalent bonds

52
Q

What affects the physical properties of a solid?

A

Strength of attraction between its particles - melting/boiling points
Type of particles it contains - solubility
Prescence of charged particles that are free to move - conductivity

53
Q

Is the boiling/melting point of Ionic substances high or low?

A

High

54
Q

What state are ionic substances at room temp?

A

Solid

55
Q

Do ionic substances conduct electricity?

A

only when in liquid

56
Q

Are ionic substances soluble in water?

A

Yes

57
Q

Are simple covalent substances soluble in water?

A

This depends on the polarisation of the molecule

58
Q

Do simple covalent substances have high or low mp/bp?

A

Low - don’t have to break covalent bonds, just IMFs

59
Q

Do simple covalent substances conduct electricity?

A

No

60
Q

Do giant covalent substances conduct electricity?

A

No (except graphite)

61
Q

Do giant covalent structures have low or high mp/bp?

A

High

62
Q

WHat state are simple covalent structures at room temp?

A

Generally liquid or gas, but can be solid like I2

63
Q

What state are giant covalent structures at room temp?

A

Solid

64
Q

What state are metallic substances at room temp?

A

Solid

65
Q

Do metallic substances generally have high or low mp/bp?

A

High

66
Q

Can metallic substances conduct electricity?

A

Yes - liqud and solid

67
Q

Are metallic substances soluble in water?

A

No

68
Q

Are giant covalent substances soluble in water?

A

No

AQA A Level Chemistry (25 decks)

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