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Chapter 24: Problem 75

A palladium complex formed from a solution containing bromide ion and pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}\) (a good electronpair donor), is found on elemental analysis to contain \(37.6 \%\) bromine, \(28.3 \%\) carbon, \(6.60 \%\) nitrogen, and \(2.37 \%\) hydrogen by mass. The compound is slightly soluble in several organic solvents; its solutions in water or alcohol do not conduct electricity. It is found experimentally to have a zero dipole moment. Write the chemical formula, and indicate its probable structure.

Short Answer

Expert verified
The chemical formula of the palladium complex is \(\mathrm{PdBr_{2}(C_{5}H_{5}N)_{2}}\), and its probable structure is square planar, in which the palladium atom is coordinated to two bromine atoms and two pyridine ligands.

Step by step solution

01

Calculate the moles of each element

To determine the empirical formula of the complex, we need to find the moles of each element: bromine (Br), carbon (C), nitrogen (N), and hydrogen (H). Assume 100 g of the sample, so the mass percentages directly convert to grams. Moles of Br = \(\frac{37.6\,\text{g}}{79.904\,\text{g/mol}} = 0.471\) mol Moles of C = \(\frac{28.3\,\text{g}}{12.011\,\text{g/mol}} = 2.36\) mol Moles of N = \(\frac{6.60\,\text{g}}{14.007\,\text{g/mol}} = 0.471\) mol Moles of H = \(\frac{2.37\,\text{g}}{1.008\,\text{g/mol}} = 2.35\) mol
02

Find the empirical formula

Now, we have to divide the moles of each element by the smallest value among them (0.471) to find the empirical formula. Moles of Br : \(\frac{0.471}{0.471} = 1\) Moles of C : \(\frac{2.36}{0.471} = 5\) Moles of N : \(\frac{0.471}{0.471} = 1\) Moles of H : \(\frac{2.35}{0.471} = 5\) Thus, the empirical formula is found to be: BrC鈧匟鈧匩
03

Use the properties of the complex

Since the complex is non-conductive when dissolved in water or alcohol, it indicates that the complex is not ionic. The solubility in organic solvents further suggests that the complex has a covalent nature. Moreover, Pyridine (C鈧匟鈧匩) is known as a strong electron-pair donor.
04

Consider the zero dipole moment

The zero dipole moment property suggests that the arrangement of atoms in the complex is likely symmetrical.
05

Determine the probable structure

Given the empirical formula, BrC鈧匟鈧匩, and taking into account that Pyridine (C鈧匟鈧匩) is a strong electron-pair donor, we can determine that a probable structure for the palladium complex is PdBr鈧�(C鈧匟鈧匩)鈧�. In this structure, the palladium atom is coordinated to two bromine atoms and two pyridine ligands. The overall geometry of the complex is square planar, which is symmetrical, meeting the requirement of a zero dipole moment. Hence, the chemical formula of the palladium complex is \(\mathrm{PdBr_{2}(C_{5}H_{5}N)_{2}}\), and its probable structure is square planar, in which the palladium atom is coordinated to two bromine atoms and two pyridine ligands.

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Most popular questions from this chapter

(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 \(2 \mathrm{~mol}\) 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 \(3 \mathrm{~mol}\) of \(\mathrm{AgCl}\) per mole of complex. What has happened in the ensuing time?

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) tetraaquadibromomanganese(III) perchlorate (b) bis(bipyridyl)cadmium(II) chloride (c) potassium tetrabromo(ortho-phenanthroline)cobaltate (III) (d) cesium diamminetetracyanochromate(III) (e) tris(ethylenediammine)rhodium(III) tris(oxalato)cobaltate(III)

(a) What is meant by the term chelate effect? (b) What thermodynamic factor is generally responsible for the chelate effect? (c) Why are polydentate ligands often called sequestering agents?

The \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) ion has an absorption maximum at about \(725 \mathrm{~nm}\), whereas the \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) ion absorbs at about \(570 \mathrm{~nm} .\) Predict the color of each ion. (b) The \(\left[\mathrm{Ni}(\mathrm{en})_{3}\right]^{2+}\) ion absorption maximum occurs at about \(545 \mathrm{~nm}\), and that of the [Ni(bipy) \(\left._{3}\right]^{2+}\) ion occurs at about \(520 \mathrm{~nm}\). From these data, indicate the relative strengths of the ligand fields created by the four ligands involved.

For each of the following metals, write the electronic configuration of the atom and its \(3+\) ion: (a) \(\mathrm{Ru}\), (b) Mo, (c) Co. Draw the crystal-field energy-level diagram for the \(d\) orbitals of an octahedral complex, and show the placement of the \(d\) electrons for each \(3+\) ion, assuming a weak-field complex. How many unpaired electrons are there in each case?
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