Hard and Soft principle of acids and bases : The Lewis acids and bases are classified as the hard and soft acids and bases. The hardness is defined as property of retaining valence electrons quite strongly. Hence a hard acid is that in which the electron-accepting a atom is small, has the high positive charge and has no electron at all which can be simply polarised or removed for example Li⁺, Na⁺, Be²⁺, Mg²⁺, Al³⁺, BF₃, SO₃ etc.. On contrary, a soft acid is that in which acceptor atom is large in size, carries a low positive charge or it has electrons in the orbitals which are easily polarised or distorted      for example Pb²⁺, cd²⁺, Pt²⁺, Hg²⁺, Ro⁺, Rs⁺, I₂ etc..

The Lewis base which holds its electrons strongly is known as hard base, for example OH^-, F^-, H₂O, NH₃, CH₃OCH₃, etc. or we can say that a Lewis base in which position of the electrons is easily polarised or removed is called a soft base for example I^-, CO, CH₃S^-, (CH₃)₃P, etc.

In common, hard acids prefer to bind to hard bases and the soft acids prefer to bind to soft bases. The bonding between the hard acids and hard bases is chiefly ionic and that between the soft bases and soft acids is majorly covalent.

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