METALLIC BOND

Front

What is a metallic bond?

Back

A metallic bond is the attraction between positive metal ions and free-moving electrons.

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 contributing to the 'sea' of electrons.

Front

What property of metals allows them to be drawn into thin wires?

Back

Ductility.

Front

Why do metallic compounds conduct electricity as solids?

Back

Metallic compounds conduct electricity as solids because the valence electrons are mobile, allowing electricity to flow through the metal.

Front

What is the role of delocalized electrons in metallic bonding?

Back

Delocalized electrons create a 'sea' of electrons that hold the metal ions together and allow for conductivity.

Front

How does the structure of metals contribute to their malleability?

Back

The layers of atoms in metals can slide over each other without breaking the metallic bond, allowing metals to be shaped.

Front

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

Back

The 'sea of electrons' allows for conductivity, malleability, and ductility in metals.

Front

Why do metals have high melting points?

Back

Metals have high melting points because the negatively charged electrons act as a glue to hold the positively charged ions together.

Front

What is the effect of increasing the number of valence electrons on metallic bonding?

Back

Increasing the number of valence electrons strengthens the metallic bond, leading to higher melting points.

Front

What is the relationship between metallic bonding and electrical conductivity?

Back

Metallic bonding allows for free-moving electrons, which are responsible for the electrical conductivity of metals.