In: Chemistry
Which of the following ions does not have the same electron configuration as the noble gas neon?
AI+3
Mg+2
O-2
F-
S-2
The electron configuration is the arrangement of electrons in space around the nucleus.
For Neon(Ne) the atomic number is 10.
Thus, the number of electrons = 10.
The electronic configuration of Ne is as follows:
1s2 2s2 2p6
Now,
1) For Al+3 :
The atomic number of Al is 13, Thus the total number of electrons for neutral aluminum is 13.
After losing 3 electrons, Al+3 ion is formed.
Thus, Al3+ contains 10 electrons.
The electronic configuration of Al+3 is as follows:
1s2 2s2 2p6
Thus, Al+3 ion has the same electronic configuration as the noble gas neon.
2) For Mg+2 :
The atomic number of Mg is 12, Thus the total number of electrons for neutral magnesium is 12.
After losing 2 electrons, Mg+2 ion is formed.
Thus, Mg+2 contains 10 electrons.
The electronic configuration of Mg+2 is as follows:
1s2 2s2 2p6
Thus, Mg+2 ion has the same electronic configuration as the noble gas neon.
3) For O-2 :
The atomic number of O is 8, Thus the total number of electrons for neutral oxygen is 8.
After gaining 2 electrons, O-2 ion is formed.
Thus, O-2 contains 10 electrons.
The electronic configuration of O-2 is as follows:
1s2 2s2 2p6
Thus, O-2 ion has the same electronic configuration as the noble gas neon.
4) For F- :
The atomic number of F is 9, Thus the total number of electrons for neutral fluorine is 9.
After gaining 1 electron, F- ion is formed.
Thus, F- contains 10 electrons.
The electronic configuration of F- is as follows:
1s2 2s2 2p6
Thus, F- ion has the same electronic configuration as the noble gas neon.
5) For S-2 :
The atomic number of S is 16, Thus the total number of electrons for neutral sulfur is 16.
After gaining 2 electrons, S-2 ion is formed.
Thus, S-2 contains 18 electrons.
The electronic configuration of S-2 is as follows:
1s2 2s2 2p6 3s2 3p6
Thus, S2- ion does not have the same electronic configuration as the noble gas neon.