1. Sodium, magnesium and aluminium are metals. Their melting and boiling points increase across the period becasue the metal-metal bonds get stronger. The bonds get stronger because the metal ions have an increasing number of delocalised electrons and a decreasing radius. This leads to a higher charge density, which attracts the ions together more strongly.
2. Silicon is macromolecular, with a tetrahedral structure - strong covalent bonds link all its atoms together. A lot of energy is needed to break these bonds, so silicon hs high melting and boiling points.
3. Phosphorus (P4), sulphur (S8) and chlorine (Cl2) are all molecular substances. Their melting and boiling points depend upon the strength of the Van der Waals forces between their molecules. Van der Waals are weak and easily overcome so these elements have low melting and boiling points.
4. More atoms in a molecule mean stronger Van der Waals forces. Sulphur is the biggest molecule (S8), so it's got higher melting and boiling points than phosphorus or chlorine.
5. Argon has very low melting and boiling points because it exists as individual atoms (they're monatomic) resulting in very weak Van der Waals.
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