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GCSE Chemisty > C2 structure,bonding and the properties of matter > Flashcards

C2 structure,bonding and the properties of matter Flashcards

1
Q

Ionic bonding

A

Metals and non metals
Partials are oppositely charged ions
Structure- large crystals made from ions attracted to each other by electrostatic attraction
Room temp- solids
Melting point- high
Conductor of electricity- not when solid, yes when molten

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2
Q

Covalent bonding

A

Compounds of non metals and in most non metallic elements
Atoms that share pairs of electrons
Structure- molecules made from atoms bonded by covalent bonds
Room temp- liquid and gases
Melting point- low
Conductor of electricity- no or very little
Very strong

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3
Q

Metallic bonding

A

Metallic elements and alloys
Atoms that share delecoalised electrons
Structure- lumps or sheets of metal made from atoms packed together so that the delocalised electrons move through the fixed position
Room temp- solids (expect Mercury liquid)
Melting point- high
Sharing delocalised electrons makes strong bonds
Conductor of electricity- yes, good conductor

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4
Q

When metals and non metals transfer electrons

A 
Atoms become charged. Make ions.
Metal is positively charged
Non metal is negatively charged 
Ionic bonding
Positive and negative attracted by electrostatic attraction
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5
Q

Why do atoms bond

A

To make stable electronic structures
It is easier for metals to lose electrons and become positive ions
And easier for non metals to gain electrons to become negative ions

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6
Q

Giant structures

A

An ionic compound is a giant structure of ions in a lattice

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7
Q

Ball and stick diagram pros

A

The structure in 3D
The charges on the ions
The arrangement of ions in 3D
The type of ions in all directions

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8
Q

Ball and stick cons

A

Ions are actually closer together

Gives false image of bond direction when it is only electrostatic attraction

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9
Q

Ball and stick best represents

A

The number and type of ions in 3D

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10
Q

Close packed pros

A 
The structure in 3D
The charges on the ions
The arrangement of ions
In 2D (look at the front face of the diagram)
The closeness of ions
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11
Q

Close packed cons

A

Difficult to see arrangement of ions in 3D

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12
Q

Close packed best represents

A

The way that ions are packed close together

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13
Q

States of matter

A 
Solid} sublimation} gas
Gas} condensation} liquid 
Liquid} boiling} gas
Liquid} freezing} solid
Solid} melting} liquid
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14
Q

In melting and boiling

A

Forces between particles decrease
Distance between particles increases
Arrangement becomes more random
Particles move more so need more energy from surroundings

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15
Q

In freezing and condensing

A

The strength of the particles remains the same
Distance between particles decreases
Arrangement becomes less random
Particles move less so less energy required from surroundings

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16
Q

Limitations of simple model

A

There are no forces represented between spheres
All particles represented as spheres
The spheres are represented as solid and inelastic

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17
Q

Small molecule

A

2 or 3 atoms joined together with no charge
Relatively low melting points and boiling points
Weak intermolecular forces
Can’t conduct electricity as have no charge

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18
Q

Polymers

A

Very large molecules
Atoms are linked to other atoms by strong covalent bonds
Form long chains
Intermolecular forces between polymer molecules are weaker
Allow chains to slide over each other but not pulled apart

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19
Q

Intramolecular bonds

A

The atoms of the monomers along the chains in a polymer are held together by strong covalent bonds. These are bonds within the polymer molecules

20
Q

Intermolecular

A

The chains of the polymer are held together by weak forces of attraction. These forces between polymer molecules

21
Q

Weak intermolecular forces of attraction

A

Stretches easily

Lower melting point

22
Q

Strong cross linkes- chemical bonds between the chains

A

Rigid

Higher melting points

23
Q

Making polymers

A

By addition

By condensation

24
Q

Addition polymers

A

Long chains of units made from one molecule that has at least 1 double bond between carbon atoms
🔴➖🔴➖🔴➖🔴➖🔴➖🔴

25
Q

Condensation polymers

A

Made of units using at least 2 different molecules
Losing a water molecule in the process
🔴➖🔶➖🔴➖🔶➖🔴➖🔶

26
Q

Giant covalent structures

A

All atoms are linked to each other by strong covalent bonds

Eg. Diamond,silicon dioxide

27
Q

Diamond properties

A 
Lustrous 
Transparent
Colourless
Very hard
Very high melting point 
Insoluble in water
Doesn't conduct electricity
28
Q

Silicon dioxide

A 
White crystalline solid
Very hard
Very high melting point 
Insoluble in water
Does not conduct electricity
29
Q

Forms of carbon

A

Diamond
Graphite
Structures are very different

30
Q

Structure of diamonds

A

Each carbon atom forms 4 bonds
Forms tetrahedron shape
The 4 covalent bonds makes it very hard to break
Carbon atoms share electrons

31
Q

Graphite

A

Made from carbon
Carbon atoms only make 3 covalent bonds
Make hexagonal rings which form layers
Cut across layers but not through layers
No covalent bonds between layers
High melting point
Weak forces hold layers together
Sea of delocalised electrons conducts electricity
Delocalised electrons move easily along layers

32
Q

Uses of graphite

A

Electrodes - conducts electricity
Lubricant- layers slide over each other
High temp lubricant- high melting point

33
Q

Graphene

A

Single layer of graphite
One atom thick
Hexagonal rings of carbon atoms connected with strong covalent bonds

34
Q

Fullerenes

A

Carbon rings can form hollow 3D shapes

35
Q

Buckminsterfullerene

Bucky ball

A

Rings of 5&6 carbon atoms
C60
Spherical shape
Used in medicine

36
Q

Uses of fullerenes

A 
Drug delivery into the body
Lubricants
Catalysts
Act as hollow cages to trap other molecules 
Make nanotubes
37
Q

Nanotube properties

A

High tensile strength
High electrical conductors
High thermal conductivity

38
Q

Nanotube uses

A

Semi conductors in electrical circuits
As catalysts
Reinforcing materials eg. Tennis rackets

39
Q

Properties of graphene

A 
2D compound
Thermally stable
Monolayer 
Electrical conductor through 'ballistic transport'
Strongest material ever
Elastic
Absorb white light
40
Q

Nanoparticals

A

Between 1&100 nm in size
Most are made from metals,metal oxides and silicates
Each nanoparticle contains only a few hundred atoms

41
Q

When materials are present in nano particles it changes properties

A

Silver- stops bacteria growing (in clothes/deodorants)
Titanium dioxide- protects from ultraviolet light (in sun cream) bigger particles do the same but leave white coating on skin
Used to deliver drugs to the right cells

42
Q

Nanoparticle safety

A

Avoid breathing in as can be hazardous

Could damage organs and tissue

43
Q

Changing surface area to volume ratio

Nanoparticles

A

When a material becomes a nanoparticle its properties change
Gold- displays different colours
Titanium dioxide- becomes invisible
Silver- destroys bacteria
Other materials become more reactive as sa to v ratio increases making them better catalysts

44
Q

Radius of atom

A

1 x 10-12 m

45
Q

Radius of nucleus

A

1 x10-15 m

GCSE Chemisty (10 decks)

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