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Chapter 23: Problem 31

For each of the following pairs, identify the molecule or ion that is more likely to act as a ligand in a metal complex: (a) acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\) or ammonium \(\left(\mathrm{NH}_{4}^{+}\right)\) (b) hydride \(\left(\mathrm{H}^{-}\right)\) or hydronium \(\left(\mathrm{H}_{3} \mathrm{O}^{+}\right),(\mathbf{c})\) carbon monoxide \((\mathrm{CO})\) or methane \(\left(\mathrm{CH}_{4}\right)\) .

Short Answer

Expert verified
(a) Acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\) is more likely to act as a ligand in a metal complex because it has a lone pair of electrons on the nitrogen atom, while ammonium \(\left(\mathrm{NH}_{4}^{+}\right)\) does not. (b) Hydride \(\left(\mathrm{H}^{-}\right)\) is more likely to act as a ligand in a metal complex because it has a lone pair of electrons, while hydronium \(\left(\mathrm{H}_{3} \mathrm{O}^{+}\right)\) does not. (c) Carbon monoxide \(\left(\mathrm{CO}\right)\) is more likely to act as a ligand in a metal complex because it has a lone pair of electrons on the carbon atom, while methane \(\left(\mathrm{CH}_{4}\right)\) does not.

Step by step solution

01

(a) Acetonitrile (CH3CN) vs Ammonium (NH4+)

Comparing acetonitrile and ammonium, we can see that acetonitrile (CH3CN) has a lone pair of electrons on the nitrogen atom, while ammonium (NH4+) does not have any lone pair of electrons available. Therefore, acetonitrile is more likely to act as a ligand in a metal complex.
02

(b) Hydride (H-) vs Hydronium (H3O+)

In the second pair, hydride (H-) has a lone pair of electrons, while hydronium (H3O+) does not have a lone pair of electrons available for donation. Hence, hydride is more likely to act as a ligand in a metal complex.
03

(c) Carbon Monoxide (CO) vs Methane (CH4)

Comparing carbon monoxide and methane, we observe that the carbon monoxide (CO) molecule has a lone pair of electrons on the carbon atom, while methane (CH4) does not have any lone pair of electrons available for donation. Thus, carbon monoxide is more likely to act as a ligand in a metal complex. So the answers are: (a) Acetonitrile (CH3CN) (b) Hydride (H-) (c) Carbon Monoxide (CO)

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Most popular questions from this chapter

A palladium complex formed from a solution containing bromide ion and pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\) (a good electron-pair 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.

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(a) Sketch a diagram that shows the definition of the crystal-field splitting energy \((\Delta)\) for an octahedral crystal-field. (b) What is the relationship between the magnitude of \(\Delta\) and the energy of the \(d\)-\(d\) transition for a \(d^{1}\) complex? (c) Calculate \(\Delta\) in \(\mathrm{k} J / \mathrm{mol}\) if a \(d^{1}\) complex has an absorption maximum at 545 \(\mathrm{nm} .\)

A manganese complex formed from a solution containing potassium bromide and oxalate ion is purified and analyzed. It contains \(10.0 \% \mathrm{Mn}, 28.6 \%\) potassium, \(8.8\%\) carbon, and 29.2\(\%\) bromine by mass. The remainder of the compound is oxygen. An aqueous solution of the complex has about the same electrical conductivity as an equimolar solution of \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] .\) Write the formula of the compound, using brackets to denote the manganese and its coordination sphere.

The complex \(\left[\mathrm{Mn}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) contains five unpaired electrons. Sketch the energy-level diagram for the \(d\) orbitals, and indicate the placement of electrons for this complex ion. Is the ion a high-spin or a low-spin complex?
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