Attached.

Propose a structure and d-electrical configuration for each complex and explain, in your words, why this
electron configuration makes sense in light of what you know about transition metal complexes
𝑀𝑛𝐶𝑙2 . 4𝐻2 𝑂
The electronic configuration of manganese (II) is [Ar] 3d5 4s2. Each chloride ion in this combination
contributes one electron toward the formation of a coordination bond with the manganese ion. Mn(II) is
therefore present in MnCl2 in a coordination sphere with a d-electron configuration of 5. Mn(II) is also
present in MnCl24H2O with a d-electron configuration of 5. Because transition metal complexes
frequently have partially filled d-subshells, which have intriguing electronic and chemical properties, this
configuration makes sense.
𝑁𝑖𝐶𝑙2 . 6𝐻2 𝑂
Electronically, nickel (II) has the configuration [Ar] 3d8 4s2. To create a coordination bond with the
nickel ion in this complex, each chloride ion contributes one electron. As a result, Ni(II) is present in
NiCl2 as a coordination sphere with a d-electron configuration of 8. Even though all of the d-orbitals in
this configuration are fully occupied, it makes sense because it is consistent with the tendency of
transition metal complexes to have partially filled d-subshells. In accordance with the coordination
geometry of Ni(II) complexes, the complex's octahedral structure.
𝐶4 𝑆𝑂4 . 5𝐻2 𝑂
The electronic configuration of copper (II) is [Ar] 3d9 4s1. This complex has a coordination number of
four because each sulfate ion (SO4-) contributes four oxygen atoms to the formation of coordination
bonds with the copper ion. Cu (II) is therefore present in CuSO4 in the coordination sphere of a d9electron configuration. The Cu(II) ion is coupled to four oxygen atoms from the sulfate ligands and one
water molecule in the tetrahedral structure of CuSO45H2O.Because it is consistent with transition metal
complexes' propensity to have partially filled d-subshells, this configuration makes sense.
𝐾3 Fe (𝐶𝑁)6
Potassium hexacyanoferrate (III), also known as 𝐾3 Fe (𝐶𝑁)6 , is a complex made up of six cyanide ligands
and six Fe(III) ions. The electronic configuration of iron (III) is [Ar] 3d5 4s2. Each cyanide ion (CN-) in this
complex contributes one electron to the formation of a coordination bond with the Fe(III) ion. The
coordination sphere of Fe(III) in [Fe(CN)6]-3 has a d-electron configuration of 5, and as a result, contains
Fe(III). K3[Fe(CN)6] has an octahedral structure with six cyanide ligands coupled to the Fe(III) ion.The
Fe(III) ion in K3[Fe(CN)6] has an electron configuration of d5, which is consistent with the fact that
transition metal complexes typically have partially filled d-subshells. The...