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Chemistry GCSE > Chemistry GCSE: C2 Bonding, Structure and Properties of matter > Flashcards

Chemistry GCSE: C2 Bonding, Structure and Properties of matter Flashcards

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1
Q

Ionic bonds form between…

A

Positively charged metals ions and negatively charged non-metal ions.

Ionic bonds are (electrostatic) attractions between oppositely charged ions.

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2
Q

Do ionic bonds involve…

  1. Sharing electrons
  2. Loss and gain of electrons
  3. Free electrons
A

Loss and gain of electrons

Metal atoms lose electrons to form positive ions.

Non-metals atoms gain electrons to form negative ions.

These ions are (electrostatically) attracted to each other.

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3
Q

What charge do metal ions have?

A

Positive.

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4
Q

Why do metal atoms form positive ions?

A

Because they have to lose electrons to fill their outer shell.

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5
Q

What charge do non-metal ions have?

A

Negative

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6
Q

Why do non-metal atoms form negative ions?

A

Because they have to gain electrons to fill their outer shell.

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7
Q

What charge will a magnesium ion have. Explain your answer.

Magnesium is in group 2 of the periodic table.

A

Magnesium ions have a charge of 2+ (Mg2+).

Because they lose two electrons to have a full outer shell.

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8
Q

What charge will a chloride ion have. Explain your answer.

Chlorine is in group 7 of the periodic table.

A

Chloride ions have a charge of 1- (Cl-).

Because they gain an electron to fill their outer shell.

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9
Q

What charge will an oxide ion have. Explain your answer.

Oxygen is in group 6 of the periodic table.

A

Oxide ions have a charge of 2- (O2-).

Because they gain two electrons to fill their outer shell.

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10
Q

What charge will a neon ion have. Explain your answer.

Neon is in group 0 of the periodic table.

A

Neon atoms do not form ions.

Because they have a stable electronic structure/full outer shell of eletrons.

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11
Q

What happens when a metal atoms react with a non-metal atoms?

A

Electrons are transferred from the outer shell of the metal atom to the outer shell of the non-metal atom.

Forming oppsitely charged ions which are attracted to each other.

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12
Q

HIGHER:

What is the formula for sodium bromide? Explain your answer.

Sodium (Na) is in group 1

Bromine (Br) is in group 7

A

NaBr

Each sodium atom loses one electron (Na+) which is gained by a bromine atom (Br-)

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13
Q

HIGHER:

What is the formula for calcium oxide? Explain your answer.

Calcium (Ca) is in group 2

Oxygen (O) is in group 6

A

CaO

Each calcium atom loses two electron (Ca2+) which are gained by an oxygen atom (O2-)

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14
Q

HIGHER:

What is the formula for sodium oxide? Explain your answer.

Sodium (Na) is in group 1

Oxygen (O) is in group 6

A

Na2O

Two sodium atoms lose their outer electron (Na+), which are gained by an oxygen atom (O2-).

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15
Q

HIGHER:

What is the formula for calcium bromide? Explain your answer.

Calcium (Ca) is in group 2

Bromine (Br) is in group 7

A

CaBr2

Each calcium atom loses two electrons (Ca2+), which are gained by two bromine atoms (Br-).

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16
Q

What is the formula and charge of a hydroxide ion?

A

OH-

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17
Q

What is the formula and charge of a hydroxide ion?

A

OH-

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18
Q

TRIPLE

What is the formula (and charge) of a carbonate ion?

A

CO32-

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19
Q

TRIPLE

What is the formula (and charge) of a sulfate ion?

A

SO42-

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20
Q

What type of structure do solid ionic compounds have?

A

A giant lattice structure

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21
Q

Why are ionic compounds such as sodium chloride solid at room temperature?

A

The ions are in a giant lattice.

There are strong attractions between the oppositely charge ions.

It takes lots of energy to break the attractions/ionic bonds.

So they have high melting and boiling points.

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22
Q

In what states do ionic compunds like sodium chloride conduct electricity?

A

When they are…

  • Liquid/molten/melted
  • Aqueous/dissolved/in solution
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23
Q

Why do ionic compunds conduct electricity when they are liquid or aqueous?

A

The ions (charged particles) can move around.

So they can carry an electric current.

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24
Q

Covalent bonds are found…

A

In molecular elements (e.g O2, graphite) and compounds (CO2) made from non-metals.

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25
Q

Do covalent bonds involve…

  1. Sharing electrons
  2. Loss and gain of electrons
  3. Free electrons
A

Atoms share electrons.

To fil their outer shells.

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26
Q

Which of the following contain covalent bonds:

  1. Simple molecular substances (e.g carbon dioxide)
  2. Giant covalent structures (e.g graphite)
  3. Polymers (e.g DNA)
  4. Alloys
A
  1. Simple molecular substances (e.g carbon dioxide)
  2. Giant covalent structures (e.g graphite)
  3. Polymers (e.g DNA)
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27
Q

Which of the following are simple molecular substances and which are giant covalent structures?

Water, graphite, diamond, carbon dioxide, oxygen and methane.

A

Simple molecular substances: Water, carbon dioxide, oxygen and methane.

Giant covalent structures: Graphite and diamond.

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28
Q

Explain why simple molecular substances like water, carbon dioxide, oxygen, methane and nitrogen are liquids or gases at room temperature.

A

The molecules are held together by weak intermolecular forces.

It only takes a small amount of energy to overcome these forces.

They therefore have very low melting and boiling points.

29
Q

Can small molecular substances conduct electricity.

Explain your answer.

A

No

Because the molecules have no ovedrall charge and they do not have free/delocalised electrons.

30
Q

What element are diamond and graphite made from?

A

Carbon

31
Q

Why do diamond and graphite solid at room temperature?

A
  1. The carbon atoms are in a giant structure.
  2. The carbon atoms are held tgether by strong covalent bonds.
  3. It takes lots of energy to break the bonds.
  4. They have very high melting points.
32
Q

Why is diamond really hard?

A

Because each carbon atom has 4 covalent bonds.

The carbon atoms are in a giant lattice.

33
Q

Why can’t diamond conduct electricity?

A

Because it has no delocalised/free electrons or ions.

34
Q

Why is graphite soft? Why can it be used as a lubricant?

A
  1. Because the carbon atoms are in layers (made from hexagons of carbon atoms).
  2. The layers are held together by weak forces.
  3. The layers can slide over each other.
35
Q

Why can graphite conduct electricity?

A
  1. Each carbon atom only has three covalent bonds.
  2. One of the electrons in the outer shell of each carbon atom is free to move around/delocalised.
36
Q

Silicon dioxide (silica) is another giant covalent structure.

  1. What is silicon dioxide made from?
  2. What substance is made from grains of silicon doxide?
A
  1. Silicon and oxygen
  2. Sand
37
Q

Why are sand (silicon dioxide) grains solid?

A
  1. The atoms are in a giant structure.
  2. The silicon and oxygen atoms are held together by strong covalent bonds.
  3. It takes lots of energy to break these bonds.
  4. So sand (silicon dioxide) has a very high melting point.
38
Q

What is graphene?

A

A single layer of graphite/carbon atoms joined together in hexagons.

The

39
Q
  1. What are the properties of graphene?
  2. And what can it be used for?
A
  1. It can conduct electricity (contains delocalised electrons), and it is very light and strong.
  2. It can be used in electronic components and it can be added to composite materials to give them extra strength (without adding weight).
40
Q

Fullerenes are molecules made from carbon. What shapes do they have?

A

Tubes

or

Hollow balls (e.g buckminsterfullerine)

41
Q

What are fullerenes used for?

A

Tubes: Used in electronics (to conduct electricity) and added to sports equipment (e.g tennis rackets) to add strength without adding much weight.

Hollow balls: Delivering drugs, in lubricants and for increasing the surface area of industrial catalysts.

42
Q

Metallic bonds are found…

A

In metal elements and in alloys.

43
Q

Do metallic bonds involve…

  1. Sharing electrons
  2. Loss and gain of electrons
  3. Free/deloclaised electrons
A

Delocalised electrons.

44
Q

Describe how the atoms/ions are bonded together in a piece of metal.

A
  1. Positive metals ions which are surrounded by (shared) delocalised electrons.
  2. The positive metals ions are attracted (electrostatic attractions) to the delocalised electrons.
45
Q

Explain why most metals are solid at room temperature.

A
  1. There are strong (electrostatic) attractions between the metal ions and delocalised electrons.
  2. It takes lots of energy to break the strong attractions.
  3. So they have very high melting points.
46
Q

Explain why metals can conduct electricity and heat?

A
  1. Because they have delocalised electrons.
  2. Which can move around/flow.
  3. And carry electrical current or thermal energy.
47
Q

Metals are malleable. What does malleable mean?

A

Malleable means that they can be bent or hammered into shape, or rolled into sheats.

48
Q

Why are metals malleable?

A

Because the metal atoms/ions can slide over each other.

49
Q

What are alloys?

A

Mixtures of metals.

50
Q

Why are alloys (mixtures of metals) harder than pure metals?

A
  1. It is harder for the metals atoms/ions to slide over each other in alloys.
  2. Because the metals atoms/ions are different sizes.
51
Q

Give examples of alloys.

A

Steel

Bronze

Brass

Gold alloy

Aluminium alloy

52
Q

What type of bond is shown below? How can you tell?

A

An ionic bond.

Because it is an attraction between oppositely charge ions.

53
Q

What type of bond is shown in the diagram below?

How can you tell?

A

Covalent

The atoms are sharing electrons

54
Q

What type of bond is shown in the diagram below?

How can you tell?

What compund is shown?

A

Covalent

The atoms are sharing electrons

Water (H2O)

55
Q

What type of bond is shown in the diagram below?

How can you tell?

A

Metallic

There are positive metal ions attracted to delocalised electrons

56
Q

What type of bond is shown in the diagram below?

What compund is it?

A

Covalent.

Water.

57
Q

Give the four states of matter and the state symbol for each:

  1. Solid (s)
A
  1. Sold (s)
  2. Liquid (l)
  3. Gas (g)
  4. Aqueous (aq): This means dissolved in water
58
Q

For solids, describe the following:

  1. The arrangement of the particles.
  2. The strength of the forces between the particles.
  3. How the particles move.
A

solids

  1. The particles are close together in a fixed position.
  2. There are strong forces between the particles.
  3. The particles vibrate (but do not change position). They vibrate more at higher temperatures.
59
Q

For liquids, describe the following:

  1. The arrangement of the particles.
  2. The strength of the forces between the particles.
  3. How the particles move.
A

Liquids

  1. The particles are close together but can change position (can move past each other).
  2. There are weak forces between the particles.
  3. The particles constantly move (changing position). They move more at higher temperatures.
60
Q

For gases, describe the following:

  1. The arrangement of the particles.
  2. The strength of the forces between the particles.
  3. How the particles move.
A

Gases

  1. The particles are far apart and move freely.
  2. There are very weak forces between the particles.
  3. The particles constantly move (changing position). They move more at higher temperatures.
61
Q

For solids, liquids and gases, say whether they have a

  1. Definite shape
  2. Definite volume
A

Solids: Definite shape and volume (although they can expand slighly when heated).

Liquids: Their shape can change to fill the bottom of their container. They have a definite volume (although they can expand slighly when heated).

Gases: Their shape and volume can change to fill the container they are in.

62
Q

Describe and exaplin what happens during MELTING.

A

Solids change into liquids

The particles have enough energy to break free of the forces holding them in their fixed position, so they begin to move around each other.

63
Q

Describe and exaplin what happens during BOILING.

A
  1. Liquids change into gases.
  2. The particles have enough energy to break free of the forces holding them together so move apart from each other.
64
Q

Describe and exaplin what happens during FREEZING.

A
  1. Liquids change into solids
  2. Bonds form between the particles holding them in a fixed position.
65
Q

Describe and exaplin what happens during CONDENSING.

A
  1. Gases change into liquids
  2. Bonds form between the particles holding them together.
66
Q

The melting point of bromine is -7oC and the boiling point is 59oC. What state is bromine at room temperature (20oC).

Explain your answer.

A

Bromine is a liquid at room temperature.

Because its melting point is below 20oC (room temperature) and its boiling point is above 20oC (room temperature).

67
Q

The melting point of iodine is 114oC and the boiling point is 184oC. What state is iodine at room temperature (20oC).

Explain your answer.

A

Iodine is a solid at room temperature.

Because both its melting and boiling point are above 20oC (room temperature).

68
Q

Chlorine is a gas at room temperature (20oC). What does this tell you about the melting and boiling point of chlorine.

A

They are both lower than 20oC.

Chlorine must have melted and boiled to be a gas.

Chemistry GCSE (10 decks)

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