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GCSE Chemistry > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

1
Q

What are the three types of strong chemical bonds?

A
  • Ionic bonds
  • Covalent bonds
  • Metallic bonds
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2
Q

What is an ion?
Where do ionic bonds occur?

A

Atoms that have gained or lost electrons
Between positive and negative ions

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3
Q

Do ions have an overall charge?

A

Yes

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4
Q

What do ions have the same electronic structure as?

A

Noble gas - complete outer shell of electrons

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5
Q

What does ionic bonding involve?

A

The transfer of electrons from metal atoms to non-metal atoms

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6
Q

Describe what the charge of metal and non-metal atoms when they react to become ions.

A

Metals = lose electrons and become positively charged
Non-metals = gain electrons and become negatively charged

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7
Q

What is an ionic bond?

A

A strong electrostatic force of attraction between the positive metal ion and the negative non-metal ion

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8
Q

Practice question:
Describe what happens when two sodium atoms react with one molecule of chlorine.
Sodium has 1electron in outer shell
Chlorine has 7 electrons in outer shell

A

One chlorine molecule = 2 chlorine atoms
Sodium atom transfers one electron to one of chlorine atoms
All now have 8 electrons in outer shell
Become Na+ and Cl-
2Na + Cl2 —— 2NaCl

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9
Q

What are ionic compounds?

A

Giant structures of ions

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10
Q

What are ionic compounds held together by?

A

Strong forces of attraction (electrostatic forces) that act in all directions between oppositely charged ions

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11
Q

Name some properties of ionic compounds.

A
  • High melting points
  • Do NOT conduct electricity when solid because ions cannot move
  • Do conduct electricity when molten or in solution because the charged ions are free to move about and carry their charge
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12
Q

Why do metals form positively charged ions?

A

Because they lose electrons in order to form ions

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13
Q

Why do ionic compounds have high melting and boiling points?

A

Ionic bonds are very strong and therefore requires a lot of energy to overcome them

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14
Q

Where does metallic bonding occur?

A

In metallic elements such as iron and copper
Alloys such as stainless steel

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15
Q

Describe the structure of metals.

A

A giant 3D lattice in which electrons in the outer shell are delocalised

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16
Q

What is a metallic bond?

A

The attraction between the positive ions and the delocalised negatively charged electrons

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17
Q

Why are metals good thermal and electrical conductors?

A

The delocalised electrons can move freely and transfer energy

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18
Q

Why do most metals have high melting and boiling points?

A

Metallic bonds are very strong meaning that a lot of energy is required to break them

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19
Q

Why can metals be bent and hammered into different shapes?

A

The layers are able to slide over each other quite easily

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20
Q

Practice question:
Why is copper used to make water pipes?

A
  • It’s an interactive metal, so it does not react with water
  • It can be easily shaped
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21
Q

What is an alloy?

A

Mixtures that contain a metal and at least one other element

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22
Q

Why are pure metals rarely used?

A

They are to soft

23
Q

In alloys, what does the added element do to the arrangement of the metal atoms?

A

It disturbs the regular arrangement so the layers do not slide over each other so easily

24
Q

What is steel?

A

A very useful alloy made from iron

25
Q

When iron oxide is reduced in a blast furnace what does this produce?

A

Iron

26
Q

What does molten iron, obtained from a blast furnace, contain?

A

Approx. 96% iron and 4% impurities l, including carbon phosphorus and silica

27
Q

Why is iron brittle when obtained from a blast furnace?

A

It’s impure

28
Q

How are the atoms in pure iron arranged?

A

In layers that can slide over one another easily making it soft and malleable

29
Q

Name some properties of steel depending on the amount of carbon/ other elements.

A
  • Steel with a high carbon content is hard and strong
  • Steel with a low carbon content is soft and easily shaped
  • Stainless steel contains chromium and nickel and is hard and resistant to corrosion
30
Q

What is a covalent bond?

A

A shared pair of electrons between atoms

31
Q

Where do covalent bonds occur (what type of elements)?

A
  • Non-metallic elements e.g. oxygen
  • Compounds of non-metals e.g. sulfur dioxide
32
Q

Example question:
A chlorine atom has seven electrons in its outer shell. In order to bond with another chlorine atom what occurs?

A
  • An electron from each atom is shared
  • This gives each chlorine atom eight electrons in the outer shell
  • Each atom now has a complete outer shell
33
Q

Are covalent bonds strong or weak?

A

Strong

34
Q

What do simple molecules contain?

A

A relatively small number of non-metal atoms joined together by covalent bonds

35
Q

Why do simple molecular substances (e.g. water) have low melting and boiling points?

A

There are weak forces of attraction between the molecules which are easily overcome

36
Q

Do simple molecular substances conduct electricity?
Why?

A

No, they have no overall electrical charge

37
Q

Key point:

A

The intermolecular forces between simple molecules are very weak compared to the strength of covalent bonds in the molecules themselves

38
Q

How does the size of molecules relate to the strength of the intermolecular forces between simple molecules?

A

The larger the molecules are the stronger the intermolecular forces between simple molecules become. This means larger molecules have higher melting and boiling points

39
Q

How does differ in Group 7 of the periodic table?

A

The molecules get larger as you go down and so the melting and boiling points also increase

40
Q

What are all the atoms in giant covalent structures linked by?

A

Strong covalent bonds

41
Q

What are giant covalent structures?

A

Solids with very high melting and boiling points

42
Q

What is diamond?

A

A form of carbon

43
Q

Name some features of diamond?

A
  • It has a giant, rigid covalent structure (lattice)
  • Each carbon atom forms four strong covalent bonds with other carbon atoms
  • All the strong covalent bonds mean that it is a very hard with a very high melting point
  • There are no charged particles, so it does not conduct electricity
44
Q

What is graphite?

A

A form of carbon

45
Q

What structure does graphite have?

A

Giant covalent structure

46
Q

Does graphite have a high or low melting point?

A

High

47
Q

What does each carbon atom form?

A

Three covalent bonds with other carbon atoms

48
Q

Describe the structure of graphite.

A

A layered, hexagonal structure

49
Q

What are the layers in graphite held together by?
What does this mean?

A

Weak intermolecular forces.
This means that the layers can slide last each other, making graphite soft and slippery

50
Q

One electron from each carbon atom in graphite is delocalised. What does this allow graphite to do?

A

Conduct heat and electricity

51
Q

Describe the structure of silicon dioxide.

A

Giant covalent structure and has lattice structure similar to diamond

52
Q

In silicon dioxide what is each oxygen atom joined too?

A

Two silicon atoms

53
Q

In silicon dioxide what is each silicon atom joined too?

A

Four oxygen atoms

GCSE Chemistry (2 decks)

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