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

Physical Chapter 3: Bonding Flashcards

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
How do Charge clouds interact with each other?
They repel each other, forming the molecule shape
26
What atom shape will be formed when the central atom has 2 electron pairs? What is its bond angle?
Linear - 180 degrees
27
What atom shape will be formed when the central atom has 3 electron pairs? What is its bond angle?
Trigonal planar - 120 degrees
28
What atom shape will be formed when the central atom has 4 electron pairs & 0 lone pairs? What is its bond angle?
Tetrahedral - 109.5 degrees
29
What atom shape will be formed when the central atom has 4 electron pairs & a lone pair? What is its bond angle?
Trigonal Pyramidal - 107 degrees
30
What atom shape will be formed when the central atom has 4 electron pairs & two lone pairs? What is its bond angle?
Bent/V-Shaped - 104.5 degrees
31
What atom shape will be formed when the central atom has 5 electron pairs & no lone pairs? What is its bond angle?
Trigonal Bipyramidal - 90 & 120 degrees
32
What atom shape will be formed when the central atom has 5 electron pairs & 1 lone pair? What is its bond angle?
Seesaw - 102 degrees
33
What atom shape will be formed when the central atom has 5 electron pairs & 2 lone pairs? What is its bond angle?
T-shaped: 88 degrees
34
What atom shape will be formed when the central atom has 6 electron pairs & no lone pairs? What is its bond angle?
Octahedral - 90 degrees
35
What atom shape will be formed when the central atom has 6 electron pairs & two lone pairs? What is its bond angle?
Square planar - 90 degrees
36
What is electronegativity?
The ability of an element to pull the bonding pair of electrons towards itself.
37
What is the effect of elctronegativity on covalent bonds?
They will become polar
38
What intermolecular forces occur in substances with polar bonds?
Dipole-dipole forces
39
What are the three types of IMFs?
Dipole-Dipole forces VdW forces Hydrogen bonding
40
What are Van der Walls' forces?
Electron movement causes temporary dipoles, causing attraction between molecules.
41
What causes VdW force strength to increase?
Larger electron clouds Shape of molecule - longer straight chains are better
42
What IMFs hold together ionic lattices such as Iodine?
Covalent bonds keep the I2 together, while VdW forces keep the molecules together.
43
What is the order of strength of IMFs?
Hydrogen bonds > Dipole-dipole > VdW forces
44
When does Hydrogen bonding occur?
When hydrogen is covalently bonded to flourine, nitrogen, or oxygen.
45
How does Hydrogen bonding occur?
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
What effect does hydrogen bonding have on properties of substances?
They will have higher boiling & melting points H-bonding can cause the solid to be less dense than the liquid - H2 and ice.
47
What structure do metal elements exist as?
Giant metallic lattice structures
48
How does Metallic bonding explain high melting point of metals?
Strong electrostatic attraction between positive metal ions & delocalised electrons More delocalised electrons - higher M.P. (Na has lower mp than Mg)
49
How does metallic bonding explain conductivity of metals?
Dolecalised electrons can move to carry charge or heat
50
How does metallic bonding explain their insolubility?
The bonds are strong, so the metal is insoluble.
51
Which bonds are broken during melting & boiling?
IMFs - not covalent bonds
52
What affects the physical properties of a solid?
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
Is the boiling/melting point of Ionic substances high or low?
High
54
What state are ionic substances at room temp?
Solid
55
Do ionic substances conduct electricity?
only when in liquid
56
Are ionic substances soluble in water?
Yes
57
Are simple covalent substances soluble in water?
This depends on the polarisation of the molecule
58
Do simple covalent substances have high or low mp/bp?
Low - don't have to break covalent bonds, just IMFs
59
Do simple covalent substances conduct electricity?
No
60
Do giant covalent substances conduct electricity?
No (except graphite)
61
Do giant covalent structures have low or high mp/bp?
High
62
WHat state are simple covalent structures at room temp?
Generally liquid or gas, but can be solid like I2
63
What state are giant covalent structures at room temp?
Solid
64
What state are metallic substances at room temp?
Solid
65
Do metallic substances generally have high or low mp/bp?
High
66
Can metallic substances conduct electricity?
Yes - liqud and solid
67
Are metallic substances soluble in water?
No
68
Are giant covalent substances soluble in water?
No

AQA A Level Chemistry (25 decks)

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