sodium ion Na, +and Ca +2 have very similar atomic radii but hydration enthalpy of Ca2 +is four times than that of Na +
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Explanation:
The nuclear charge of sodium is lower than the nuclear charge of magnesium. Hence, the atomic radius of sodium is greater than that of magnesium.
Due to greater nuclear charge of Mg than that of Na, the attraction of nucleus for outermost electron is stronger for Mg than for Na. Hence, the metallic bond in Mg is stronger than that of Na.
Magnesium has lower melting and boiling points than that of Ca. This is due to higher effective nuclear charge on Ca than Mg which leads to stronger bonds.
Among the alkaline earth metals, Mg and Ca have highest abundance.
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