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Chapter 23: Problem 2

Draw the structure for $\mathrm{Pt}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}$ and use it to answer the following questions: (a) What is the coordination number for platinum in this complex? (b) What is the coordination geometry? (c) What is the oxidation state of the platinum? (d) How many unpaired electrons are there? [Sections 23.2 and 23.6\(]\)

Short Answer

Expert verified
The coordination number for platinum in the complex Pt(C2O4)(NH3)2 is 4, and the coordination geometry is square-planar. The oxidation state of platinum is +4, and there are no unpaired electrons in the complex.

Step by step solution

01

Draw the structure

First, draw a circle to represent the platinum atom (Pt). Draw two lines outwards from Pt on either side to connect the NH3 molecules. Draw a square around Pt and connect the two opposite corners of the square to the two C2O4 molecules. C2O4 is a bidentate ligand hence the square shape represents the two oxygen atoms in the ligand.
02

Determine the coordination number

In this case, we see that Pt is surrounded by and connected to 2 NH3 and 2 C2O4 ligands. The coordination number is the total number of ligands bound to the metal center. So, the coordination number for platinum in this complex is 4.
03

Identify the coordination geometry

The coordination geometry is based on the position of the coordinating groups around the central metal atom. Since the coordination number is 4 and the shape is like a square with one NH3 and one O from C2O4 at each corner, we can safely say that the coordination geometry is square-planar.
04

Calculate the oxidation state of platinum

To calculate the oxidation state of platinum, we can assume the oxidation state of Pt to be x. We know that: 1. The charge on NH3 is 0. 2. C2O4 is a bidentate ligand and has a -2 charge due to the presence of two negatively charged oxygen atoms. So, we can write: x + [2 * (-2)] + [2 * 0] = 0 x - 4 = 0 x = 4 Therefore, the oxidation state of the platinum is +4.
05

Determine the number of unpaired electrons

Now, we must find the electronic configuration of platinum (Pt) in order to determine the number of unpaired electrons. Platinum has an atomic number of 78, and its ground state electronic configuration is [Xe] 4f14 5d9 6s1. But since it has an oxidation state of +4, we need to consider its electronic configuration in the +4 oxidation state, which is [Xe]4f14 5d5. There are no unpaired electrons since all five d-electrons are paired. So, to answer the given questions: a) The coordination number for platinum in this complex is 4. b) The coordination geometry is square-planar. c) The oxidation state of platinum is +4. d) There are no unpaired electrons.

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Most popular questions from this chapter

Write names for the following coordination compounds: (a) \(\mathrm{Na}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{5} \mathrm{NO}\right]\) (b) \(\left[\mathrm{CoO}\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{Br}\) (c) \(\mathrm{Na}_{2}\left[\mathrm{NiBr}_{4}\right]\) (d) $\left[\mathrm{Rh}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]_{3}$

Which transition metal atom is present in each of the following biologically important molecules: (a) hemoglobin, (b) chlorophylls, (c) siderophores, (d) hemocyanine.

Carbon monoxide, CO, is an important ligand in coordination chemistry. When CO is reacted with nickel metal, the product is \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right],\) which is a toxic, pale yellow liquid. (a) What is the oxidation number for nickel in this compound? (b) Given that \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is a diamagnetic molecule with a tetrahedral geometry, what is the electron configuration of nickel in this compound? (c) Write the name for \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) using the nomenclature rules for coordination compounds.

Polydentate ligands can vary in the number of coordination positions they occupy. In each of the following, identify the polydentate ligand present and indicate the probable number of coordination positions it occupies: (a) \(\operatorname{Cr}(\mathrm{EDTA})^{-}\) (b) $\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] \mathrm{Br}_{2}$ (c) $\left[\mathrm{Ru}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{3}$ (d) \(\mathrm{K}_{2}\left[\mathrm{Fe}(\mathrm{O}\) -phen \()(\mathrm{CN})_{4}\right]\)

(a) A compound with formula $\mathrm{RuCl}_{3} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ is dissolved in water, forming a solution that is approximately the same color as the solid. Immediately after forming the solution, the addition of excess \(\mathrm{AgNO}_{3}(a q)\) forms 2 mol of solid \(\mathrm{AgCl}\) per mole of complex. Write the formula for the compound, showing which ligands are likely to be present in the coordination sphere. (b) After a solution of \(\mathrm{RuCl}_{3} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) has stood for about a year, addition of \(\mathrm{AgNO}_{3}(a q)\) precipitates 3 mol of AgCl per mole of complex. What has happened in the ensuing time?
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