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Chemistry > Bonding > Flashcards

Bonding Flashcards

(47 cards)

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1
Q

What are the 3 types of bonds?

A

Ionic bonds
Covalent bonds
Metallic bonds

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2
Q

When does ionic bonding occur?

A

Between a metal and non-metal

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3
Q

When are positive and negative ions created?

A

Positive ions are created when an atom LOSES electrons

Negative ions are created when an atom GAINS electrons

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4
Q

How is ionic bonding shown in a diagram?

A

Dot and cross diagram
Transfer of electrons (dot/cross) between outer shells of two atoms shown through arrows
Must show two stages of process: one showing transfer and other showing result

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5
Q

What are ionic compounds held together by?

A

The attraction between oppositely charged ions/electrostatic forces/ionic bonds (all the same)

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6
Q

What do all ionic compounds exist as?

A

Giant ionic structures - Many ions joined to each other with ionic bonds in a giant ionic lattice

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7
Q

What are the properties of ionic compounds?

A

Generally soluble - Water molecules are attracted to charged ions
High mpt and bpt - Strong bonds between oppositely charged ions are hard to break
Do not conduct electricity when solid - Ions firmly held together in lattice (+ no free electrons)
Do conduct electricity when molten - Ions are free to move

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8
Q

Why is the melting temperature higher on a compound containing ions with higher charges?

A

The higher the charges on ions are in an ionic compound, the stronger the forces of attraction are, therefore making them harder to break

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9
Q

When does covalent bonding occur?

A

Between two non-metals

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10
Q

What happens in ionic bonding?

A

Electrons are transferred between atoms to create a full outer shell and become ions

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11
Q

What happens in covalent bonding?

A

Two ions (either different or the same) share electrons to achieve a full outer shell

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12
Q

How is covalent bonding shown?

A

In one diagram in which the shared electrons are depicted between the two ions

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13
Q

Why are covalent bonds strong?

A

The shared electrons are attracted to the nuclei of both atoms

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14
Q

What do most covalently bonded structures exist as?

A

Simple molecular structures

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15
Q

What forces of attraction are present in substances with a simple molecular structure?

A

Strong covalent bonds between atoms (intramolecular forces), but weak intermolecular forces (forces of attraction between individual molecules - hence low mpt and bpt)

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16
Q

What properties do simple molecular structures have?

A

Low mpt and bpt - Liquids and gases at room temp

Do not conduct electricity - No delocalised electrons

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17
Q

Which covalent substances exist as giant structures?

A

Diamond + Graphite

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18
Q

What properties does graphite have?

A

Very soft
Conducts electricity - sea of free moving electrons because fourth electron is unbonded
Very high mpt - Over 3600 degrees

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19
Q

Describe the structure of graphite

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A

Made of C atoms
Layers of hexagonal structures
Each C atom joined to 3 others
Fourth electron is delocalised between layers
Strong covalent bonds between C atoms but weak forces of attraction between layers

20
Q

What are the uses of graphite?

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A

Pencils + lubricants - Layers can slide because of weak forces of attraction
Electrodes

21
Q

Describe the structure of diamond?

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A

A form of C

Each C atom is joined to 4 others

22
Q

What are the properties and uses of diamond?

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A

V. hard -> Cutting tools
V. high mpt + bpt
Crystalline -> Jewellery
Does not conduct electricity

23
Q

What are metallic bonds?

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A

Forces of attraction between positive metal ions and delocalised electrons

24
Q

Describe metallic structures

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A

Giant structures of regularly arranged metal atoms in a lattice in a ‘sea’ of delocalised electrons which are free to move around the lattice

25
Why do metallic structures have delocalised electrons?
All electrons from the outer shells of the metals are delocalised (made to not belong to a particular atom)
26
What are properties of metals?
Good conductors of electricity - Delocalised electrons Malleable/ductile - Metal ions can slide over each other High mpt and bpt (generally) - Exist as giant structures
27
Why are melting + boiling temperatures different on different metals?
The higher the charge on the metal ion the more delocalised electrons there are (because they will have needed to lose more to achieve a full outer shell), so the stronger the metallic bonds
28
What are the differences between single, double and triple covalent bonds?
Double and triple covalent bonds are stronger and therefore require more energy to break them
29
What is an alloy?
A combination of 2+ elements, where at least 1 is a metal
30
What makes alloys different to pure metals?
The ions of the different elements are different sizes which makes it harder for the layers to slide across each other when a force is applied - layers are distorted This also makes them stronger then pure metals
31
What is graphene?
A single layer of graphite, just one atom thick
32
What properties does graphene have?
Very light - Only 1 atom thick Very strong - Covalent bonds between atoms Can conduct electricity - Has delocalised electrons
33
What are the uses of graphene?
Graphene makes materials stronger without making them much heavier. It can be used in solar panels, batteries etc.
34
What are fullerenes?
Cage structures made from carbon atoms Most famous is buckminsterfullerene (bucky balls) which are spherical molecules containing 60 carbon atoms (formula: C60)
35
What uses do fullerenes have?
Catalysts Lubricants Vehichles for transporting drugs into the body (because they are spherical they can enclose other molecules)
36
What are carbon nanotubes?
Single layers of graphite (graphene) rolled into a tube | They are cylindrical fullerenes
37
What could carbon nanotubes be used for in the future?
To make miniature electronic circuits
38
When is something considered to be nano-sized?
When it is between 1-100nm (nanometres)
39
What are the benefits of nanoparticles?
They have a very high surface area to volume ratio, meaning smaller amounts of materials can be used for a purpose compared to using normal sized particles. This makes them cheaper and more efficient to use than larger particles.
40
What are the drawbacks to nanoparticles?
They are still a relatively new area of research so there could still be long-term effects to human health that we don't know about
41
Why are nanoparticles different to normal particles?
When materials are produced as nano-sized particles they behave differently to the same material on bulk scale E.g. ‘normal’ gold particles are extremely unreactive, but gold nanoparticles can be very efficient catalysts for many processes because of their higher surface area
42
What are nanoparticles used as?
Catalysts - Larger surface on which reactions can be catalysed Medicine - Fullerene nanoparticles can be used to efficiently deliver drugs to a specific area of the body to target a disease. Electronics - Carbon nanotubes are used in new computer chips because of their good electrical conductivity. Cosmetics - So small that visible light passes through them, making them transparent so white substances, like sun cream, can be made transparent Deodorants - Nanoparticles can have antimicrobial properties
43
What are smart materials?
Materials with properties that react to a change in their environment. These changes are reversible.
44
What are thermochromic materials?
React to a change in temp by changing colour E.g. Thermometers made of plastic strips Baby feeding spoons
45
What are photochromic materials?
React to a change in light by changing colour E.g. Lenses for sunglasses
46
What are shape memory alloys/polymers?
``` Regain their original shape on heating E.g. Spectacle frames Self-repairing car bodies Coffee-pot thermostats Stents for veins ```
47
What are hydrogels?
Can absorb/release many times their own volume in water E.g. Nappies Soft contact lenses

Chemistry (6 decks)

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