Iodide and diamond crystals both contain covalent bonds and yet the physical properties of their crystals are very different. Their melting points are 387K and 3827K respectively. State this type of structure present in each case and explain why the melting point of diamond is so high.
please help
Did you mean iodine and not iodide.
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Iodide (I2) and diamond (C) crystals both contain covalent bonds but have different physical properties due to the type of structure present in each case.
Iodide (I2) has a molecular structure, meaning it consists of individual I2 molecules held together by intermolecular forces. These intermolecular forces are relatively weak, resulting in a low melting point of 387K.
On the other hand, diamond is a giant covalent structure that forms a three-dimensional network of carbon atoms bonded together by strong covalent bonds. In diamond, each carbon atom is bonded to four neighboring carbon atoms, forming a rigid and stable lattice structure.
The high melting point of diamond, which is 3827K, is due to the strong covalent bonds between carbon atoms. These bonds require a significant amount of energy to break, hence the high temperature required for melting. The strong covalent bonds in diamond give it a high melting point, exceptional hardness, and excellent thermal conductivity.
In summary, the difference in melting points between iodide and diamond is due to the difference in the strength and type of bonding present in their respective crystal structures. Iodide has weak intermolecular forces, resulting in a low melting point, while diamond has strong covalent bonds, leading to a high melting point.