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Chemistry gcse > Bonding, Structure And Properties Of Matter > Flashcards

Bonding, Structure And Properties Of Matter Flashcards

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1
Q

Ions

A

Charged particles

Full outer shells

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2
Q

Metal forming ions

A

Lose electrons from outer shell to form positive ions

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3
Q

Non metals forming ions

A

Gain electrons into outer shell to form negative ions

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4
Q

Ionic bonding

A

Metal and non metal
Metal atom loses electrons and non metal gains these electrons
These oppositely charged ions are strongly attracted to one another by electrostatic forced

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5
Q

Ionic compounds

A

Have giant ionic lattice structure
Ions form a closely packed regular lattice arrangement and there are very strong electrostatic forces of attraction between oppositely charged ions in all directions in the lattice

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6
Q

Ionic compound properties

A

High melting and boiling points due to many strong bonds between ions
Takes lots of energy to overcome this attraction
When solid ions are held in place so can’t conduct electricity
Dissolve easily in water
Ions separate and are all free to move in the solution so they’ll carry electric current

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7
Q

Covalent bonding

A

Non metal atoms bond together
Share electrons
The positively charged nucleus of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces, making covalent bonds very strong

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8
Q

Properties of simple molecular substances

A

Substances containing covalent bonds usually have simple molecular structures
The atoms within the molecules are held together by very strong covalent bonds
The forever of attraction between these molecules are very weak
Low melting and boiling point because all you have to do is break the feeble intermolecular forces
Mostly gases or liquids at room temp
Intermolecular forces get stronger as molecules get bigger
Don’t conduct electricity because they aren’t charged so there’s no free electrons or ions

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9
Q

Polymers

A

Lots of small units linked together to form a long molecule that had repeating sections
All atoms are joined by strong covalent bonds
Intermolecular forces between polymer molecules are larger than between simple covalent bonds so more energy is needed to break them meaning most are solid at room temp
Intermolecular forces are still weaker than ionic or covalent bonds so have lower boiling points than ionic or giant molecular compounds

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10
Q

Giant covalent structures

A

All atoms are bonded to each other by strong covalent bonds
High MP and BP as a lot of energy is needed to break covalent bonds between the atoms
Don’t contain charged particles so don’t conduct electricity
Diamond, graphite, silicon dioxide

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11
Q

Diamond

A

Each carbon atom forms four covalent bonds in a very rigid giant covalent structure

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12
Q

Graphite

A

Each carbon atom forms three covalent bonds to create layers of hexagons
Each carbon atom also has one delocalised electron

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13
Q

Silicon dioxide

A

Silica
What sand is made of
Each grain of sand is one giant structure of silicon and oxygen

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14
Q

Allotropes

A

Different structural forms of the same element in the same physical state

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15
Q

What are allotropes of carbon?

A

Diamond
Graphite
Graphene
Buck minster fullerene

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16
Q

Diamond properties

A

has a giant covalent structure, made up of carbon atoms that each form four covalent bonds This makes diamond really hard
Those strong covalent bonds take a lot of energy to break and give diamond a very high melting point
It doesn’t conduct electricity because it has no free electrons or ions.

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17
Q

Graphite properties

A

in graphite, each carbon atom only forms three covalent bonds creating sheets of carbon atoms arranged in hexagons.
There aren’t any covalent bonds between the layers - they’re only held together weakly, so they’re move over each other. This makes graphite soft and slippery, so it’s ideal as a lubricating material.
Graphite’s got a high melting point-the covalent bonds in the layers need loads of energy to break.
Only three out of each carbon’s four outer electrons are used in bonds, so each carbon atom has one electron that’s delocalised (free) and can move. So graphite conducts electricity and thermal energy.

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18
Q

Graphene properties

A

Graphene is a sheet of carbon atoms joined together in hexagons.
The sheet is just one atom thick, making it a two-dimensional compound.
The network of covalent bonds makes it very strong.
It’s also incredibly light, so can be added to composite materials to improve their strength without adding much weight.
Like graphite, it contains delocalisesd elecrons so can conduct electaicity through the whole structure. This means it has the potential to be used in electronics.

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19
Q

Fullerenes

A

Molecules of carbon shaped like closed tubes or hollow balls
Mainly made up of atoms arranged in hexagons but can also contain pentagons or heptagons
They can be used to cage other molecules
This could be used to deliver as drug into the body
Have huge surface areas so could help make great industrial catalysts - individual catalysts could be attached to the fullerenes
Also make great lubricants

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20
Q

Buckminster fullerene

A

C60

Forms a hollow sphere containing 20 hexagons and 12 pentagons

21
Q

Nanotubes

A

1) Fullerenes can form nanotubes -tiny carbon cylinders.
The ratio between the length and
the diameter of nanotubes is very high
Nanotubes can conduct both ectricity and thermal energy (heat)
They also have a high tensile strength (‘they don’t break when they’re stretched)
Technology that uses very small particles such as nanotubes is called nanotechnology.
Nanotubes can be used in electronics or to strengthen materials without adding much weight such in tennis racket frames.

22
Q

What substances have high melting and boiling points due to strong bonds?

A

Ionic compounds, metals and giant covalent structures

23
Q

Why does ions bonding work?

A

Because they end up with opposite charges so attract

24
Q

What is a metallic bond?

A

The attraction between the positive ions and the delocalised electrons

25
Q

What is the structure of a metal?

A

A giant lattice in which electrons are delocalised (not bound to one atom)

26
Q

What causes a metal to have a giant lattice structure?

A

The delocalised electrons causes there to be positive ions. It is held together by the electrostatic forces between the delocalised electrons and the positive ions

27
Q

Why do metals have high mp and bps?

A

Because metallic bonds are strong and so need a lot of energy to overcome them

28
Q

Why are metals good thermal and electrical conductors?

A

Because the delocalised electrons can move around freely and transfer energy

29
Q

Why can lure metals be easily shaped?

A

The particles have a regular arrangement so the layers can easily slide over each other

30
Q

What’s an alloy?

A

Mixtures that contain a metal and at least one other element

31
Q

Why do we use alloys?

A

Pure metals are too soft for many purposes

32
Q

Why are alloys harder than pure metals?

A

Because adding another element disrupts the regular arrangement so the layers don’t slide over each other

33
Q

Solid properties

A

Strong forces of attraction between particles
Regular lattice arrangement, fixed positions
Keep definite shape and volume
Particles vibrate about their positions the hotter the solid becomes
Expand slightly when heated

34
Q

Liquid properties

A

Weak force of attraction between particles
Randomly arranged particles and free to move past each other but tend to stick closely together
Definite volume but don’t keep definite shape
Will flow to fill bottom of container
Particles constantly moving with random motion
Hotter the liquid the faster they move
Liquids expand slightly when heated

35
Q

Gas properties

A

Very weak force if attraction between particles
Free to move and are far apart
Gas particles travel in straight lines
Don’t keep definite volume or shape
Will always fill any container
Particles move constantly with random motion
Hotter the gas - faster they move
Gases either expand when heated or their pressure increases

36
Q

Solid to liquid

A

Melting

37
Q

Liquid to gas

A

Boiling

38
Q

Gas to liquid

A

Condensing

39
Q

Liquid to solid

A

Freezing

40
Q

Aqueous meaning

A

Dissolved in water

41
Q

Diameter of coarse particles

A

Between 1x10-5 m and 2.5x10-6 m

42
Q

Diameter of fine particles

A

Between 1x10-7 m and 2.5x10-6 m

43
Q

Diameter of nanoparticles

A

Between 1x10-9 and 1x10-7

44
Q

How many atoms do nanoparticles contain?

A

Only a few hundred

45
Q

Why are smaller particles effective catalysts?

A

They have a high surace area:volume ratio

46
Q

How are the required properties /effects of nanoparticles achieved?

A

Each individual atom can be placed in the correct position

47
Q

Why are nanoparticles used in sun cream?

A

They help to provide better coverage hence protecting skin better

48
Q

What are concerns of nanoparticles?

A

That they could get into the body and damage cells

Chemistry gcse (10 decks)

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