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Refer to the periodic table while reading the explanation below to understand better.
After gaining three electrons nitrogen ion has the electronic configuration of Ne.
S and Cl after gaining electrons two and one electron respectively have electronic configuration of Ar.
Similarly Br will have that of Kr.
As we go down the group (in this case noble gas group) the size increases as there is an increase in number of electron shell.
Thus Br- is the biggest and N-3 is the smallest.
Now we are left with S-2 and Cl -1.
Atomic number of S is 16 and that of Cl is 17. Thus S-2 has 16 protons and Cl -1 has 17 protons. (Note that proton number does not change. )
Therefore Cl -1 has greater nuclear charge between the nucleus and electrons. (One more proton means one more positive charge which attracts negatively charged electrons. )
The explanation in the square bracket is just an additional info for you.
[ Both have the same number of electrons after gaining respective electrons (electron number similar to that of Ar) therefore, screening effect (interelectronic repulsion) between the shells and between each electron is the same. ]
In conclusion, Cl-1 has stronger attraction between the nucleus and electron shells thus electron shells are closer to the nucleus resulting in smaller size than S-2.
All these above give us the answer A.
Hope this helps.
After gaining three electrons nitrogen ion has the electronic configuration of Ne.
S and Cl after gaining electrons two and one electron respectively have electronic configuration of Ar.
Similarly Br will have that of Kr.
As we go down the group (in this case noble gas group) the size increases as there is an increase in number of electron shell.
Thus Br- is the biggest and N-3 is the smallest.
Now we are left with S-2 and Cl -1.
Atomic number of S is 16 and that of Cl is 17. Thus S-2 has 16 protons and Cl -1 has 17 protons. (Note that proton number does not change. )
Therefore Cl -1 has greater nuclear charge between the nucleus and electrons. (One more proton means one more positive charge which attracts negatively charged electrons. )
The explanation in the square bracket is just an additional info for you.
[ Both have the same number of electrons after gaining respective electrons (electron number similar to that of Ar) therefore, screening effect (interelectronic repulsion) between the shells and between each electron is the same. ]
In conclusion, Cl-1 has stronger attraction between the nucleus and electron shells thus electron shells are closer to the nucleus resulting in smaller size than S-2.
All these above give us the answer A.
Hope this helps.
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