What is the effect of metallic bonding on the chemical reactivity of metals?

Metallic bonding generally makes metals less chemically reactive due to the strong attraction between positive ions and delocalised electrons.

Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions. It is the main type of bonding that occurs in metals and it gives metals their unique properties such as high melting and boiling points, good electrical conductivity, and malleability.

In terms of chemical reactivity, metallic bonding tends to make metals less reactive. This is because the strong attraction between the positive ions and the delocalised electrons in the 'sea of electrons' model of metallic bonding makes it difficult for other substances to react with the metal ions. The delocalised electrons act as a shield, protecting the positive ions from reacting with other substances.

However, it's important to note that not all metals are equally unreactive. The strength of the metallic bond, and therefore the reactivity of the metal, can vary depending on the number of delocalised electrons per atom and the size of the positive ions. For example, alkali metals like sodium and potassium have only one delocalised electron per atom and relatively large positive ions, which makes their metallic bonds weaker and these metals more reactive.

On the other hand, transition metals like iron and copper have more delocalised electrons per atom and smaller positive ions, which makes their metallic bonds stronger and these metals less reactive. So, while metallic bonding generally makes metals less reactive, the specific reactivity of a metal can be influenced by other factors as well.