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Chemistry A Level > Covalent, Ionic and Metallic Bonding > Flashcards

Covalent, Ionic and Metallic Bonding Flashcards

1
Q

Structure between metals?

A

Giant metallic structure

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2
Q

Bonding between metals?

A

Metallic bonding

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3
Q

What is metallic bonding?

A

Electrostatic attraction between positive ions and delocalised electrons in a layered structure

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4
Q

Trend in melting points in metals

A

Al3+ is stronger than Mg2+ which is stronger than Na+ as it has more protons and more delocalised electrons so a stronger metallic bond

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5
Q

Are metals malleable/ ductile and if yes why?

A

Yes, because layers of ions can slide over each other

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6
Q

Why are metals electrical conductors?

A

The delocalised electrons can travel through the layers

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7
Q

Drawing silver as a metal in the mark scheme

A

6 same sized particles attached , each with a single + in the centre

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8
Q

Group 4 NON-METALS: structure?

A

Giant macromolecular structure

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9
Q

Group 4 NON-METALS: bonding?

A

Covalent bonding

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10
Q

What is covalent bonding?

A

Electrostatic attraction between a shared pair of electrons and a positive nucleus

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11
Q

What is the melting point of group 4 non-metals?

A

High because very strong covalent bonds must be broken between atoms

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12
Q

Electrical conductivity of silicon dioxide and diamond (group 4)

A

None as no delocalised electrons or free ions

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13
Q

Electrical conductivity of graphite (group 4)

A

Can conduct as delocalised electrons between layers can move

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14
Q

Structure of diamond

A

4 carbon atoms covalently bonded in tetrahedral structure 109.5 degree bond angle

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15
Q

Structure of graphite

A

3 Carbon atoms covalently bonded in a hexagonal layered structure, 4th electron delocalised between the layers. Bond angle 120 degrees between carbon atoms

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16
Q

Why can graphite act as a lubricant?

A

Weak van der waal forces between the layers allows the layers to slide past each other

17
Q

Group 5,6,7,8 non metals structure?

A

Simple molecular structure

18
Q

Group 5,6,7,8 non metals bonding?

A

Covalent bonding

19
Q

Group 5,6,7,8 non metals melting point?

A

Low because of weak IMF between molecules so they are easily broken.

20
Q

Group 5,6,7,8 non metals electrical conductivity?

A

None due to no free electrons

21
Q

Why is the melting point of S8 higher than P4 than Cl2?

A

S8 has more electrons/ is a bigger molecule than P4, than Cl2 than a noble gas do it has more intermolecular forces so needs more energy to break the weak forces

22
Q

When discussing simple molecular structures what should you talk about to get marks?

A

IMF

23
Q

Metals and non-metals structure?

A

Giant ionic structure

24
Q

Metals and non-metals bonding?

A

Ionic bonding

25
Q

What is ionic bonding?

A

The strong electrostatic attraction between positive and negative ions

26
Q

Do Metals and non-metals have high melting points?

A

Yes because the strong electrostatic forces between positive and negstive ions need lots of energy to break a strong bond

27
Q

Electrical conductivity in ionic solids?

A

None as no free ions

28
Q

Electrical conductivity in molten or aqueous ionic liquids?

A

Yes, as ions are free to move through the structure

29
Q

Drawing an ionic lattice mark scheme

A

3D cube with + and - in correct places

30
Q

What happens across period 3?

A
  • Increased nuclear charge
  • Atomic radius decreases
  • Stronger pull on outer shell electrons
  • Same shielding
31
Q

Why does Aluminium have a higher melting point than sodium

A

No. of outer shell electrons increases so more electrons can be delocalised leading to a greater attraction between positive ions and delocalised electrons

32
Q

What is a lattice?

A

A regular repeating pattern

33
Q

What is the difference between simple molecular and giant macromolecular?

A

Giant breaks actual covalent bonds, simple breaks weak intermolecular forces between molecules

Chemistry A Level (25 decks)

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