To find the number of unpaired electrons in a molecule, you need to determine the electron configuration of each atom within the molecule. Unpaired electrons are usually found in the valence shell, which is the outermost shell of an atom.
In the case of MgSO4, let's determine the electron configuration for each atom:
- Magnesium (Mg): The atomic number of magnesium is 12, so the electron configuration is 1sĀ² 2sĀ² 2pā¶ 3sĀ². Since it loses two electrons to form a stable divalent cation (MgĀ²āŗ), it has a completely filled valence shell. Therefore, magnesium has 0 unpaired electrons.
- Sulfur (S): The atomic number of sulfur is 16, so the electron configuration is 1sĀ² 2sĀ² 2pā¶ 3sĀ² 3pā“. Sulfur needs two electrons to complete its valence shell, so it can form two single covalent bonds. Thus, sulfur has 2 unpaired electrons.
- Oxygen (O): The atomic number of oxygen is 8, so the electron configuration is 1sĀ² 2sĀ² 2pā“. Oxygen needs two electrons to complete its valence shell, so it can form two single covalent bonds. Therefore, oxygen has 2 unpaired electrons.
Now let's calculate the total number of unpaired electrons in MgSO4:
Mg: 0 unpaired electrons
S: 2 unpaired electrons
O: 2 unpaired electrons
Total unpaired electrons = 0 + 2 + 2 = 4 unpaired electrons.
So, the correct number of unpaired electrons in the MgSO4 molecule is 4, not 10.