Metals constitute the majority of elements in our periodic table of elements. They are extremely useful for a number of application due to their unique properties, especially, electrical conductivity, high melting and boiling points, malleability and ductility etc. Metals have attained their unique properties due to their atomic structure. Metals have valence electrons that can be donated and these valence electrons have a high degree of freedom of movement. For example, alkali metals (such as sodium, potassium, etc.) have only 1 valence electron and they donate it readily to form cations. Similarly, alkaline earth metals donate 2 electrons to form ions and (subsequently) compounds.
Metals have very strong metallic bonds between individual atoms and valence electrons are free to move along these bonds. These metallic bonds are the reason metals have high melting and boiling points. The metallic atoms are arranged in a very organized manner and individual layers of these atoms can slide over each other, providing the much used property of malleability.
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