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Chemistry - GCSE > Covelant Bonds > Flashcards

Covelant Bonds Flashcards

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1
Q

How many electrons does hydrogen have in its outer shell?

A

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2
Q

How many electrons does carbon have in its outer shell?

A

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3
Q

How many electrons does nitrogen have in its outer shell?

A

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4
Q

How many electrons does oxygen have in its outer shell?

A

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5
Q

How many electrons does chlorine have in its outer shell?

A

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6
Q

How any covenant bonds does hydrogen have?

A

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7
Q

How any covenant bonds does carbon have?

A

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8
Q

How any covenant bonds does nitrogen have?

A

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9
Q

How any covenant bonds does oxygen have?

A

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10
Q

How any covenant bonds does chlorine have?

A

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11
Q

What are ionic bonds always between?

A

A metal and a non metal

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12
Q

What are covenant bonds always between? What do they involve?

A

Two non metals, involves a shared pair of electrons

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13
Q

In a shared pair of electrons, where must the shared electrons be from?

A

One electron from each element

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14
Q

What are the properties of a simple covalent substance?

A

Low melting and boiling point, does not conduct electricity?

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15
Q

What are the properties of a giant molecular substance?

A

High melting and boiling point, does not conduct electricity, is not soluble

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16
Q

What is the one giant molecular substance that does conduct electricity?

A

Graphite

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17
Q

Why do simple molecular substances have low melting and boiling points?

A

Because weak molecular forces between molecules are broken easily

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18
Q

What are giant molecular structures held together by?

A

Strong covalent bonds

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19
Q

What holds atoms together?

A

Bonds

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20
Q

What holds molecules together?

A

Forces

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21
Q

Why can’t simple molecular substances conduct electricity?

A

Because everything is banded together and nothing is free to move.

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22
Q

How does the number of carbon atoms in a chain relate to melting and boiling points?

A

The more carbon atoms in the chain, the higher the melting and boiling points

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23
Q

What is a polymere?

A

A polymere is a large molecule containing chains of carbon atoms.

24
Q

How are polymeres made?

A

They are made from joining together many smaller carbon chains

25
Q

Why does melting boiling point increase with chain length?

A

Because as chain length increases there are more intermolecular forces between polymers, and energy is needed to break them

26
Q

What are monomers?

A

Monomers are small, simple molecules that can be joined to make polymere

27
Q

What are allotropes?

A

Allotropes are different structural forms of the same element

28
Q

What are the four allotropes of carbon?

A

Diamond
Graphite
Graphing
Fullerenes

29
Q

What are the two properties of allotropes of carbon?

A

They have high melting points due to large number of covenant bonds, and are giant covalent molecules

30
Q

What is graphene? What are it’s notable properties?

A

It is an allotropes of carbon, 1 atom thick, giant covalent, exceptional strength, electrical conductor

31
Q

What is fullerene? What are it’s notable properties?

A

It’s carbon covalently bonded to 3 carbons with a delocalised electron, spherical shape, low melting point, conducts electricity, poor reactivity, soft and slippery

32
Q

Why is diamond hard?

A

Because the giant structure is held together by a strong tetrahedral arrangement of covalently bonded carbon atoms

33
Q

Why is granite soft?

A

Because it is the only held together by weak intermolecular forces between the sheets of atoms

34
Q

WHY do graphite and graphite conduct electricity?

A

Because delocalised electrons allow a flow of charge

35
Q

Why is C{little 60} unstable as a SOlid st high temperatures?

A

Because there are only weak intermolecular forces between simple molecules

36
Q

Why is graphene transparent?

A

Because it is made of a single 2D sheet of atoms

37
Q

What are the results of delocalised electrons being free to move?

A

When a potential difference is applied, the electrons flow in one direction

38
Q

Give five properties of metals

A 
High density
Usually solid at room temperature
Shiny
Conductor of heat and electricity
Forms cations
Sonorous - makes a ringing noise
Iron, cobalt, nickel and copper conduct electricity
High melting points
Malleable - can be shaped
Ductile - pull it and it becomes thinner
Colourful
39
Q

What is density?

A

Weight relative to volume

40
Q

What is the one metal that isn’t solid at room temperature?

A

Mercury

41
Q

What does it means for something to be sonorous

A

It makes a ringing noise

42
Q

What 4 metals conduct electrocity?

A

Iron, cobalt, nickel, copper

43
Q

What does it mean for something to be malleable?

A

It can be shaped

44
Q

What does it mean for something to be ductile?

A

Pull it and it becomes thinner

45
Q

What are four MAIN properties of non metals?

A

Low melting points
Poor conductor
Gas liquid or solid
Brittle

46
Q

What are four MAIN properties of metals?

A

High melting point
Good conductors
Shiny solids
Malleable

47
Q

What is the structure of metal?

A

Positive metal ions arranged in rows in | | | structure
| |
Held together by negatively charged delocalised electrons

48
Q

What happens to the structure of metal when heated?

A

The positive ions will separate

49
Q

What does it mean for an atom to be delocalised?

A

Not fixed in position/free to move around

50
Q

Why is metallic bonding so strong?

A

Because the positive ions (cations) and electrons are strongly attracted to each other, so metallic bonding is strong and a lot of energy is needed to break bonds and change state

51
Q

What happens when you apply force to metal?

A

The regularly arranged ions move over one another. Doesn’t break because ions are still held together by delocalised electrons

52
Q

What’s an alloy? How does it compare to metal?

A

Metal and non metal or 2 metals nodded together. They are strong and less mailable than metal.

53
Q

What are the properties of an ionic material? Give one example of one.

A

Conducts electricity when molten or dissolved. High melting and boiling points. Nacl(salt

54
Q

What are the properties of an simple molecular material? Give two examples of one.

A

Low melting and boiling points
Weak intermolecular forces
Usually in gas or liquid states
H(little2)O , CO(little2)

55
Q

What are the properties of an giant molecular material? Give two examples of one.

A 
High melting and boiling points
Doesn't conduct electricity 
Diamond, graphite
Diamond doesn't Dissolve in water
Graphite is the one giant molecular that does conduct electricity
56
Q

What are the properties of an metallic material? Give two examples of one.

A

Conducts heat and electricity
Shiny, coloured
Medium melting and boiling points

Zinc, copper

Chemistry - GCSE (9 decks)

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