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Chemistry > 2. Bonding, Structure and the Properties of matter (Ions, Ionic and Metallic Bonding) > Flashcards

2. Bonding, Structure and the Properties of matter (Ions, Ionic and Metallic Bonding) Flashcards

1
Q

What are ions?

A

Ions are charged particles due to the loss or gain of electrons

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2
Q

What are positive ions called?

A

Cations

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3
Q

What are negative ions called?

A

Anions

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4
Q

How are positive ions formed?

A

When an atom loses electrons, which are negatively charged, the overall charge becomes positive

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5
Q

How are negative ions formed?

A

When an atom gains electrons, which are negatively charged, so the overall charge becomes negative

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6
Q

What ions do Group 1 atoms form?

A

+1 ions

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7
Q

What ions do Group 7 atoms form?

A

1-

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8
Q

What ions do Group 2 atoms form?

A

2+

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9
Q

What ions do Group 6 atoms form?

A

2-

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10
Q

What are group 7 ions called?

A

Halide ions

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11
Q

What is an ionic bond?

A

The strong electrostatic force of attraction between a positively charged ion and a negatively charged ion between a metal and non-metal

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12
Q

What is ionic bonding between?

A

A metal and a non-metal

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13
Q

What does ionic bonding involve?

A

The transferring of electrons

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14
Q

Explain how an Ionic bond works?

A
  1. In order to gain a full outer shell, the metal will transfer electrons to the non-metal
  2. The metal now has a full outer shell and a positive charge, the non-metal has gained electrons and will also have a full outer shell but now has a negative charge
  3. Now as the ions are oppositiely charged, they are attracted to one another, hence an ionic bond
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15
Q

What does the dot and cross model show?

A

The transferring of electrons

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16
Q

What structure will ionic bonds form?

A

A lattice structure

17
Q

What is a lattice structure?

A

A regular repeating pattern

18
Q

What is an electrostatic force of attraction?

A

The force between unlike charges

19
Q

What ions are bigger than the other in a lattice structure?

A

The negative ions are bigger than positive ions

20
Q

What are the properties of ionic compounds?

A
  • They have high melting and boiling points
  • They cannot conduct electricity in solid form, they must be in molten or aqueous form
21
Q

Why do ionic bonds have high melting and boiling points?

A

Due to the strong electrostatic force of attraction between the positive and negative ions, which requires a lot of energy to overcome

22
Q

Why can’t ionic bonds conduct electricity in solid form and only molten/aqueous?

A
  • the ions are not free to move in a solid form
  • so must be in a molten or aqueous form so that the ions are free to move
  • and are able to carry an electrical charge
23
Q

What does molten mean?

A

Liquid (has been melted)

24
Q

What does aqueous mean?

A

dissolved in water

25
Q

Why can’t solid ionic compounds conduct electricty?

A
  • The strong electrostatic forces of attraction between oppositely charged ions arranged in a regular lattice structure
  • means that they are in fixed positions so are unable to move
  • so they can’t carry a charge
  • so cannot conduct electricty
26
Q

Why can molten/aqueous ionic compounds conduct electricty?

A
  • an aqueous ionic compound means the ionic compound has been dissolved into a solution
  • Molten means that heat has been applied to melt the ionic compound and overcome the electrostatic forces of attraction
  • so the ions are free to move
  • so can carry an electrical charge
  • so can conduct electricty
27
Q

What is metallic bonding?

A

The electrostatic attraction between positively charged metal ions and negatively charged electrons in a lattice structure

28
Q

Why are metallic bonds arranged in a lattice structure?

A

Due to the strong electrostatic force of attraction between the positive metal ions and the sea of delocalised electrons

29
Q

What are the properties of metals? (4)

A
  • High melting and boiling points
  • Good conductors of electricty
  • Malleable
  • Ductile
30
Q

Why do metals have high melting and boiling points?

A

Because a lot of energy is required to overcome the strong electrostatic force of attraction

31
Q

Why are metals good conductors of electricity?

A
  • As the delocalised electrons are free to move
  • so can carry an electrical charge
  • through the metal structure
32
Q

What does malleable mean?

A

Able to be moulded / bent into shape

33
Q

Why are metals malleable?

A

Because the regular layers means the layers can slide over each other easily when force is applied

34
Q

What does ductile mean?

A

Able to be drawn into wires

35
Q

What are alloys?

A

A mixture of 2 or more metals

36
Q

Why are alloys harder than regular metals?

A
  • Because they are a mix of different metals, which have different shapes and sizes, so distort the regular layers of the pure metal
  • So is harder for the layers to slide over each other, so are less malleable, therefore harder

Chemistry (34 decks)

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