The oxide of an element whose electronic configuration is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$ is :

amphoteric.

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basic.

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acidic.

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neutral.

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Solution

The correct option is B basic.
One electron present in outermost s-orbital, so it is a monovalent element.
Hence, the oxide formed will have the chemical formula $M_{2} O$ . Such compounds will be basic oxides.
From electronic configuration, it is seen that it has a total of 11 electrons, so it must be Na atom. Oxide of Na atom $(N a_{2} O)$ gives 2NaOH in aqueous solution.

$N a_{2} O + H_{2} O ⟶ 2 N a O H$

Also, according to their basic behavior, they react with acids in typical acid-base reactions to produce salts and water.
Hence, option $B$ is correct.

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Similar questions

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

An element having electronic configuration 1s², 2s² 2p⁶, 3s² 3p⁶, 4s¹ forms

A

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

B

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}

A

B

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

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