Metallic bonding

Front

What is metallic bonding?

Back

Metallic bonding is the electrostatic attraction between positively charged metal ions and delocalised electrons in a 'sea' of electrons, allowing metals to conduct electricity and heat.

Front

Why does the melting point of metals increase across period 3 from Sodium (Na) to Aluminium (Al)?

Back

The melting point increases due to the increased number of valence electrons contributed to the 'sea', enhancing the attraction between the metal ions and the delocalised electrons.

Front

What property of metals allows them to conduct electricity?

Back

The delocalised electrons are able to move freely, allowing metals to conduct electricity.

Front

What do metals conduct?

Back

Metals conduct both heat and electricity.

Front

Why do metallic compounds conduct electricity as solids?

Back

Valence electrons are mobile, allowing electricity to flow through the metal.

Front

True or False: There are more metals than non-metals in the periodic table.

Back

True.

Front

What is the 'sea of electrons' in metallic bonding?

Back

The 'sea of electrons' refers to the delocalised electrons that are free to move around, which contribute to the conductivity and malleability of metals.

Front

What is the significance of delocalised electrons in metals?

Back

Delocalised electrons allow metals to conduct electricity and heat, and contribute to their malleability and ductility.

Front

How does the size of atoms affect metallic bonding?

Back

As the size of atoms decreases, the attraction between the metal ions and the delocalised electrons increases, leading to higher melting points.

Front

What is the role of valence electrons in metallic bonding?

Back

Valence electrons are the electrons in the outer shell of metal atoms that become delocalised and contribute to the metallic bond.