Given that the electronic configuration of an element X is 1s22s22p63s 23p4, it can be deduced that X
-
belongs to group VI in the Periodic Table
- belongs to periodic Table
- contains 3 unpaired electrons in the ground state
- has atomic number 27
The correct answer is: A
Explanation
Adding up the electrons( numbers in the superscript) from the configuration, we have 2+2+6+2+4 = 16. The element with atomic number 16 is Sulphur and it's in group VI.
Alternatively, since the atomic number is 16, it can be deduced that we have 2, 8, 6 when arranged in shells or orbits. Because it the last digit is 6, thus the element belongs to group VI. Option A