Covalent, Ionic and Metallic Bonding

Question 1

Structure between metals?

Answer 1

Giant metallic structure

Question 2

Bonding between metals?

Answer 2

Metallic bonding

Question 3

What is metallic bonding?

Answer 3

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

Question 4

Trend in melting points in metals

Answer 4

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

Question 5

Are metals malleable/ ductile and if yes why?

Answer 5

Yes, because layers of ions can slide over each other

Question 6

Why are metals electrical conductors?

Answer 6

The delocalised electrons can travel through the layers

Question 7

Drawing silver as a metal in the mark scheme

Answer 7

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

Question 8

Group 4 NON-METALS: structure?

Answer 8

Giant macromolecular structure

Question 9

Group 4 NON-METALS: bonding?

Answer 9

Covalent bonding

Question 10

What is covalent bonding?

Answer 10

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

Question 11

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

Answer 11

High because very strong covalent bonds must be broken between atoms

Question 12

Electrical conductivity of silicon dioxide and diamond (group 4)

Answer 12

None as no delocalised electrons or free ions

Question 13

Electrical conductivity of graphite (group 4)

Answer 13

Can conduct as delocalised electrons between layers can move

Question 14

Structure of diamond

Answer 14

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

Question 15

Structure of graphite

Answer 15

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

Question 16

Why can graphite act as a lubricant?

Answer 16

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

Question 17

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

Answer 17

Simple molecular structure

Question 18

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

Answer 18

Covalent bonding

Question 19

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

Answer 19

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

Question 20

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

Answer 20

None due to no free electrons

Question 21

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

Answer 21

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

Question 22

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

Answer 22

IMF

Question 23

Metals and non-metals structure?

Answer 23

Giant ionic structure

Question 24

Metals and non-metals bonding?

Answer 24

Ionic bonding

Question 25

What is ionic bonding?

Answer 25

The strong electrostatic attraction between positive and negative ions

Question 26

Do Metals and non-metals have high melting points?

Answer 26

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

Question 27

Electrical conductivity in ionic solids?

Answer 27

None as no free ions

Question 28

Electrical conductivity in molten or aqueous ionic liquids?

Answer 28

Yes, as ions are free to move through the structure

Question 29

Drawing an ionic lattice mark scheme

Answer 29

3D cube with + and - in correct places

Question 30

What happens across period 3?

Answer 30

- Increased nuclear charge - Atomic radius decreases - Stronger pull on outer shell electrons - Same shielding

Question 31

Why does Aluminium have a higher melting point than sodium

Answer 31

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

Question 32

What is a lattice?

Answer 32

A regular repeating pattern

Question 33

What is the difference between simple molecular and giant macromolecular?

Answer 33

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