Explain, in terms of bonding and structure, the difference in the melting point between SrCl2 and SiCl4. ?

1 Answer
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Apr 17, 2018

#SrCl_2# is held together by strong ionic bonds whereas #SiCl_4# is held together by relatively weak intermolecular forces

Explanation:

#SrCl_2# is an ionic compound. In solid #SrCl_2# theparticles are arranged in a lattice structure, held together by strong ionic bonds between the oppositely charged #Sr^(2+)# and #Cl^-# ions.

#SiCl_4# is a covalent compound, and so in solid #SiCl_4#, the molecules are held together by weak intermolecular forces.

Ionic bonds are incredibly strong, and require a lot of energy to break. As a result, ionic compounds have high melting points.

Intermolecular forces are weak, however, requiring less energy to break than ionic bonds, so covalent compounds have low melting points.

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