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Chemistry GCSE Mock 2018/19 > Chemistry GCSE: C2 Bonding, Structure and Properties of matter > Flashcards

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

1
Q

Ionic bonds are between…

A

Metal (ions) and non-metal (ions).

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2
Q

Covalent bonds occur…

Give examples.

A

In molecules and compounds made from non-metals.

For examples: Oxygen molecules (O2), water, carbon dioxide, graphite.

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3
Q

Metallic bonds occur…

A

In metal elements and alloys (mixtures/formulations of metal atoms).

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4
Q

In covalent bonds….

Select one of the following:

  • Atoms have lost or gained electrons forming oppositely charged ions which attract each other.
  • Atoms share electrons
  • Metal ions are attracted to delocalised electrons
A

Atoms share electrons

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5
Q

In ionic bonds….

Select one of the following:

  • Atoms have lost or gained electrons forming oppositely charged ions which attract each other.
  • Atoms share electrons
  • Metal ions are attracted to delocalised electrons
A

Atoms have lost or gained electrons forming oppositely charged ions which attract each other.

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6
Q

In metallic bonds….

Select one of the following:

  • Atoms have lost or gained electrons forming oppositely charged ions which attract each other.
  • Atoms share electrons
  • Metal ions are attracted to delocalised electrons
A

Metal ions are attracted to delocalised electrons

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7
Q

What charge do metal ions have?

Explain why

A

A positive charge

  • Because metal atoms lose electrons to fill their outer shells
  • Therefore, they have more positively charged protons than negatively charged electrons.
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8
Q

What charge do non-metal ions have?

Explain why

A

A negatve charge

  • Because non-metal atoms gain electrons to fill their outer shells
  • Therefore, they have more negatively charged electrons han positively charged protons.
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9
Q

What type of structure do solid ionic compounds have?

A

A giant lattice structure

Giant lattice: https://www.bbc.com/bitesize/guides/zqmrsrd/revision/2

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10
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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11
Q

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

Chlorine is in group 7 of the periodic table.

A

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

Because they gain an electron to fill their outer shell.

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12
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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13
Q

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

A

An ionic bond.

  • Because it is an (electrostatic) attraction between oppositely charge ions: Electrons have been lost/gained.
  • It is a bond between matla and non-metal ions.
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14
Q

What type of bond is shown in the diagram below?

How can you tell?

A

Covalent

  • The atoms are sharing electrons
  • It is a bond between non-metal atoms
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15
Q
  1. What type of bond is shown in the diagram below?
  2. How can you tell?
  3. What compund is shown?
A
  1. Covalent
  2. The atoms are sharing electrons: the bonds are between non-metal atoms.
  3. Water (H2O)
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16
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

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17
Q

What type of bond is shown in the diagram below?

What compund is it?

A

Covalent.

Water.

18
Q

Why do ionic compounds have high melting and boiling points?

A
  1. Beacuse they are made of oppositely charge ions held together by strong (electrostatic) attractions.
  2. The ions are in a giant lattice.
  3. It takes lots of energy to break the (electrostatic) attractions/ionic bonds.
19
Q

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

A

When they are…

  1. Liquid/molten/melted
  2. Aqueous/dissolved/in solution
20
Q

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

A

Because the ions (charged particles) can move around.

21
Q

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

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

A

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

Giant covalent structures: Graphite and diamond.

22
Q

Explain why simple molecular substances like water, carbon dioxide, oxygen, methane and nitrogen have low melting and boiling points.

A
  1. Because the molecules are held together by weak intermolecular forces.
  2. It only takes a small amount of energy to overcome these forces.
23
Q

Why are most simple molecuar substances like water and oxygen liquids or gases at room temperature?

A
  1. Because they have low melting and boiling points.
  2. There are only weak intermolecular forces holding the molecules together.
24
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.

25
What element are diamond and graphite madce from?
Carbon
26
Why do diamond and graphite have high melting and boiling points?
1. Because the carbon atoms are held tgether by **strong covalent bonds**. 2. The atoms are in a giant structure. 3. It takes **lots of energy to break the bonds.**
27
Why is diamond really hard?
1. Because each carbon atom has 4 covalent bonds. 2. The carbon atoms are in a giant lattice.
28
Why can't diamond conduct electricity?
Because it has no delocalised electrons or ions.
29
Why is graphite soft? Why can it be used as a lubricant?
1. Because the carbon atoms are in layers. 2. That can slide over each other. 3. Because, the layers are held together by weak forces.
30
Why can graphite conduct electricity?
1. Because there are delocalised electrons. 2. Each carbon atom only has three covalent bonds 3. Therefore, one of the electrons in the outer shell of each carbon atom is free to move around.
31
What is graphene?
A single layer of graphite.
32
What are the propertoes of graphene? And what can it be used for?
Graphene is very light and it can conduct electricity. It can be used in electronic components and it can be added to materials to give them extra strength.
33
Describe how the atoms/ions are bonded together in a piece of metal.
1. The metal atoms form positive ions which are suurounded by delocalised electrons. 2. The positive metals ions are attracted to the delocalised electrons.
34
Explain why most metals are solid at room temperature.
There are **strong attractions** between the metal ions and delocalised electrons. It takes **lots of energy to break** the strong attractions/metallic bonds. So most metals have high melting points.
35
Explain why metals can conduct electricity and heat?
Because they have delocalised electrons. Which can move around/flow/for a current. Which carries energy.
36
Metals are malleable. What does malleable mean?
Malleable means that they can be bent or hammered into shape or rolled into sheats.
37
Why are metals malleable?
Because the metal atoms/ions can slide over each other.
38
What are alloys?
Mixtures/formulations of metals.
39
Why are alloys (mixtures/formulations of metals) harder than pure metals?
1. Because it is harder for the metals atoms/ions to slide over each other in alloys. 2. Because the metals atoms/ions are different sizes.
40
The melting point of bromine is -7oC and the boiling point is 59oC. What state is bromine at room temperature (20oC). Explain your answer.
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).
41
The melting point of iodine is 114oC and the boiling point is 184oC. What state is iodine at room temperature (20oC). Explain your answer.
Iodine is a solid at room temperature. Because both its melting and boiling point are above 20oC (room temperature).
42
Chlorine is a gas at room temperature (20oC). What does this tell you about the melting and boiling point of chlorine.
They are both lower than 20oC. Chlorine must have melted and boiled to be a gas.

Chemistry GCSE Mock 2018/19 (1 decks)

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