C3 - Structure and bonding 1️⃣✅ Flashcards

1
Q

What bonding occurs between a metal and non-metal?

A

Ionic bonds

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2
Q

What bonding occurs between a non-metal and a non-metal?

A

Covalent bonds

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3
Q

What bonding occurs between a metal and a metal?

A

Metalic bonds

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4
Q

What is ammonia?

A

A compound containing the elements nitrogen and hydrogen NH3

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5
Q

What is ionic bonding?

A

Ionic bonding is when a non-metal and a metal react together, one element looses electrons in order to make the other elements outer shell full

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6
Q

What is covalent bonding?

A

Covalent bonding is when a non-metal and a non-metal share electrons to complete each others outer shell

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7
Q

What is metallic bonding?

A

Metallic bonding is the electrostatic attraction between the positive metal ions and the free moving delocalised electrons

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8
Q

What are the 2 allotropes of carbon?

A

Diamond and graphite

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9
Q

Why is melting a ionic substance so difficult?

A

Because ionic substances have a regular repeating and strong structure with many bonds, in order to melt the substance, you would have to break all the bonds. Therefore the melting point is very high as breaking all of the bonds takes a very long time

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10
Q

What is the structure of ionic substances?

A

Giant ionic lattice (regular, repeating pattern, like covalent ionic bonds are strong)

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11
Q

How do you calculate mr?

A

You do the elements mass number x its occurrence for however many elements there are and then add them together

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12
Q

What is a single bond?

A

When each atom shares one pair of electrons

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13
Q

What is a double bond?

A

When each atom shares two pairs of electrons

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14
Q

What ions do group 1 form?

A

1+

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15
Q

What ions do group 2 form?

A

2+

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16
Q

What ions do group 3 form?

A

3+

17
Q

What ions do group 4 form?

A

They do no t form ions

18
Q

What ions do group 5 form?

A

3-

19
Q

What ions do group 6 from?

A

2-

20
Q

What ions do group 7 form?

A

1-

21
Q

What ions do group 0 form?

A

They do not form ions as they already have full outer shells so there are no free spaces for a bond

22
Q

When you melt a substance are what are you actually melting?

A

You arent melting the strong bonds as they are way too strong, you are actually melting the weak intermolecular forces that hold together the strong bonds. The bigger the molecule the bigger/ stronger the intermolecular forces are, therefore, the higher the melting point

23
Q

What are the properties of diamond?

A
  • Each carbon covalently bonded to 4 other carbons therefore no free delocalised electrons
  • lots of strong bonds
  • melting point of 4000℃
  • doesn’t conduct electricity because no spare delocalised electrons
  • hard & sparkly
24
Q

What are the properties of graphite?

A
  • Each carbon covalently bonded to 3 other carbons therefore one (delocalised) electron left
  • delocalised electrons hold layers together so not bonded
  • melting point of 3600℃
  • conducts electricity because of free delocalised electrons
  • brittle and breaks easily
  • slippery & layers can slide
25
Q

What is graphine?

A

one layer of graphtie

26
Q

Explain why graphite is soft?

A

Layers are not bonded so can slide over eachother

27
Q

What is an ion?

A

An atom that has lost or gained electrons

28
Q

Which kinds of elements form ionic bonds?

A

metals and non-metals

29
Q

Which kinds of elements form ionic bonds?

A

non-metals and metals

30
Q

Explain why graphite is soft

A

Layers have no covalent bonds so can slide over each other as they are held together by weak intermolecular forces

31
Q

Why are metals good conductors?

A

Because delocalised electrons are free to move through the whole structure

32
Q

What is an alloy?

A

An alloy is a mixture of two or more elements, at least one of which is a metal

33
Q

What is a nanoparticle?

A

Nanoparticles are structures, 1-100 nanometres (nm) in size, that usually contain only a few hundred atoms

34
Q

What do silver nanoparticles do?

A

Silver nanoparticles continuously release a low level of sliver ions to protect against a bacteria.

35
Q

Where are silver nanoparticles most commonly used?

A

To clean operating theatres in hospitals, textiles, keyboards and wound dressings

36
Q

What are the negatives for nanoparticles?

A

When used in sum creams we don’t know if they can infiltrate our body’s and possibly damaged body cells or that if they are washed into the ocean that they are damaging the environment

37
Q

What is a common use for a fullerene sphere?

A

To deliver drugs to specific areas around the body

38
Q

What was the first fullerene?

A

Buckminsterfullerene

39
Q

What shape and what formula did the first fullerene have?

A

(Buckminsterfullerene) A spherical fullerene shape and has a formula of C60