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Chemistry unit 2 GCSE > 1.) Topic 1 Bonding, structure and properties > Flashcards

1.) Topic 1 Bonding, structure and properties Flashcards

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1
Q

What is ionic bonding?

A

Ionic bonding is the bonding between a metal and non metal

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2
Q

What does it mean by malleable?

A

Can be bent into different shapes

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3
Q

What does it mean by ductile?

A

Can be stretched into wires

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4
Q

What is covalent bonding?

A

Bonding between non metals e.g. hydrogen and oxygen

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5
Q

Arrangement of electrons are:

A

2,8,8,4 maximum

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6
Q

In ionic bonding do metals gain or lose electrons

Do non-metals gain or lose electrons

A

Metals lose electrons and non metals gain electrons

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7
Q

Ionic compounds are made up of billions of oppositely charged ions held together in a giant structure. What’s this structure called?

A

A Crystal lattice

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8
Q

In ionic bonding, ions held together by ___________ forces

A

By strong electrostatic forces

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9
Q

In ionic bonding, in a lattice the ions are packed very tightly together. Does it take little or lots of energy to pull the ions apart?

A

Lots of energy because they are held together by strong electrostatic forces

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10
Q

Do ionic compounds conduct electricity when you melt or dissolve them and why?

A

Yes because the ions are free to move

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11
Q

Why do covalent compounds have low melting and boiling points?

A

Because they are made up of simple molecules with weak forces existing between them

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12
Q

Do covalent compounds conduct electricity?

A

No because they have no ions or free of electrons to carry charge

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13
Q

Do covalent compounds dissolve in water?

A

No because water attracts molecules that have charged ions and covalent molecules don’t have charged ions

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14
Q

How does covalent bonding work?

A

By sharing electrons

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15
Q

Name 8 properties of metals

A
  1. Good conductors of heat and electricity
  2. Malleable
  3. High melting and boiling points
  4. React with oxygen to form basic oxides
  5. Shiny when polished
  6. Lustrous
  7. High density
  8. Ductile
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16
Q

Name 4 properties of non metals

A
  1. Don’t conduct electricity or heat-insulators
  2. Low melting points
  3. Not malleable
  4. Not ductile
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17
Q

In metallic bonding are the metals ions positive or negative and what are they surrounded by?

A

Made up of positive metal ions in a sea of electrons

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18
Q

What does it mean by delocalised electrons?

A

Electrons which are not attached to one particular ion

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19
Q

Why do metals conduct heat and electricity?

A

Because they have a sea of electrons which are delocalised

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20
Q

List 2 uses of aluminium

A

Foil for wrapping things and electrical transmission lines

aero plane parts, cans, foil, window frames etc…

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21
Q

Describe the structure and bonding in a metal

A

Metals are made up of a giant structure of positive ions surround by a sea of delocalised electrons. The attraction between the two is called a metallic bond

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22
Q

Why does copper conduct electricity?

A

Because the electrons are delocalised. Able to move about

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23
Q

Why is copper ductile?

A

Because the ions can slide over each other

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24
Q

Why does magnesium have a higher melting point than sodium
Mg - 650°c
Na - 98°c

A

Because magnesium is a harder metal with more delocalised electrons. Also magnesium has a greater charge on ion and a stronger metallic bond

25
Q

What are allotropes and give examples

A

Different structural forms of the same elements and diamond and graphite are allotropes of carbon

26
Q

In diamond

how are the atoms are arranged?

Giant or small structure?

Strong or weak bonds?

Ionic or covalent bonds?

A

Tetrahedrally

Giant structure

Strong

covalent bonds between the atoms

27
Q

Does diamond have free electrons?

Does diamond conduct electricity?

A

Diamond has no free electrons

It don’t conduct electricity

28
Q

Would it take little or lots of energy to break the bonding in diamond and why

A

Lots of energy because there are many strong covalent bonds

29
Q

Name 4 uses of diamond

A

Ends of drills
Cutting tools
Jewellery
Diamond top saws

30
Q

Graphite it made up of ______ layers of carbon atoms

A

Hexagonal layers

31
Q

In graphite are the hexagonal layers held together by weak or strong forces

A

Weak

32
Q

There are ______ _______ bonds between the carbon atoms. This gives its the property to having a _____ melting point.

A

Strong covalent bonds between the carbon atoms. This gives it a HIGH melting point

33
Q

Name some properties of graphite and how does it have these properties

A

Soft and used as a lubricant because the layers can slide over each other as there are no covalent bonds between them

34
Q

Name 3 uses of graphite

A

Used in pencils
Electrolysis and electrodes
Lubricants

35
Q

Why is diamond hard and has a high melting point?

A

Giant structure with lots of covalent bonds in all directions so it takes lots of energy to break the bonds

36
Q

Why is graphite soft and feel greasy?

A

Because it is arranged hexagonally with weak forces between the layers so layers can slide over each other

37
Q

What is graphene?

A

Just one layer of the graphite molecule. Consists of a single layer of carbon atoms that are bonded together in a hexagonal honeycomb lattice

38
Q

What is nanotechnology?

A

The study and use of extremely small substances, often called Nano particles

39
Q

What is the size scale to be classed as a Nano particle

A

Between 1-100 nm in diameter

40
Q

Nanoparticles have ______ properties to the substance in its _____ state

A

Different properties to the substance in its bulk state

41
Q

What 3 properties does nano-silver have?

A

Antiviral, anti fungal and anti bacterial properties

42
Q

Where is nano sized silver used and why?

A

Plasters, deodorants, linings of fridges, lining of socks. It kills bacteria

43
Q

Give a use of nanoparticles which contain Titanium Dioxide

A

Sunscreen contains nanoparticles of titanium dioxide which absorb and reflect UV rays from the sun

44
Q

Why are nanoparticles of titanium dioxide used in self cleaning glass?

A

Glass is coated with nano particles which catalyse the breakdown of dirt in presence of UV light and also cause water to spread out in a thin film, rather than forming droplets on the surface

45
Q

Risks of nanoparticles x2

A

Long terms effects are unknown and so small there is a concern it can be absorbed into the skin

46
Q

What are smart materials?

A

Smart materials are a range of substances whose properties change with a change in the surroundings

47
Q

What are Thermochromic pigments and where are they used?

A

Thermochromic pigments change colour due to temperature and can be found in t shirts, coffee mugs and baby spoons

48
Q

What are photochromic pigments and where are they used?

A

Photochromic pigments change colour with changes in light intensity and they can be used as security markers and transition lenses

49
Q

What are shape memory alloys and where are they used?

A

Shape memory alloys are materials which can bend or twist when cool but when you heat them up they regain their original shape. They can be used for coffee pots, surgical plates and electrical devices

50
Q

What are the 2 types of shape polymers?

A

1) shape memory polymers

2) hydrogels

51
Q

What are shape memory polymers and where are they used?

A

When heated, the polymer returns to rests original shape and they are found somewhere between thermoplastics and thermosetting plastics. They are found in plastic car bodies

52
Q

What is shape retention?

A

Shape retention is when reheating a polymer it returns to its original shape

53
Q

What do polymer hydrogels do?

A

They have the ability to expose or absorb water if subjected to conditions such as temperature changes, pH changes and salt concentration

54
Q

How many times more can hydrogels swell up than its volume?

A

1000 times it’s volume

55
Q

Where are hydrogels found? x5

A

Disposable nappies, artificial muscles, drug delivery, robotic arms and fire fighting

56
Q

What is the reason why polymer and hydrogels work?

A

Because they have an open structure so the polymer is cross linked and this means that liquid molecules such as water molecules can get trapped in their structure. This allows the polymer to swell and later burst

57
Q

What do you need to conduct electricity?

A

You need free electrons

58
Q

Why is aluminum malleable? [4]

A

Aluminum is made up of a giant structure of positive (Al3+) surrounded by a sea of delocalized electrons. The attraction between the two is called the metallic bond. Aluminum is malleable as the ions can slide over each other

Chemistry unit 2 GCSE (6 decks)

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