Explain why the ionic radius of Q is larger than that of M?

The ionic radius of an atom is determined by the number of electrons and the nuclear charge of the atom. In general, as you move down a group in the periodic table, the ionic radius increases because there are more electron shells present, leading to increased shielding of the outer electrons from the nucleus.

In this case, Q is likely located lower in the periodic table compared to M. This means that Q has more electron shells than M, resulting in a larger ionic radius for Q. Additionally, the increased number of electron shells in Q also leads to increased electron-electron repulsion, which further contributes to the larger ionic radius of Q compared to M.

The ionic radius of Q is larger than that of M due to its higher atomic number. The atomic number refers to the number of protons in the nucleus of an atom. As the atomic number increases, the number of electrons also increases. The electrons occupy shells around the nucleus, and as more electrons are added, the outermost shell becomes larger. This results in an increase in the ionic radius.

In the case of Q and M, Q has a higher atomic number than M. Therefore, Q has more electrons and a larger outermost shell, resulting in a larger ionic radius compared to M.