Metallic Bonding

Question 1

What is metallic bonding?

Answer 1

A strong electrostatic attraction between positive metal ions and delocalised electrons.

Metallic bonding involves a lattice structure of positive ions with delocalised electrons that can move freely.

Question 2

What are delocalised electrons?

Answer 2

Electrons from the outer shell of metal atoms that can move freely throughout the metallic structure.

They are not fixed to a particular atom.

Question 3

What is the structure of metals?

Answer 3

A giant lattice structure of positive ions layered in three dimensions.

This structure contributes to the unique properties of metals.

Question 4

List the key properties of metals due to metallic bonding.

Answer 4

• Electrical conductivity
• Thermal conductivity
• High melting and boiling points
• Malleability
• Ductility

These properties stem from the presence of delocalised electrons and the strong metallic bonds.

Question 5

How does electrical conductivity occur in metals?

Answer 5

Due to the delocalised electrons, which are free to move.

This allows metals to conduct electricity.

Question 6

What is malleability in metals?

Answer 6

The ability to be shaped without breaking, as layers of positive ions slide over each other while maintaining strong metallic bonds.

This occurs because the delocalised electrons move with the layers.

Question 7

What is ductility in metals?

Answer 7

The ability to be pulled into wires, as positive ions roll over each other while delocalised electrons move with them.

This ensures strong metallic bonds remain intact.

Question 8

How does the size of metal atoms affect melting points?

Answer 8

Melting points decrease as atoms get larger due to increased shielding and weakened electrostatic attraction.

Larger metals have more electron shells and electrons, leading to weaker metallic bonds.

Question 9

What is the melting point of lithium?

Answer 9

181 °C

Lithium is a group 1 metal.

Question 10

What is the melting point of beryllium?

Answer 10

1278 °C

Beryllium is a group 2 metal.

Question 11

Why do group 2 metals have higher melting points than group 1 metals in the same period?

Answer 11

Group 2 metals have two delocalised electrons per positive ion, leading to greater electron density and stronger electrostatic attraction.

This results in stronger metallic bonds.

Question 12

Fill in the blank: The _______ model is used to explain the properties of metallic bonding.

Answer 12

[metallic bonding]

This model helps in understanding the behavior of metals under various conditions.

Question 13

True or False: The electrostatic attractions between positive ions and delocalised electrons are weak in larger metals.

Answer 13

True

This weakening leads to lower melting points in larger metals.