Which option orders the elements from least to greatest first ionization energy A. Mg, AI, S, Ar
B. Ar, S, AI, Mg
C. Mg, Ar, AI, S
D. Ar, Mg, S, AI

A. Mg, AI, S, Ar

Explanation:

First of all we will discuss the trend of ionization energy along period.

As we move from left to right across the periodic table the number of valance electrons in an atom increase. The atomic size tend to decrease in same period of periodic table because the electrons are added with in the same shell. When the electron are added, at the same time protons are also added in the nucleus. The positive charge is going to increase and this charge is greater in effect than the charge of electrons. This effect lead to the greater nuclear attraction. The electrons are pull towards the nucleus and valance shell get closer to the nucleus. As a result of this greater nuclear attraction atomic radius decreases and ionization energy increases because it is very difficult to remove the electron from atom and more energy is required.

All these elements are present in period 2 magnesium is present on left side thus it has lowest ionization energy then comes Al, S and at the end argon is present. Thus argon have greatest ionization energy.

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