Consider the elements $M g, A l, S, P$ and $S i$ the correct increasing order of their first ionization enthalpy is:

M g < A l < S i < S < P

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A l < M g < S i < S < P

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M g < A l < S i < P < S

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A l < M g < S < S i < P

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Solution

The correct option is B $A l < M g < S i < S < P$
In general, from left to right in a period, ionization enthalpy increases due to an increase in effective nuclear charge.
But due to extra stability of half filled $(P)$ and full filled electronic configuration $(M g)$ , required ionisation enthalpy is more from neighbouring elements. i.e., first ionization enthalpy order is
$A l < M g < S i < S < P$

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Similar questions

The first ionistation enthalpies of Na, Mg, Al, and Si are in the order
(a) Na< Mg > Al < Si (b) Na> Mg > Al > Si
(c) Na< Mg< Al< Si (d) Na> Mg> Al < Si

Q. Consider the elements

M g, A l, S, P

and

S i,

the correct increasing order of their first ionization enthalpy is :

Q. The first ionisation energies of six

3^{r d}

period elements are 496, 578, 738, 789, 1000 and 1012

{kJ mol}^{- 1}

. The elements to which these energies correspond respectively are:

Q. Arrange Mg, Al, Si, P and S in the correct order of their ionisation potentials.

Q. Consider the following orderings:

I

A l > S i > P > C l

I I

B e < M g < C a < S r

I I I

I < B r < C l < F

I V

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

Which of these give(s) a correct trend in ionization energy?

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Consider the elements Mg,Al,S,P and Si the correct increasing order of their first ionization enthalpy is:

Consider the elements $M g, A l, S, P$ and $S i$ the correct increasing order of their first ionization enthalpy is: