Two electron configuration:
Mg(Ne)3s^2
Zn(Ar)4s^2 3d^10
Using the configurations, explain the difference in relative reactivity of the 2 metals ( which are Mg and Zn)
To explain the difference in relative reactivity between magnesium (Mg) and zinc (Zn) based on their electron configurations, we need to analyze their valence electrons.
Valence electrons are the electrons present in the outermost energy level of an atom. These electrons are crucial in determining an atom's reactivity as they participate in chemical bonding.
1. Electron configuration of Magnesium (Mg):
Mg has an atomic number of 12. The electron configuration of Mg is 1s^2 2s^2 2p^6 3s^2. The noble gas Neon (Ne) is used within brackets to simplify the configuration.
The valence electron configuration of Mg is 3s^2 since the outermost energy level is the 3rd energy level, and there are 2 electrons in the 3s orbital.
2. Electron configuration of Zinc (Zn):
Zn has an atomic number of 30. The electron configuration of Zn is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10. The noble gas Argon (Ar) is used within brackets to simplify the configuration.
The valence electron configuration of Zn is 4s^2 3d^10 since the outermost energy level is the 4th energy level, and there are 2 electrons in the 4s orbital, and 10 electrons in the 3d orbitals.
Now, let's compare the valence electron configurations of Mg and Zn.
Mg: 3s^2
Zn: 4s^2 3d^10
From the comparison, we can observe that Mg has a completely filled 3s^2 orbital, while Zn has a partially filled 4s^2 and completely filled 3d^10 orbitals.
The reactivity of an element is generally determined by its ability to lose or gain electrons during a chemical reaction. Elements tend to react in a way that allows them to achieve a stable electron configuration, often following the "octet rule" to attain a full outer energy level.
Since Mg has two valence electrons in its 3s orbital, it tends to lose these two electrons to achieve a stable and completely filled lower energy level (similar to a noble gas configuration). This makes Mg highly reactive, especially in reactions involving the transfer of electrons.
On the other hand, Zn has a partially filled 4s^2 orbital and a completely filled 3d^10 orbital. It takes more energy to remove electrons from the 4s orbital compared to the 3s orbital in Mg. Therefore, Zn is less reactive than Mg and tends to lose its 2 valence electrons less readily.
In summary, the difference in reactivity between Mg and Zn can be attributed to the difference in their valence electron configurations. Mg readily loses its 2 valence electrons from the 3s orbital, while Zn is less likely to lose its 2 valence electrons from the partially filled 4s orbital.