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GCSE - Chemistry (New) > Section 1 - Pgs 10-14 > Flashcards

Section 1 - Pgs 10-14 Flashcards

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1
Q

How are ions formed?

A

By the loss or gain of electrons in an atom.

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2
Q

What is ionic bonding?

A

When a metal reacts with a non-metal, electrons are transferred from the metal to the non-metal, forming ions. These ions are bonded together due to the strong electrostatic attraction between them.

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3
Q

What charge do metals receive in ionic bonding?

A

Positive

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4
Q

What charge do non-metals receive in ionic bonding?

A

Negative

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5
Q

What is the loss of electrons called?

A

Oxidation

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6
Q

What is the gain of electrons called?

A

Reduction

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7
Q

In ionic bonding, do metals lose or gain electrons?

A

Lose

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8
Q

In ionic bonding, do non-metals lose or gain electrons?

A

Gain

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9
Q

Group 1 and 2 elements are…

A

Metals

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10
Q

Group 6 and 7 elements are…

A

Non-metals

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11
Q

What is a cation?

A

A positively charged ion.

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12
Q

What is an anion?

A

A negatively charged ion.

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13
Q

In ionic bonding, do metals become anions or cations?

A

Cations

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14
Q

In ionic bonding, do non-metals become anions or cations?

A

Anions

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15
Q

What does an element’s group tell you about its structure?

A

It has that many electrons in its outer shell.

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16
Q

What are dot and cross diagrams used for?

A

To show what happens to electrons in bonding.

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17
Q

In diagrams, how are ions represented?

A
  • Square brackets around the ion
  • Charge in the top right corner
  • Number of each ion on the left of it
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18
Q

What type(s) of structure does ionic bonding create?

A
  • Giant ionic
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19
Q

What is a giant ionic structure?

A

An arrangement where ions are held closely together in a 3D lattice by their electrostatic attraction.

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20
Q

What are the properties of giant ionic structures and why?

A
  • High boiling point
  • Conductors of electricity when dissolved or molten
  • Brittle

This is because ionic bonds are strong and a lot of energy is required to break them. Also, they contain ions which are free to move and conduct electricity when the compound is molten. The ions are in fixed positions, so the structure is brittle.

21
Q

What affects the boiling point of giant ionic structures?

A

The charges on the ions in the lattice. (i.e. A structure with 2+ and 2- ions will be held together more strongly than one with 1+ and 1- ions)

22
Q

What is a typical giant ionic structure?

A

Sodium chloride (i.e. salt)

23
Q

What is covalent bonding?

A

When two atoms (non-metals) share electrons to fill their outer shells. There is a strong attraction between the shared electrons and the nucleus of each atom.

24
Q

How many covalent bonds does an atom need to make?

A

As many as the number of electrons it is missing in the outer shell.

24
Q

How many covalent bonds does a hydrogen molecule contain? (H2)

A

1 single bond

25
Q

How many covalent bonds does a chlorine molecule contain? (Cl2)

A

1 single bond

26
Q

How many covalent bonds does a hydrogen chloride molecule contain? (HCl)

A

1 single bond

27
Q

How many covalent bonds does an ammonia molecule contain? (NH3)

A

3 single bonds - The nitrogen makes a single bond with each of the hydrogens

28
Q

How many covalent bonds does a nitrogen molecule contain? (N2)

A

1 triple bond

29
Q

How many covalent bonds does a water molecule contain? (H2O)

A

2 single bonds - The oxygen makes a single bond with each of the hydrogens.

30
Q

How many covalent bonds does an oxygen molecule contain? (O2)

A

1 double bond

31
Q

How many covalent bonds does a carbon dioxide molecule contain? (CO2)

A

2 double bonds - The carbon makes a double bond with each of the oxygens.

32
Q

How many covalent bonds does a methane molecule contain? (CH4)

A

4 single bonds - The carbon forms a single bond with each of the hydrogens.

33
Q

How many covalent bonds does an ethane molecule contain? (C2H6)

A

7 single bonds - The carbons make a single bond with 3 hydrogens each, and a single bond with each other.

34
Q

How many covalent bonds does an ethene molecule contain?

A

4 single bonds and 1 double bond - The carbons make a single bond with 2 hydrogens each, and a double bond with each other.

35
Q

How can each type of bonding be represented?

A

Ionic - Dot and cross diagrams

Covalent - Dot and cross diagrams OR Display formula (e.g. H-H)

36
Q

What type(s) of structure does covalent bonding create?

A
  • Simple molecular

- Giant covalent

37
Q

What are the properties of simple molecular substances and why?

A
  • Low boiling point
  • Not conductive

This is because, although they have strong covalent bonds WITHIN the molecules, the inter-molecular forces are weak and require little energy to overcome. Also, they do not have any free electrons and so are not conductive.

38
Q

What state are most simple molecular structures at room temperature?

A

Liquids or gases (due to low boiling point)

39
Q

What are the properties of giant covalent structures and why?

A
  • Very high boiling point
  • Not conductive (except graphite)
  • Insoluble
  • Hard and brittle

This is because of the large amount of strong covalent bonds which have to be broken in order to melt/boil the substance. Also, they do not have any free electrons or ions (except graphite) to allow them to conduct electricity. The atoms are held in place, making the structure hard and brittle.

40
Q

Give some examples of simple molecular substances.

A
  • Chlorine
  • Oxygen
  • Water
41
Q

Give some examples of giant covalent structures.

A
  • Diamond

- Graphite

42
Q

What is the structure of diamond like?

A
  • Each carbon forms 4 bonds (tetrahedron shape)
  • Strong covalent bonds

Check an image on the internet

43
Q

What is the structure of graphite like?

A
  • Each carbon forms 3 bonds
  • Layers (hexagon shaped bond structure)
  • 1 electron per C delocalised
  • Strong covalent bonds within layers
  • Weak forces between layers
  • Layers slide over each other
  • Check an image on the internet*
44
Q

What is special about graphite?

A

It is a conductor of electricity because each carbon has a free electron. Also, the layers slip over each other, which makes it a good lubricant.

45
Q

What are the properties of diamond like?

A
  • Very high melting point
  • Very hard
  • Insoluble
46
Q

What are the properties of graphite like?

A
  • Very high melting point
  • Conductor of electricity
  • Insoluble
  • Slippery
47
Q

What are the uses of diamond and why?

A

It is used for drill tips and cutting tools. This is because it is hard and insoluble.

48
Q

What are the uses of graphite and why?

A

It is used as a lubricant (for machinery), because the layers slip over each other easily.

GCSE - Chemistry (New) (18 decks)

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