When the substances Si,KCl,CH_3OH,and C_2H_6 | vedclass

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(D) The melting point depends on the strength of intermolecular forces and the type of lattice structure:$1$. $C_2H_6$ (Ethane) is a non-polar molecul

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$C_2H_6 < CH_3OH < KCl < Si$

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(D) The melting point depends on the strength of intermolecular forces and the type of lattice structure:$1$. $C_2H_6$ (Ethane) is a non-polar molecule with weak van der Waals forces (molecular lattice),resulting in the lowest melting point.$2$. $CH_3OH$ (Methanol) is a polar molecule with hydrogen bonding (molecular lattice),which is stronger than the forces in $C_2H_6$.$3$. $KCl$ (Potassium chloride) is an ionic compound with strong electrostatic forces (ionic lattice),requiring more energy to break.$4$. $Si$ (Silicon) forms a giant covalent network (covalent lattice),which has the highest melting point among these substances.Therefore,the correct order of increasing melting point is: $C_2H_6 < CH_3OH < KCl < Si$.

When the substances $Si$,$KCl$,$CH_3OH$,and $C_2H_6$ are arranged in order of increasing melting point,what is the correct order?

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