Give the coordination number and oxidation state of the central metal ion in each of coordination compound.
a.[CoCl4(NH3)2]^-
b.Pt(en)2Cl2]^2+
c.K[Co(H2O)2(C2O4)2]
d.[Ru(H2O)2(NH3)2Cl2]Br
a. Coordination number: 6 (Co is bonded to 4 Cl and 2 NH3)
Oxidation state: +3
b. Coordination number: 6 (Pt is bonded to 2 en and 2 Cl)
Oxidation state: +2
c. Coordination number: 6 (Co is bonded to 2 H2O and 2 C2O4)
Oxidation state: +3
d. Coordination number: 6 (Ru is bonded to 2 H2O, 2 NH3, and 2 Cl)
Oxidation state: +3
Give the coordination number and oxidation state of the central metal ion in each of coordination compound.
a.[CoCl4(NH3)2]^-
b.Pt(en)2Cl2]^2+
c.Mg3[CrCl5Br]2
d.K[Co(H2O)2(C2O4)2]
e.[Ru(H2O)2(NH3)2Cl2]Br
a. Coordination number: 6 (Co is bonded to 4 Cl and 2 NH3)
Oxidation state: +3
b. Coordination number: 4 (Pt is bonded to 2 en and 2 Cl)
Oxidation state: +2
c. Coordination number: 6 (Cr is bonded to 5 Cl and 1 Br)
Oxidation state: +3
d. Coordination number: 6 (Co is bonded to 2 H2O and 2 C2O4)
Oxidation state: +3
e. Coordination number: 6 (Ru is bonded to 2 H2O, 2 NH3, and 2 Cl)
Oxidation state: +3
a. [CoCl4(NH3)2]^-
- Coordination number: 6
- Oxidation state of the central metal ion (Co): +3
b. [Pt(en)2Cl2]^2+
- Coordination number: 4
- Oxidation state of the central metal ion (Pt): +2
c. K[Co(H2O)2(C2O4)2]
- Coordination number: 6
- Oxidation state of the central metal ion (Co): +3
d. [Ru(H2O)2(NH3)2Cl2]Br
- Coordination number: 6
- Oxidation state of the central metal ion (Ru): +2
a. To determine the coordination number of the central metal ion in [CoCl4(NH3)2]^-, count the number of ligands bonded to the central metal ion. In this case, the ligands are Cl^- and NH3. There are four Cl^- ligands and two NH3 ligands, so the coordination number is 6.
Next, let's determine the oxidation state of the central metal ion. Since there are four Cl^- ligands, and each Cl^- ion has a charge of -1, the total charge from the Cl^- ligands is -4. The overall charge of the coordination compound is -1, indicating that the central metal ion must have a charge of +3 to balance out the negative charge. Therefore, the oxidation state of the central metal ion, Co, is +3.
b. In [Pt(en)2Cl2]^2+, the coordination number can be determined by counting the number of ligands bonded to the central metal ion. In this case, there are two Cl^- ligands and two en (ethylenediamine) ligands. Therefore, the coordination number is 4.
The oxidation state of the central metal ion, Pt, can be determined by considering the overall charge of the coordination compound. In this case, the overall charge is +2, indicating that the Pt ion needs to have a charge of +2 to balance out the positive charge. Therefore, the oxidation state of the central metal ion, Pt, is +2.
c. In K[Co(H2O)2(C2O4)2], the coordination number can be determined by counting the number of ligands bonded to the central metal ion. In this case, there are two H2O (water) ligands and two C2O4 (oxalate) ligands. Therefore, the coordination number is 4.
The oxidation state of the central metal ion, Co, can be determined by considering the charge of the anion, K^+, which is +1. Since the overall compound is neutral, the Co ion needs to have a charge of +1 to balance out the positive charge from K^+. Therefore, the oxidation state of the central metal ion, Co, is +1.
d. In [Ru(H2O)2(NH3)2Cl2]Br, the coordination number can be determined by counting the number of ligands bonded to the central metal ion. In this case, there are two H2O (water) ligands, two NH3 ligands, two Cl^- ligands, and one Br^- ligand. Therefore, the coordination number is 7.
The oxidation state of the central metal ion, Ru, can be determined by considering the overall charge of the coordination compound. In this case, the overall charge is not provided, so we cannot determine the exact oxidation state of the Ru ion without additional information.