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AS-Level Chemistry Unit 1 > 1.5 Solid Structures > Flashcards

1.5 Solid Structures Flashcards

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1
Q

What are two giant covalent structures?

A

diamond, graphite

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2
Q

What are diamond and graphite known as?

A

carbon allotropes

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3
Q

What are examples of physical properties?

A

boiling point
melting point
solubility
conductivity

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4
Q

What does allotrope mean?

A

different physical form of the same element

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5
Q

How many covalent bonds does carbon have?

A

4

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6
Q

What are the types of crystal structures?

A

ionic, metallic, simple molecular, giant covalent

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7
Q

What are ionic substances?

A

consists of a lattice of positive and negative ions held together by strong electrostatic forces
the alternating pattern in ionic substances maximise electrostatic attraction and minimise repulsion

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8
Q

What are examples of ionic substances?

A

sodium chloride and caesium chloride

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9
Q

What does coordination number mean?

A

number of oppositely charged ions which surround an ionic compound

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10
Q

What is the coordination number of sodium chloride?

A

6:6

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11
Q

Why does sodium chloride have a coordination number of 6:6?

A

6 sodium ions surround a single chloride ion
6 chloride ions surround a single sodium ion

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12
Q

What is the coordination number of caesium chloride?

A

8:8

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13
Q

Why does caesium chloride have a coordination number of 8:8?

A

8 caesium ions surround a single chloride ion
8 chloride ions surround a single caesium ion

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14
Q

Why does caesium chloride have a different coordination number to sodium chloride?

A

caesium ions are larger as it has a bigger atomic radium so it can fit more chloride ions around it, compared to sodium ions

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15
Q

What type of m.p/b.p do ionic substance have?

A

high

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16
Q

Why do ionic substance have high m.p/b.p?

A

it requires large amounts of energy to overcome the strong electrostatic forces between oppositely charged ions

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17
Q

What is electrical conductivity like in ionic substances?

A

in the solid structure the ions are fixed in position by the strong ionic bonds, therefore the ions are not free to move and carry current
whereas when molten, the ions separate and no longer held in a lattice, so they are free to move and carry a flow charge which is an electrical current

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18
Q

What is the strength in ionic substances?

A

Hard but brittle

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19
Q

Why are ionic substances hard but brittle?

A

opposingly charged ions are held together by strong electrostatic forces of attraction
if the structure is hit, the layers distort, breaking up the lattice into fragments

20
Q

What is the solubility of ionic substances?

A

very soluble

21
Q

Why are ionic substances soluble?

A

the polar nature of the water molecules are able to pull the ions apart due to opposite charges attracting

22
Q

What are metallic structures?

A

a lattice of positively charged ions surrounded by a sea of delocalised electrons
there are strong forces of attraction between these

23
Q

What are the m.p/b.p of metallic structures?

A

high

24
Q

Why do metallic structures have high m.p/b.p?

A

because large amounts of energy is needed to break up the strong forces of attraction between the positive ions and delocalised electrons

25
Q

Electrical conductivity- metallic structures?

A

good

26
Q

Why are metallic structures a good conductor of electricity?

A

cations are formed by donating valance electrons to form a sea of delocalised electrons
the negative charge is able to move and carry the flow of charge through the structure

27
Q

What is the strength of metallic structures?

A

strong but malleable and ductile

28
Q

Why are metals malleable and ductile?

A

it can change shape or be drawn into wires as the layer of positive ions are able to slide over one another, while still being attracted to the sea of delocalised electrons

29
Q

Are metals soluble?

A

no

30
Q

what are simple molecular structures?

A

consist of covalently bonded molecules held together by weak van der waal’s forces
these are the type of intermolecular force that act between the molecules holding them in structure

31
Q

What are examples of simple molecular structures?

A

iodine and ice

32
Q

What is the difference between intermolecular and intramolecular forces?

A

intermolecular- between molecules
intramolecular- within the molecule

33
Q

What is the structure of iodine?

A

consists of molecules of iodine held in a lattice by weak intermolecular forces called Van Der Waals, but has strong intramolecular forces called covalent bonds
vdw are much weaker than covalent bonds but are often strong enough to keep the substance in a solid/liquid state

34
Q

What is the structure of ice?

A

ice is less dense than water
water molecules are joined by weak hydrogen bonding, these forces stay rigid when when ice forms creating an open structure

35
Q

What type of m.p/b.p do simple molecular structures have?

A

low

36
Q

Why do simple molecular structures have low m.p/b.p?

A

not a lot of energy is required to break the weak vdw/ hydrogen forces

36
Q

Why do simple molecular structures have low m.p/b.p?

A

not a lot of energy is required to break the weak vdw/ hydrogen forces

37
Q

What is electric conductivity like in simple molecular structures?

A

poor

38
Q

Why do simple molecular structure have poor electric conductivity?

A

there are no free electrons within the structure to carry the flow of charge and the molecules are too far apart to conduct electricity

39
Q

What is the strength of simple molecular structures?

A

brittle

40
Q

Why are simple molecular structures brittle?

A

weak forces of attraction can be broken easily with little force

41
Q

What is the solubility of simple molecular structures?

A

slightly soluble

42
Q

Why are simple molecular structures slightly soluble?

A

water cannot form any attractions with a simple covalent structure

43
Q

What is the structre of graphite?

A

arranged in a hexagonal pattern forming a layered sheet structure
graphite only forms 3 of the 4 possible covalent bonds, therefore one electron is unpaired. this unpaired electron becomes delocalised and moves freely through the structure

44
Q

What is the structure of diamond?

A

tetrahedral structure and the 4 bonds formed by carbon are multi directional
eat carbon atom form 4 out of the 4 possible covalent bonds, leaving no spare electrons

45
Q

what are fullerenes?

A

AS-Level Chemistry Unit 1 (8 decks)

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