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Chemistry > C5.2- Bonding, Structure And The Properties Of Matter > Flashcards

C5.2- Bonding, Structure And The Properties Of Matter Flashcards

1
Q

What bonds do 2 non-metals form?

A

Covalent

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2
Q

What bonds to 2 metals form?

A

Metallic bonds

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3
Q

What bonds do a metal and non-metal form?

A

Ionic

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4
Q

What is ionic bonding?

A

The sharing of electrons between a metal and non-metal in order to achieve a full outer shell. They form a positive and negative ion.

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5
Q

What ratio do aluminium and oxygen react together?

A

Al2O3

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6
Q

What would you draw for the reaction between magnesium and oxygen?

A

Magnesium with 3 shells oxygen with 2 shells. Then magnesium with 3 shells (an empty one for the third one) and square brackets with a charge of 2+. Oxygen with 2 shells and square brackets with a charge of 2-

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7
Q

What is formula for magnesium chloride?

A

MgCl2

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8
Q

Why do ionic compounds have a high melting point?

A

There are strong electrostatic forces between oppositely charged ions, these forces of attraction act in all directions, it takes a lot of energy to overcome these forces and separate the ions meaning they have a high melting point.

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9
Q

Do ionic structures conduct?

A

When molten or dissolved the ions can move freely, this means they can carry charge through the structure. When solid the ions cannot move freely therefore charge cannot be carried through the structure.

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10
Q

Why are ionic compounds brittle?

A

All of the bonds are the same type of bond, these bonds are strong and if enough force is applied many of these bonds will break at the same time, not just one.

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11
Q

What are the 3 ways covalent bonds can be drawn?

A

Dot and cross diagram, displayed formula, 3D model

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12
Q

Why do simple covalent molecules have low melting/boiling points?

A

Weak intermolecular forces because they are small means a low amount of energy can be applied to overcome them and turn them into a gas

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13
Q

Why don’t simple covalent molecules conduct?

A

Because they have an overall charge of 0. Electricity is an electron so needs charge to be carried but molecules have no charge.

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14
Q

How is graphite able to conduct?

A

The carbon atoms only form 3 bonds each meaning there is a delocalised electron per carbon to carry charge through the structure.

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15
Q

What holds the layers of graphite together?

A

Weak intermolecular forces

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16
Q

Why don’t diamonds conduct?

A

There are no delocalised electrons as the carbons make the 4 bonds they need. This means charge cannot flow through the structure.

17
Q

What is a fullerene?

A

Molecules made up of hexagonal rings of carbon atoms

18
Q

What structure can fullerenes make?

A

Hollow balls or tubes

19
Q

How many carbon atoms are there in a buckminsterfullerene?

A

60 arranged in the same way as a football (20 hexagons and 12 pentagons)

20
Q

What are the properties of carbon nanotubes?

A

They conduct and have high melting/boiling points

21
Q

What are some uses of fullerenes?

A

Lubricants, drug and gene delivery, absorbent for gases, x-ray imaging contrast agents

22
Q

Describe a metal structure.

A

Positively charged ions in a cloud of delocalised electrons

23
Q

What are the properties of pure metals?

A

Good conductors, malleable and ductile, soft, high melting point

24
Q

Why are alloys stronger than pure metals?

A

The ions are different sizes meaning they don’t form neat layers and then won’t slide over each other

25
Q

What is graphene?

A

One layer of graphite

26
Q

Why do polymers have a higher melting/boiling point than small covalently bonded molecules?

A

Because they have stronger intermolecular forces which require more energy to overcome.

27
Q

What are some used of nano particles?

A

Sunscreen, electronics, catalysts, medical treatments

28
Q

Why could nanoparticles be harmful?

A

Because they are so small it may be possible for them to pass into cells and catalyse reactions that are harmful. Toxic substances could bind to them and get into the body.

29
Q

How large are nanoparticles?

A

PM2.5=2500nm
PM10=10000nm

Chemistry (12 decks)

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