Bonding in Metals

Question 1

Metallic bonds

Answer 1

• Metal elements exist as giant metallic lattice structures.
• The outermost electrons of metal atom are delocalised.
• The ions formed are attracted to delocalised electrons and they form lattice of closely packed cations in a sea of delocalised electrons.
• Metallic bonding is the strong electrostatic attraction between cations and delocalised electrons.

Question 2

Properties of metal

Answer 2

• Strong metallic bonds - attraction between positive and delocalised electrons.
• High electrical conductivity
• High melting and boiling points

Question 3

Melting and boiling points

Answer 3

• Most metals have high melting and boiling points.
• Melting point depends on the strength of the metallic holding together the atoms in the giant metallic lattice.
• High temp necessary to provide large amount of energy needed to overcome the strong electrostatic attraction between cations and electrons.
• M.P and B.P increases across period because bonds get stronger as metal ions have greater charge, an increasing no. of delocalised electrons and decreasing ionic radius. This leads to higher charge density.

Question 4

Solubility

Answer 4

Metals are insoluble, except in liquid metals, because of the strength of the metallic bonds.