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Chemistry Paper 1 > Strcuture and Bonding > Flashcards

Strcuture and Bonding Flashcards

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1
Q

Whtat are the three strong chemical bonds?

A

Ionic, covalent and metallic

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2
Q

For ionic bonding the particles are …

A

Oppositely charged ions

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3
Q

For covalent bonding the particles are …

A

Atoms which share pairs of electrons

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4
Q

For metallic bonding the particles are …

A

Atoms which share delocalised electrons

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5
Q

Ionic bonding occurs in compounds formed from …

A

Metals combined with non-metals

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6
Q

Covalent bonding occurs in …

A

Most non-metallic elements and compounds of non-metals

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7
Q

Metallic bonding occurs in …

A

Metallic elements and alloys

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8
Q

The diagram for ionic bonding is …

A

Dot and Cross Diagram

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9
Q

Ionic bonding is the ——– of electrons

A

Transfer

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10
Q

Covalent bonding is the ——- of pairs of electrons

A

Sharing

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11
Q

Metal atoms —- electrons to become ———- charged ions

A

Lose
Positively

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12
Q

Non-metal atoms —- electrons to become ———- charged ions

A

Gain
Negatively

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13
Q

Which groups of metals undergo ionic bonding to achieve a full outer shell?

A

Groups 1 and 2
Groups 6 and 7

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14
Q

What is an ionic compound?

A

A giant structure of ions

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15
Q

How are ionic compounds held together?

A

Strong electrostatic forces of attraction between oppositely charged ions

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16
Q

Which ionic compound’s strcuture does this describe?
“Each sodium ion is surrounded by six chloride ions, and each chloride ion is surrounded by six sodium ions”

A

Sodium chloride

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17
Q

Ionic compounds form a ——- structure

A

Giant ionic lattice

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18
Q

Make this molecular formula an empirical formula
“C2H4”

A

CH2

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19
Q

Covalently bonded substances have —– bonds

A

Strong

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20
Q

Covalently bonded substances may consist of —– molecules

A

Small

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21
Q

Polymers have very —– molecules

A

Large

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22
Q

Diamond and Silicon Dioxide are …

A

Giant covalent molecules

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23
Q

Diamond is formed from the element ——

A

Carbon

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24
Q

In diamond, each carbon atom is covalently bonded to - other carbon atoms

A

4

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25
Q

What are the properties of diamond?

A

Doesn’t conduct electricity
Very high melting point
Very hard

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26
Q

Why can’t diamond conduct electricity?

A

It has no free electrons to carry a charge because all outer electrons are in covalent bonds

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27
Q

Silicon dioxide can be referred. to as ——

A

Silica

28
Q

What are the properties of silica?

A

Hard
High melting point

29
Q

What is silicon dioxide made up of?

A

Silicon and oxygen atoms covalently bonded

30
Q

In silica, each silicon atom is bonded to - oxygen atoms

A

4

31
Q

Try to draw dot and cross diagrams for the molecules of hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia and methane

A

…

32
Q

The advantage of a dot and cross diagram is …

A

It is very clear where the electrons are coming from

33
Q

The disadvantage of a dot and cross diagram is …

A

It doesn’t show the shape of a molecule

34
Q

2D stick diagrams are bad because …

A

They do not show the shape of a molecule
It is unknown which electron came from which atom

35
Q

The advantage of a ball and stick diagram is …

A

It allows us to clearly see the ions in three dimensions

36
Q

A space filling diagram is good because …

A

It more accurately shows how closely packed each ion is

37
Q

Ball and stick diagrams, and space filling diagrams are misleading in regards to the —- of a giant ionic lattice

A

Size

38
Q

Metals consist of —– ———- of atoms arranged in a ——- pattern

A

Giant structures
Regular

39
Q

Outer shell electrons of metal atoms are ———–

A

Delocalised

40
Q

Delocalised electrons are free …

A

To move through the whole strcuture

41
Q

Strong metallic bonds are formed from …

A

The sharing of delocalised electrons

42
Q

A delocalised electron is an electron that is not …

A

Connected to a single atom or a covalent bond (free to move)

43
Q

What are the limitations of the particle model?

A

There are no forces
All particles are spheres
All particles are solid

44
Q

Give the 4 state symbols

A

s - solid
l - liquid
g - gas
aq - aqueous

45
Q

Ionic compounds conduct electricity when … because …

A

Melted or dissolved in water because the ions are free to move

46
Q

The larger the molecule, the —— the melting and boiling point

A

Higher

47
Q

Atoms in polymers are linked with …

A

Strong covalent bonds

48
Q

Polymers are —– at room temperature

A

Solids

49
Q

The strucutre of a polymer is typically shown as a …

A

Long chain

50
Q

Diamond and graphite are forms of what?

A

Carbon

51
Q

Graphene is …

A

A single layer of graphite and has properties that make it useful in electronics and composites

52
Q

What structure is diamond?

A

Giant covalent structure

53
Q

In diamond, each carbon atom forms how many bonds?

A

Four covalent bonds with other carbon atoms

54
Q

In graphite, each carbon atom forms how many bonds

A

Three covalent bonds with three other carbon atoms

55
Q

What shaped rings are formed in graphite?

A

Hexagonal rings with no covalent bonds between the layers

56
Q

How many electrons are delocalised in graphite

A

One from every carbon atom

57
Q

Definition of graphene

A

A single layer of graphite with useful properties for electronics and composites

58
Q

What was the first fullerene to be discovered?

A

The buckminsterfullerene

59
Q

What is a cylindrical fullerene?

A

A carbon nanotube (very high length to diameter ratio)

60
Q

What are carbon nanotubes useful for?

A

Nanotechnology, electronics and materials

61
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

62
Q

How does the size of a cube affect the surface area to volume ratio?

A

As the side length decreases, SA to volume ratio increases

63
Q

How small is a nanometre?

A

1 x 10^-9 m

64
Q

List of applications of nanoparticles

A

Medicine, electronics, cosmetics, sun creams, deodorants and catalysts

65
Q

What is a disadvantage of nanoparticles?

A

They can interact wih cells inside our body that cause health problems

Chemistry Paper 1 (6 decks)

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