C2 Flashcards

1
Q

What are the 3 bonds?

A

Ionic, covalent and metallic

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2
Q

Summary for ionic bonding?

A

1 positive metal ion and 1 negative non-metal ion. Transfers electrons from metal to non-metal and then the ions are strongly attracted to each other with electrostatic forces.

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3
Q

Summary for covalent bonding?

A

2 non-metal atoms which share electrons. Attracted together by strong electrostatic forces.

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4
Q

Summary for metallic bonding?

A

2 metal atoms which share delocalised electrons. Electrostatic attraction between positive nuclei and negative shared electrons.

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5
Q

What’s the diagram for ionic bonding?

A

Dot and cross diagram

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6
Q

What is an ionic compound?

A

A giant structure of ions held together by strong electrostatic forces of attraction between oppositely charged ions.

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7
Q

What are the limitations of the dot and cross diagram?

A

They don’t show:
- Structure of compound
- Size of ions
- How they’re arranged

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8
Q

What are the limitations of ball and stick diagram?

A

It’s not to scale. There are in fact no gaps between ions.

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9
Q

What’s the empirical formula?

A

Just basically the regular formula

e.g. K2O

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10
Q

What type of structure does most gases have?

A

Simple covalent structure.

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11
Q

What type of structure does sodium chloride and magnesium chloride have?

A

Giant ionic structure.

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12
Q

What type of structure does diamond, graphite, graphene and fullerenes have?

A

Giant covalent structure.

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13
Q

What type of structure does gold, copper and zinc have?

A

Giant metallic structure.

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14
Q

What type of structure does steel and bronze have?

A

Giant metallic structure.

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15
Q

Why can’t most gases conduct electricity?

A

No ions, no delocalised electrons (which usually carry charge).

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16
Q

How can sodium chloride and magnesium chloride conduct electricity?

A

When liquid, the ions can move and carry charge through the structure.

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17
Q

Why can’t sodium chloride and magnesium chloride conduct electricity?

A

When solid, the ions can’t move.

18
Q

Why can’t diamond conduct electricity?

A

Each carbon makes 4 strong bonds so there are no spare electrons so no delocalised electrons (which usually carry charge).

19
Q

Why can graphite, graphene and fullerenes conduct electricity?

A

Each carbon makes 3 strong bonds so there’s a spare electron. So, there’s delocalised electrons which carry charge and move through the structure.

20
Q

Why can metals conduct electricity?

A

They have delocalised electrons which move and carry charge through the structure.

21
Q

What are limitations of the solid, liquid, gas diagram?

A

There are no forces included, all particles are spheres and the spheres are solid.

22
Q

Which state has the highest boiling and melting point?

23
Q

Which state has the most energy?

24
Q

What’s an ionic compound?

A

Structure with strong electrostatic forces of attraction between oppositely charged ions.

25
Q

Why do ionic compounds have high melting and boiling points?

A

Large amount of energy needed to overcome the strong bonds.

26
Q

Summary about polymers

A
  • Very large molecules
  • Atoms linked to other atoms by strong covalent bonds.
  • Relatively strong intermolecular forces between molecules.
27
Q

Why are alloys harder than pure metals?

A

Because they have differently sized particles with uneven layers so they cannot easily slide over each other like pure metals can.

28
Q

In graphite what forces are in between layers?

A

Weak forces

29
Q

What is graphene useful for?

A

Electronics and composite materials

30
Q

What is a fullerene?

A

Fullerenes are molecules of carbon atoms with hollow shapes.

31
Q

What was the first fullerene discovered?

A

Buckminsterfullerene (C60) (sphere)

32
Q

What do carbon nanotubes have?

A

They are cylindrical fullerenes with very high length to diameter ratios.

33
Q

How are carbon nanotubes useful?

A

Nanotechnology, electronics and materials.

34
Q

What does nanoscience refer to?

A

Structures 1-100nm.

35
Q

What’s the order for tiny particles?

A

Nanoparticles 1-100nm
Fine particles 100-2500nm
Coarse particles (dust) 2500-10000nm

36
Q

What do nanoparticles have as a property?

A

High surface area to volume ratio.

37
Q

What happens as a side of a cube decreases by a factor of 10?

A

The surface area to volume ratio increases by a factor of 10.

38
Q

What are some uses of nanoparticles?

A

Medicine, electronics, cosmetics, sun cream, deodorant, catalysts.

39
Q

What are some advantages of nanoparticles?

A

Small so less can be used for same effect. Environmentally friendly.

40
Q

What are some disadvantages of nanoparticles?

A

If absorbed into skin, could be toxic.