Which of these ions have one d electron in the outmost d subshell?
Zn2+
Fe2+
y2+
Cd2+
Sc2+
Hg2+
Tc2+
To determine which ions have one d electron in the outermost d subshell, we need to consider the electron configuration of each ion.
Let's start by looking at the electron configuration of each ion:
Zn2+ = [Ar] 3d10
Fe2+ = [Ar] 3d6
Y2+ = [Kr] 4d1
Cd2+ = [Kr] 4d10
Sc2+ = [Ar] 3d1
Hg2+ = [Xe] 4f14 5d10
Tc2+ = [Kr] 4d5
From the electron configurations, we can see that Y2+ and Sc2+ have one d electron in the outermost d subshell. Therefore, the ions Y2+ and Sc2+ have one d electron in the outermost d subshell.
To determine which of these ions have one d electron in the outermost d subshell, we need to analyze the electron configuration of each ion.
Zn2+:
The atomic number of zinc (Zn) is 30. Zn2+ indicates that it has lost two electrons, so the electron configuration would be [Ar] 3d10.
Fe2+:
The atomic number of iron (Fe) is 26. Fe2+ indicates that it has lost two electrons, so the electron configuration would be [Ar] 3d6.
Y2+:
The atomic number of yttrium (Y) is 39. Y2+ indicates that it has lost two electrons, so the electron configuration would be [Kr] 4d0.
Cd2+:
The atomic number of cadmium (Cd) is 48. Cd2+ indicates that it has lost two electrons, so the electron configuration would be [Kr] 4d10.
Sc2+:
The atomic number of scandium (Sc) is 21. Sc2+ indicates that it has lost two electrons, so the electron configuration would be [Ar] 3d0.
Hg2+:
The atomic number of mercury (Hg) is 80. Hg2+ indicates that it has lost two electrons, so the electron configuration would be [Xe] 4f14 5d10.
Tc2+:
The atomic number of technetium (Tc) is 43. Tc2+ indicates that it has lost two electrons, so the electron configuration would be [Kr] 4d3.
After analyzing the electron configurations, we can see that only Fe2+ has one d electron in the outermost d subshell.