$N a_{2} O$ , $M g O$ , $A l_{2} O_{3}$ and $S i O_{2}$ have heat of formation equal to $- 416, - 602, - 1676$ and $- 911$ $k J m o l^{- 1}$ respectively. The most stable oxide is:

N a_{2} O

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M g O

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A l_{2} O_{3}

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S i O_{2}

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Solution

The correct option is B $M g O$
$(B)$ A smaller higher charged ion will be closer to the oxide ions $(O^{2 -})$ , which means the thermal stability of $M g O$ is more or it takes more energy to break the crystal structure of $M g O$

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