Select the correct order of melting point:

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(C) Carbon $(C)$ has a higher melting point than Silicon $(Si)$ because the $C-C$ bond is stronger than the $Si-Si$ bond in their giant covalent netwo

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Both $(A)$ and $(B)$

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(C) Carbon $(C)$ has a higher melting point than Silicon $(Si)$ because the $C-C$ bond is stronger than the $Si-Si$ bond in their giant covalent network structures. Nitrogen $(N_2)$ exists as a diatomic gas at room temperature due to weak van der Waals forces,while Phosphorus $(P_4)$ is a solid due to stronger intermolecular forces,hence $N $SiO_2$ is a network covalent solid with a very high melting point,whereas $NaCl$ is an ionic solid with a lower melting point compared to $SiO_2$. Therefore,both $(A)$ and $(B)$ are correct.

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