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Explanation

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The melting points and boiling points of sodium, magnesium, and aluminum increase from sodium to aluminum because the number of delocalized electrons increases, making the metallic bonds stronger. As a result, more heat energy is needed to melt or boil aluminum than magnesium, and more heat is needed for magnesium than sodium since aluminum has the strongest metallic bonds due to the most delocalized electrons.

Explanation: the trend of MP and BP
across a Period 3
Na, Mg and Al
? Metals with metallic bonding.
? Thus, relatively high mp and bp.
? Going from Na to Al,
_ No. of delocalize e- increases
_ Metallic bond stronger
_ More heat energy needed
_ Bp & mp increase in order of :
Na < Mg < Al

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Explanation

1. Explanation: the trend of MP and BP across a Period 3 Na, Mg and Al ? Metals with metallic bonding. ? Thus, relatively high mp and bp. ? Going from Na to Al, _ No. of delocalize e- increases _ Metallic bond stronger _ More heat energy needed _ Bp & mp increase in order of : Na < Mg < Al