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Chemistry > Booklet 2 - bonding > Flashcards

Booklet 2 - bonding Flashcards

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1
Q

What are bonds?

A

They are the glue that holds atoms together

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2
Q

What happens to atoms when they react to form chemical bonds?

A

They either lose, gain or share electrons.

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3
Q

What are the three types of bonding?

A

Ionic, covalent, and metallic

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4
Q

What happens to electrons in ionic bonds? What does it take place between?

A

They electrons are lost or gained

Metal and non metals

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5
Q

What happens to electrons in covalent bonds? What does it take place between?

A

Electrons are shared in pairs

Non metals and non metals

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6
Q

What happens to electrons in metallic bonds? What does it take place between?

A

Electrons are shared as a cloud (delocalised)

Same metal with same metal

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7
Q

What happens to a metal when it reacts in ionic bonding? What does it get called?

A

It loses 1 electron in order to form a full outer shell and then has a overall charge of 1+.
Forms a positve ion.

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8
Q

What happens to a non-metal when it reacts in ionic bonding? What does it get called?

A

It gains one electron to form a full outer shell

Forms a negative ion.

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9
Q

What’s the link between metals and non-metals in ionic bonding? (electrons)

A

Metals lose their outer electrons to non-metals, so they each form full outer shells

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10
Q

How do metals and non metals attract to form ionic bonds?

A

The metals form positively charged ions and the non metals form negatively charged ions.
These oppositely charged ions attract by a force of electrostatic atttraction.

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11
Q

What do the millions of Na+1 and Cl-1 bonds in a Nacl salt crystal form?

A

A Giant ionic Lattice

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12
Q

What is a Giant Ionic Lattice?

A

All ionic compounds have this structure.

  • have high melting and boiling points due strong bonds between ions
  • have strong electrostatic forces of attraction between oppositely charged ions
  • they dissolve easily in water, so ions separate and can carry current
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13
Q

How many Cl-1 ions bond with one Na+1 ions? What does it do to the structure? And what does it give? What holds the particles together?

A

6 CL-1 ions bond, it makes the structure extremely strong and gives the NaCl a very high melting point of 801degrees
Strong electrostatic forces hold the particles together

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14
Q

What does a substance require to conduct electricity?

A

Charged particles which are free to move

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15
Q

When does NaCl conduct electricity? What happens?

A
  • When dissolved in water or when it is melted

- the ionic bonds and lattice break, the ions then are free to move and conduct electricity

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16
Q

What do non-metals require? Why?

A

Non-Metals are short of electrons and require electrons to obtain a full outer shell

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17
Q

How is a covalent bond made?

A

Non metals can gain extra electrons by sharing electron pairs with other non-metals and this forms a strong covalent bond

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18
Q

What does metallic bonding occur between?

A

Metals and metals

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19
Q

What do metals have in metallic bonding?

A

electrons in the outer shell of the metal are delocalised, so there are strong forces of electrostatic attraction between the positive metal ions and shared negative ions

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20
Q

Why do metals usually have high boiling and melting points?

A

The electrostatic attractions between electrons and positive ions; these are stong attractions which are difficult to break, and that is why metals are usually hard with high boiling and melting points.

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21
Q

Why can metals be bent or shape?

A

The layers are able to slide over each other

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22
Q

What are alloys?

A

when pure metals are too soft for many uses they’re mixed with other metals to make alloys which are harder

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23
Q

What happens to the different sized atoms of the added metal? (Alloys)

A

Its distorts the layers in the structure, making it more difficult to slide over each other and so makeballoys harder than pure metals

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24
Q

Why is pure gold rarely used in jewellery?

A

It is soft and will easily lose its shape and can be scratched easily.

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25
Q

What do the forces between solid particles require?

A

A large amount of heat energy to melt the solid into a liquid, therefore having a large melting point.

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26
Q

What do some covalent substances contain?

A

Very weak attractive forces between the molecules, called intermolecular bonds, it is these weak forces that break when the covalent substances melts.

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27
Q

What is another phrase for intermolecular forces?

A

Van der wals forces

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28
Q

What happens to the intermolecular forces with the size of the molcule?

A

The forces increase, the greater the force the higher its melting and boiling points.

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29
Q

What can atoms that share electrons also form? Give 3 Examples?

A

They can form giant covalent structures, e.g silicon dioxide (sand), diamond, graphite

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30
Q

What are allotropes? Give examples

A

Different forms if the same element eg diamond, graphite, graphene and fullerenes are forms of carbon

31
Q

what are the properties of diamond?

A

Form four bonds which makes diamond very hard with a high melting point, and doesnt conduct electricity as it has no free electrons or ions

32
Q

In Graphite, each carbon atom bonds covalently to how many other atoms? What does it form and make Graphite?

A

Bonds covalently to three others carbon atoms

  • forming layers of hexagonal rings with no covalent bonds
  • giving graphite a high boiling point as it needs lots of energy to break the layers.
  • one electron from each carbon is delocalised
33
Q

Why is Graphite soft and slippery?

A

The layers are free to slide over each other because there are no covalent bonds between the layers, only weak intermolecular forces.

34
Q

Why does Graphite conduct heat and electricity?

A

One electron from each carbon is delocalised allowing graphite to conduct

35
Q

How thick is Graphene?

A

graphene is a sheet of carbon joined together in hexagons, its one atom thick, making it two dimensional

36
Q

Why is graphene useful in electronics?

A

It conducts electricity as delocalised electrons can run through the whole structure

37
Q

Why is Graphene a very strong light-weight material with a higher tensile than steel?

A

It has strong covalent carbon carbon bonding
- network of covalent bonds making it strong, its also light so can be added to composite materials to improve their strength without adding weight

38
Q

What are the properties of fullerenes?

A

Made of molecules of carbon atoms with hollow shapes.
- The structure is based in hexagonal rings of carbon atoms but they also may contain rings with five or seven carbon atoms

39
Q

What was the first fullerene to be discovered?

A

Buckministerfullerene C60

40
Q

What are carbon nanotubes?

A

Cylindrical fullerenes with a very high length to diameter ratio

41
Q

What are the characteristics of carbon nanotubes?

A

Have high tensile strength, high conductivity, and high thermal conductivity

42
Q

Why are Fullerenes said to adopt a simple molecular structure?

A

They are generally too small to be classed as having a giant covalent structure

43
Q

Where are carbon nanotubes used?

A

Nano-technology, electronics, and materials

44
Q

What can general fullerenes be used for?

A

Drug delivery into the body, as lubricants and catalysts

45
Q

What does nanoscience refer too?

A

Structures that are 1-100m in size, of the order of a fee hundred atoms.

46
Q

What are nanoparticles smaller than?

A

Smaller than fine particles which are called particulate matter (PM2.5) which have diameters between 100 and 2500nm

47
Q

What are coarse particles called? What are their diameters? What are they referred as?

A

PM10, have larger diameters between 2.5x10-6m and 1x10-5m. Referred to as dust.

48
Q

What are 8 applications of nanoparticles?

A 
In medicine for controlled drug delivery,
Synthetic skin
Electronics
Cosmetics
Sun creams
In the developments of new catalysts for fuel cells materials
Deodorants
Fabrics to prevent growth of bacteria
49
Q

Why is titanium oxide used in suncream?

A

The nanoparticles are so small they cannot reflect visible light, they CAN reflect the harmful U.V rays without making skin go white

50
Q

What are the 2 advantages of nanoparticles in suncream?

A

Better skin coverage

More effective protection from suns rays

51
Q

What are the 2 Dis-advantages of nanoparticles in suncream?

A

Potential cell damage i.e breathing in particles harm lungs

Harmful effects on environment

52
Q

What are the properties of simple molecular structures?

A
  • strong covalent bonds
  • low melting and boiling points - as the weak intermolecular forces can be broken down easily
  • non conductive- due to not having free electrons to move around
53
Q

What are the properties of ionic compounds?

A
  • all have high melting and boiling points due to strong bonds between the ions, it takes a lot of energy to overcome this attraction
  • they have regular structures (giant ionic lattice) in which there are strong electrostatic forces of attraction between oppositely charged ions
54
Q

When can ionic compounds conduct electricity?

A

When the compounds melt, the ions are free to move and they’ll carry electrical current
- they also dissolve easily in water, so the ions separate and move and carry current

55
Q

Why are covalenr bonds strong?

A

The positively charged nuclei of the bonded atoms are attracted to the shared pair of the electrons by electrostatic forces making them strong

56
Q

What are simple molecular substances?

A

Made up of molecules containing a few atoms joined together by covalent bonds

57
Q

What are the properties of simple molecular substances?

A
  • they have very strong covalent bonds but weak intermolecular forces
58
Q

How do you melt of boil a simple molecular substance?

A

Need to break the weak intermolecular forces and not the covalent bonds. So melting and boiling point are very LOW

59
Q

Do simple molecular substances conduct electricity?

A

No as they aren’t charged so there no free electrons or ions

60
Q

What are the limitations of using dot and cross diagrams?

A

They show how ionic compounds are formed. But they dont show the structure of the compound, the size of the ions or how they’re arranged

60
Q

What do sharing of delocalised electrons in metallic bonding do?

A

They hold the forces of attraction of the atom together in a regular structure and the bonding is vwry strong

60
Q

Why do most compounds with metallic bonds have high melting and boiling points?

A

The electrostatic forces between the metal atoms and the delocalised sea of electrons are very strong, so need lots of energy to be broken

61
Q

What three things does a state of a object depend on?

A

How strong the forces of attraction are between the particles of the material eg temperature, pressure and material

62
Q

What are the properties of a liquid?

A
  • weak forces of attraction, they’re randomly arranged and are free to move past each other
  • liquids dont keep a definite shape
  • particles are constantly moving with random motion - hotter the liquid faster they move
63
Q

What are the properties of a gas?

A
  • force of attraction is very weak, they’re free to move far apart
  • gases don’t keep define shape or volume and will fill containers
  • particles move constantly with random motion, hotter the gas the faster they move
64
Q

What are the properties of a solid?

A
  • strong forces of attraction which holds them together in fixed positions
  • the particles dont move and keep definite shape and volume
  • particles vibrate about their positions - hotter the solid becomes the more they vibrate
65
Q

What are the properties of giant covalent structures?

A
  • solids with high melting points & boiling points that are linked to other atoms by strong covalent bonds
  • bonds must be overcome to melt or boil the substances
  • don’t contain charged particles, so they can’t conduct electricity
66
Q

What are examples of giant covalent structures?

A

Diamond, graphite and silicon dioxide

67
Q

what are the properties of nanoparticles?

A
  • they have a huge surface area to volume ratio
  • some conduct electricity so they can be used in tiny electric circuits for computer chips
  • also used in cosmetics, eg they are used to improve moisturisers without making them really oil
68
Q

how are nanoparticles used in Nanomedicine?

A

the idea that tiny particles are absorbed more easily by the body than most particles. this means they deliver drugs right into the cells where they are needed

69
Q

what are silver nanoparticles?

A

they have antibacterial properties, they can be added to polymer fibres that are used to make surgical masks and wound dressings, they can also be added to deodorants

70
Q

what are people concerned about in nanoparticles?

A
  • some worry that products containing nanoparticles have been made available before the effects on human health have been investigated properly, and that we don’t know what the long term impacts on health will be
71
Q

what precaution is taken with nanoparticles?

A
  • people believe that particles containing nanoscale particles should be clearly labelled, so that consumers can choose whether or not to use them

Chemistry (12 decks)

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