Among the period 4 transition metals \((\mathrm{Sc}-\mathrm{Zn}),\) which elements do not form ions where there are partially filled \(3 d\) orbitals?

We can determine the electron configurations of the period 4 transition metals through the periodic table: 1. Scandium (Sc): [Ar] 4s² 3d¹ 2. Titanium (Ti): [Ar] 4s² 3d² 3. Vanadium (V): [Ar] 4s² 3d³ 4. Chromium (Cr): [Ar] 4s¹ 3d⁵ 5. Manganese (Mn): [Ar] 4s² 3d⁵ 6. Iron (Fe): [Ar] 4s² 3d⁶ 7. Cobalt (Co): [Ar] 4s² 3d⁷ 8. Nickel (Ni): [Ar] 4s² 3d⁸ 9. Copper (Cu): [Ar] 4s¹ 3d¹⁰ 10. Zinc (Zn): [Ar] 4s² 3d¹⁰

Now, we need to determine which of these elements do not form ions with partially filled 3d orbitals. To do this, we'll examine their possible cations and the resulting electron configurations: 1. Scandium (Sc): Sc³⁺ has the electron configuration [Ar], with no remaining 3d electrons. 2. Titanium (Ti): Ti⁴⁺ has the electron configuration [Ar], with no remaining 3d electrons. 3. Vanadium (V): V⁵⁺ has the electron configuration [Ar], with no remaining 3d electrons. 4. Chromium (Cr): Cr²⁺ has the electron configuration [Ar] 3d⁴. 5. Manganese (Mn): Mn²⁺ has the electron configuration [Ar] 3d⁵. 6. Iron (Fe): Fe³⁺ has the electron configuration [Ar] 3d⁵. 7. Cobalt (Co): Co³⁺ has the electron configuration [Ar] 3d⁶. 8. Nickel (Ni): Ni²⁺ has the electron configuration [Ar] 3d⁸. 9. Copper (Cu): Cu⁺ has the electron configuration [Ar] 3d¹⁰. 10. Zinc (Zn): Zn²⁺ has the electron configuration [Ar] 3d¹⁰.

From the information in Step 2, we can determine that Scandium (Sc), Titanium (Ti), Vanadium (V), Copper (Cu), and Zinc (Zn) are the period 4 transition metals that do not form ions with partially filled 3d orbitals.