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Chemistry Y11 > Structures > Flashcards

Structures Flashcards

1
Q

Give four properties of giant Ionic lattices

A
  • soluble in water
  • high melting point
  • conducts electricity when liquid
  • crystalline
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2
Q

Give two examples of giant Ionic lattices

A

Sodium chloride

Magnesium oxide

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3
Q

Give four properties of simple Covalent / Covalent molecular structures

A
  • low melting and boiling points (tend to be mainly gases)
  • not soluble in water
  • do not conduct electricity
  • soft when solid
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4
Q

Give two examples of simple covalent / covalent molecular structures

A

Iodine and carbon dioxide

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5
Q

Give three properties of giant covalent structures

A
  • Very high melting and boiling point
  • Diamond does not conduct electricity, graphite and graphene do
  • insoluble in water
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6
Q

Give a property of Graphite

A

Slippery soft solid

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7
Q

Give a property of graphene

A

100 times stronger than steel but is very thin, light and inexpensive

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8
Q

Draw diamond

A

-

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9
Q

Draw Graphite

A

-

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10
Q

Draw and label Graphene

A

-

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11
Q

Give four properties of a giant metallic structure

A

High mpt/bpt
Conducts heat and electricity
Ductile (can be stretched into wires)
Malleable (bends)

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12
Q

List three main properties of Ionic compounds

A
  • crystalline
  • high melting point
  • conducts electricity when liquid
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13
Q

Sodium chloride conducts electricity when molten but not when solid, explain why?

A

The electrons have become delocalised and the ions are free to move and therefore carry charge

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14
Q

Why do ionic compounds have high melting and boiling points ?

A

Due to the strong electrostatic forces of attraction between oppositely charged ions which require a lot of energy to break

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15
Q

Why can’t some substances conduct electricity as a solid?

A

The ions are in a fixed position

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16
Q

Why do simple covalent structures/molecular covalent structures have low melting/boiling points?

A

Due to the weak forces of attraction between the molecules (van der Waals) despite that there are strong covalent bonds between the atoms in the molecule

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17
Q

Why does diamond not conduct electricity?

A

It has 4 carbon atoms surrounding each carbon atom and therefore has no free electrons

18
Q

Why does Graphite conduct electricity?

A

It has a free electron which can carry charge

19
Q

Why is Graphite slippery?

A

It is in forms of layers which can slide over each other due to weak van der Waals

20
Q

Why do some metallic structures have high melting points and boiling points?

A

Strong metallic bonds require a lot of energy to break

21
Q

Why do metallic structures conduct heat/electricity?

A

They have delocalised electrons which have a lot of kinetic energy to move and carry the charge/energy

22
Q

Why are metallic structures malleable?

A

The sea of electrons allows the layers of ions to slide over each other without disrupting the bonding when a force is applied

23
Q

How many atoms of carbon surround each carbon atom in Graphite?

A

3

24
Q

Why do diamond and Graphite both habe high melting points?

A

They have strong covalent bonds in all directions which require a lot of energy to break

25
Q

Which of graphite’s properties means that it can be used as a lubricant ?

A

It’s weak van der Waals enable layers to slide over one another

26
Q

Why is it that Graphite can conduct electricity?

A

Carbon is covalently bonded to three carbon atoms. This leaves one free electron per atom to carry current

27
Q

Lead is malleable because (2)

A
  • The result of tightly packed atoms cause the outer electrons to delocalised
  • and allow the layers of ions to slide over one another without disrupting the bonding
28
Q

Why can metals produce wire shapes?

A

They are ductile and have delocalised electrons which allow ions to slide over each other

29
Q

Define alloy

A

A mixture of two or more elements at least one of which is a metal, and the resulting mixture has metallic properties

30
Q

What is meant by the term ductile ?

A

Can be stretched into wires

31
Q

Explain fully how a single covalent bond forms

A

Shared pair of electrons

32
Q

Explain why metals conduct electricity

A

The electrons have become delocalised and the ions are free to move and therefore carry a charge

33
Q

Describe the bonding and structure in a typical metal like sodium. Use a labelled diagram

A

(Metal ions and free electrons from outer shells of metal atoms)
The bonding in metals is metallic and it gives a giant metallic lattice. The metallic bond is the attraction between regularly arranged positive metal ions and delocalised electrons

34
Q

Why does HCL have a low boiling point?

A

Weak van der Waals forces between the molecules, meaning there is little energy required to break the bonds

35
Q

Show the equation for working out the % of gold in an alloy

A

Number of carats divided by 24 x 100

35
Q

Use of diamond

A
  • Cutting of tools
35
Q

Draw a diagram of an alloy

A
  • Positive Ions
  • Different sized ions
  • Negative delocalised electrons
36
Q

Give an example of an alloy

A
  • Steel is an alloy of iron and carbon
37
Q

Why are alloys harder than metals (2)

A
  • The different sizes of atoms in an alloy distort the layers in the metallic structure
  • Making it more difficult for the layers of ions to slide over each other
38
Q

What is gold used in jewellery usually an alloy of ?

A
  • An alloy with silver, copper and zinc
39
Q

Uses of Graphene

A
  • Batteries

- Solar cells

Chemistry Y11 (9 decks)

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