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(A) In the periodic table,as we move from left to right across a period,the effective nuclear charge increases while the number of shells remains the

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$S < Si < Al < Mg < Na$

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(A) In the periodic table,as we move from left to right across a period,the effective nuclear charge increases while the number of shells remains the same. This results in a stronger attraction between the nucleus and the valence electrons,causing the atomic radius to decrease. All the given elements $(Na, Mg, Al, Si, S)$ belong to the $3^{rd}$ period. Following the trend of decreasing atomic radius from left to right,the order is $Na > Mg > Al > Si > S$. Therefore,the increasing order is $S < Si < Al < Mg < Na$.

The increasing order of the atomic radius of $Si, S, Na, Mg, Al$ is

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