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Chemistry - Paper 1 > Structure And bonding > Flashcards

Structure And bonding Flashcards

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1
Q

What is are the 3 states of matter ?

A

Solids, liquids and gasses .

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2
Q

What is extremely hard to do in a solid ?
Why is this ?
With almost no ….

A

Solids are really hard to compress.

This is because the particles are packed together in a regular pattern.With almost no spaces between the particles.

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3
Q

What kind of structure to solids have ?

Why is this ?

A

Solids have a fixed structure that
cannot flow from place to place .
This is because solids can vibrate but not move form place to place.

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4
Q

How are solids similar to liquids ?

Why is this ?

A

Just like liquids solids are extremely hard to compress.

This is because the particles are very close together with not many spaces between them.

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5
Q

How are liquids different to solids?

Why?

A

unlike solids , liquids take the shape of their container and flow from place to place.This is because the particular in a liquid can move.

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6
Q

How compressible are gasses ?why?

How do gases react in a container ?

A

Gasses are extremely easy to compress.
This is because the particles in gases are widely spaced .
Gases fill the space of their container.
This is because the Particles also in gas move quickly and randomly.

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7
Q

How do you change the state of a substance ?

A

You change a state of a substance by putting in or taking out energy.

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8
Q

What happens as a solid changes state to a liquid ?

Who has more Kinetic energy the particles in a liquid or solid ?

A

It’s called melting .

The particles in a liquid are moving around so they have more kinetic energy than a solid .

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9
Q

How do we break the forces of attraction in a solid ?

A

We break the forces of attraction in a solid by using energy .

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10
Q

What do we need to put in to convert a solid into a liquid ?

A

Energy

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11
Q

The stronger the forces of attraction …

And the higher…

A

The stronger the forces of attraction between the particles the more energy we’ve got to put in to break them .
And the higher the melting point .

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12
Q

What melting point does a candle wax have ?

A

Candle wax has a relatively low melting point .
This is because the forces of attraction between particles are relatively weak
So their fairly easy to break.

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13
Q

Converting a liquid back into a solid

A

Freezing

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14
Q

How do we convert a liquid into a gas

A

By boiling

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15
Q

How do we convert a gas back into a liquid ?

A

By condensing

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16
Q

What is the first limitation of the particle model ?

A

The first limitation is that the model assumes all particles are solid spheres .

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17
Q

What is the second limitation of the particle model ?

A

Secondly it assumes that there are no forces between the particles .

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18
Q

What is the structure of an ionic compound ?
What is every positive ion surrounded by ?
And what does this apply for ?

A

Ionic compounds have giant ionic lattices

Every positive ion is surrounded by a negative ion and vice versa .

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19
Q

What dimension do giant ionic lattices have ?

A

Giant ionic lattices are 3 dimensional

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20
Q

What do giant ionic lattices have ?

A

Giant ionic lattices have strong forces of attraction between positive and negative electrons.
Scientists call this electrostatic forces

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21
Q

What can electrostatic forces be called ?

A

Ionic bonds

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22
Q

What are the melting and boiling points of ionic compounds?

Why?

A

Ionic compounds have very high melting and boiling points.

This is because the strong electrostatic forces require a great deal of heat energy to break them .

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23
Q

What can ionic compounds not do when they are solid?

Why ?

A

Ionic compounds can’t conduct electricity when they are solid
This is because the ions cannot move they are locked in place by the strong electrostatic forces of attraction .

24
Q

When can ionic compounds conduct electricity ?

A

Ionic compounds can conduct electricity when they are molten or dissolved in water
That’s because ions can move and carry a charge .

25
Q

What happens to the electrons outer shell in an ionic bonding ?

A

The outer electron are transferred from the metal atom to the non metals atom.

26
Q

What is covalent bonding

A

When non metal atoms bond together

27
Q

What do scientists call the covalent bond diagram .

What does a single line represent ?

A

Energy level diagrams

A single covalent bond
Shared pair of electrons

28
Q

What happens in covalent bonding?

A

Atoms share an electron

29
Q

What do covalent bonds take place in?

What is a covalent bond .

A

Covalent bond take place between non metals.

A covalent bond is a shared pair of electron.

30
Q

What do small covalent molecules have ?

A

Small covalent molecules have low melting and boiling points
This is because they have very weak intermolecular forces .

31
Q

Giant covalent molecules are always …
Giant covalent molecules have millions of ….
Giant covalent molecules always have high melting and boiling points

A

Giant covalent molecules are always solid at room temperature
Giant covalent molecules have millions of strong covalent bonds.
Their always have high melting and boiling point

32
Q

What is diamond formed from?

A

Diamond is formed from the element carbon

33
Q

What does each carbon atom form ?
What do diamond have huge numbers of ?
When are these Brocken ?
What does this require?

A

Each carbon atom forms four strong covalent bonds .
Diamonds have a huge number of covalent bonds and these have to be Brocken when diamond is melted.
This requires a great deal of energy.

34
Q

What can diamond not do ?

Why ?

A

Diamond cannot conduct electricity .

There are no free electrons to carry electrical charge.

35
Q

What is the melting point of silicon ?

Why ?

A

Silicon has a very high melting point .

A huge number of strong covalent bonds must be Brocken and this takes a great deal of energy .

36
Q

What are the melting and boiling points to graphite?

How does graphite feel?

A

Graphite has a high melting and boiling point .
Graphite is soft and slippery
Graphite is an excellent conductor of heat and electricity

37
Q

What is graphite formed form ?

A

Graphite is formed from the element carbon .

Each carbon atom forms three covalent bonds .

38
Q

What shape do the carbon atoms form in graphite ?and how are they arranged ?
What do they have and how does this make graphite slippery ?

A

Carbon atoms form hexagonal rings ,Arranged in layers.There are no covalent bonds between the layers so they can slide this makes graphite slippery.

39
Q

What does graphite have a high melting and boiling point?

A

Because graphite has many strong covalent bonds, it takes a great deal of energy to break these bonds so graphite has a high melting and boiling point .

40
Q

What are delocalised electrons ?

A

Delocalised electrons can move .This means they can conduct thermal electricity and energy .

41
Q

How is graphite different to a metal ?
How is graphite similar to metal ?
(2 reasons)

A

Graphite is based on the element carbon so graphite is not a metal. Graphite is similar to metals as both graphite and metals are good conductors of electricity and heat .
Both graphite and metals have delocalised electrons that can move .

42
Q

How is graphene different to graphite

A

Graphene is a single layer of graphite .graphene is one thick atom.

43
Q

What graphene a good conductor of ?

How strong is graphene ?

A

Graphene is a good conductor of electricity because it has delocalised electrons .
Graphene is extremely strong .

44
Q

What shape do fullerene have ?

3 descriptions

A

Fullerene are molecules of carbon atoms with a hollow shape.
Usually fullerene has hexagonal rings of carbon atoms .
Fullerene also have rings of five or seven carbon atom.

45
Q

What are the uses of fullerene ?

3 uses

A

Pharmaceutical delivery
Lubricants
Catalyst

46
Q

What do carbon nanotubes have ?

What are they excellent conductors of ?

A

Carbon nanotubes have high tensile strength.

Carbon nano tubes are excellent conductors of heat and electricity .

47
Q

What kind of material are carbon nanotubes in ?

A

Carbon nanotubes are used in re enforcing materials such as tennis rackets

48
Q

What are the arrangements of metals ?

A

Metals are arranged in a giant structure of atoms arranged in a regular layers.
The electrons in the outer energy levels of each atoms are delocalised .

49
Q

Bonding in metals

What is metallic bond ?

A

We have a strong electrostatic attraction between the sea of delocalised negative electrons and positive metal ions .
Scientist call the electrostatic attractions in metals bonds are strong

50
Q

Why do metals have a strong boiling and melting point ?

A

Metals have a high melting and boiling points because a great deal of energy is required to break the strong metallic bonds .

51
Q

Why are metals a excellent conductor of heat and electricity ?

A

Metals are excellent conductors of heat and electricity because the delocalised electrons can move .

52
Q

What does it mean that the delocalised electrons can move ?

A

Because they are charged these moving electrons can carry an electrical current

53
Q

How can metals conduct heat

A

The moving electrons can carry thermal energy which allows allows metals to conduct heat

54
Q

How are metals shaped?

A

Metals can be bent and shaped

In metals the layers of atoms are able to slide over each other .

55
Q

What is an alloy

A

An alloy is a mixture of metals
The different sizes of atoms distorts the layers making it more difficult for them to slide over each other.
Alloys are harder than pure metals

Chemistry - Paper 1 (6 decks)

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