Na - Mg 2- Al 3- and Si 4- are isoelectronic- their ionic size will follow the order-A- Na - Mg 2- Mg 2- Al 3- Si 4-C- Na - Mg 2- Al 3- Si 4-D- Na - Al 3- Si 4-

The correct option is B Na^+ gt; Mg^2+ gt; Al^3+ gt; Si^4+ nbsp;In isoelectronic species, as the charge on the cation increases, their sizes decreases ...

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Byju's Answer

Standard X

Chemistry

Covalent Bond

Na +, Mg 2+, ...

Question

$N a^{+}$ , $M g^{2 +}$ , $A l^{3 +}$ and $S i^{4 +}$ are isoelectronic, their ionic size will follow the order:

N a^{+} > M g^{2 +} < A l^{3 +} < S i^{4 +}

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N a^{+} < M g^{2 +} < A l^{3 +} < S i^{4 +}

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N a^{+} > M g^{2 +} > A l^{3 +} > S i^{4 +}

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N a^{+} < M g^{2 +} > A l^{3 +} < S i^{4 +}

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Solution

The correct option is C $N a^{+} > M g^{2 +} > A l^{3 +} > S i^{4 +}$
In isoelectronic species, as the charge on the cation increases, their sizes decreases as the charge density increases, thereby decreasing the size of the ion. Thus, the ionic sizes of the given cations, (isoelectronic) decrease in the order.
$N a^{+} > M g^{2 +} > A l^{3 +} > S i^{4 +}$

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Na+, Mg2+, Al3+ and Si4+ are isoelectronic, their ionic size will follow the order:

$N a^{+}$ , $M g^{2 +}$ , $A l^{3 +}$ and $S i^{4 +}$ are isoelectronic, their ionic size will follow the order: