Final answer:
The charge on a d-subshell metal ion can be determined by its electronic configuration and is typically indicated by the ion's color, with partially filled d subshells forming colored complexes and empty or filled d subshells forming colorless complexes. The number of electrons removed or added to the atom's d subshell corresponds to the ion's charge.
Step-by-step explanation:
The charge on a d-subshell metal ion can usually be determined by examining its electronic configuration, which can be deduced from the oxidation state of the metal in the compound. When a metal ion has a partially filled d subshell, it can form colored complex ions, while ions with an empty (d°) or filled (dⁱ⁰) d subshell typically form colorless complexes. This is because the electrons in the d subshell can absorb visible light, causing coloration when they transition between energy levels.
To determine the charge on the d-subshell metal, one can use the concept that the number of electrons removed or added to the metal's atom corresponds to the charge of the ion. For example, if an iron atom (Fe) in its elemental form loses two electrons, it becomes a Fe²⁺ ion with a 3d⁶ configuration. Similarly, if it loses three electrons, it becomes a Fe³⁺ ion with a 3d⁵ electronic configuration. The principal quantum number (n) indicates which shell the d subshell is in, such as 3d for n = 3.
The atomic and ionic electronic configurations help verify the charge state by adding the superscripts of subshells, considering electron loss or gain. This calculation ensures all electrons are placed correctly in their subshells in the proper order, as illustrated by the example of verifying 50 electrons: 2 + 2 + 6 + 2 + 6 + 2 + 10 + 6 + 2 + 10 + 2 = 50.