In chromyl chloride, the number of d-electrons present on chromium is same as in (Given at no. of Ti : 22, V : 23, Cr : 24, Mn : 25, Fe : 26)V (IV) Mn (VII) Fe (III)Ti (III)

The question is asking for the element that has the same number of d-electrons as Chromium in Chromyl Chloride.

1. First, let's determine the oxidation state of Chromium in Chromyl Chloride (CrO2Cl2). The oxidation state of Oxygen is typically -2 and Chlorine is -1. Since there are two Oxygen atoms and two Chlorine atoms, the total negative charge is -6. To balance this, the oxidation state of Chromium must be +6.

2. Chromium (Cr) has an atomic number of 24. The electron configuration of a neutral (uncharged) Cr atom is [Ar] 3d5 4s1. When Cr is in the +6 oxidation state, it loses all 6 of these outer electrons, leaving it with no d-electrons.

3. Now, let's compare this with the other elements given:

   • V (IV): Vanadium (V) has an atomic number of 23. The electron configuration of a neutral V atom is [Ar] 3d3 4s2. When V is in the +4 oxidation state, it loses these 4 outer electrons, leaving it with 1 d-electron.

   • Mn (VII): Manganese (Mn) has an atomic number of 25. The electron configuration of a neutral Mn atom is [Ar] 3d5 4s2. When Mn is in the +7 oxidation state, it loses all 7 of these outer electrons, leaving it with no d-electrons.

   • Fe (III): Iron (Fe) has an atomic number of 26. The electron configuration of a neutral Fe atom is [Ar] 3d6 4s2. When Fe is in the +3 oxidation state, it loses these 3 outer electrons, leaving it with 5 d-electrons.

   • Ti (III): Titanium (Ti) has an atomic number of 22. The electron configuration of a neutral Ti atom is [Ar] 3d2 4s2. When Ti is in the +3 oxidation state, it loses these 3 outer electrons, leaving it with 1 d-electron.

4. Therefore, the number of d-electrons present on Chromium in Chromyl Chloride is the same as in Manganese (Mn) in the +7 oxidation state.