Question

What would be the most likely charge of an ion formed from an atom with the electron configuration: 1s22s22p63s2 (2 points) +1 -1 +2 -2

Answer 1

Answer : The correct option is, (+2)

Explanation :

The given electronic configuration is, $1s^22s^22p^63s^2$

In the given electronic configuration of an atom, '3s' shell is the outermost shell in which two electrons are present. For the stable configuration, these two electrons will remove easily from the outer shell and atom will carry (+2).

Total number of electrons in the given configuration= 12 electrons

And magnesium is the element which have 12 electrons. Due to the stable electronic configuration, magnesium atom changes their electronic configuration by losing two electrons and $Mg$ atom changes to $Mg^{2+}$ ion.

Hence, the most likely charge of an ion formed from an atom with the given electron configuration would be, (+2)

Answer 2

+2 D. because this atom is magnesium and mag. has a charge of +2