Question

When magnesium forms an ion, it loses electrons. How many electrons does it lose, and which orbitals do the electrons come from?

Answer 1

Answer:

2 electrons,   3S orbitals

Explanation:

magnesium is a metal and loses electrons to achieve its stable state. It has an atomic number of 12. with only two electrons in its valence shell. its electron configuration is;

2,8,2 according to shells and;

$1s^{2}, 2s^{2}, 2p^{6}, 3s^{2}$ according to arrangement of electrons in orbitals.

when magnesium forms an ion it loses its 3 electron found in its valence shell, this corresponds with the 3s orbital which contains 2 electrons.

Answer 2

To become an ion, Mg loses 2 electrons from the 3s orbitals and has been converted to $\rm Mg^2^+$.

Magnesium has been the metal of group 2. The metals have the tendency to lose electrons in order to attain a stable configuartion.

The atomic number of magnesium has been 12. The electronic configuration of the metal has been:

$\rm 1s^2\;2s^2\;2p^6\;3s^2$

In order to attain the stable shell configuration, Mg loses 2 electrons from the outermost shell. The outermost shell of Mg has been 3s.

Thus, to become an ion, Mg loses 2 electrons from the 3s orbitals and has been converted to $\rm Mg^2^+$.

For more information about the formation of ions, refer to the link:

https://brainly.com/question/305470