What is the electron configuration for the transition metal ion(s) in each of the following compounds? a. $\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{4}\right]$ b. $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\right] \mathrm{I}_{2}$ c. \(\mathrm{Na}_{2}\left[\mathrm{TaF}_{7}\right]\) d. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{PtI}_{4}\right]$ Pt forms \(+2\) and \(+4\) oxidation states in compounds.

Short Answer

Expert verified
The electron configurations of the transition metal ions in the given compounds are: a. Fe (+2 oxidation state): \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^6\] b. Co (+3 oxidation state): \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^6\] c. Ta (+5 oxidation state): \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^0 6s^2\] d. Pt (+2 oxidation state): \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^8 6s^1\] Pt (+4 oxidation state): \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^7\]

Step by step solution

01

Identify the transition metal ion and its oxidation state

For each compound, we need to identify the transition metal ion and also the oxidation state of the transition metal ion. a. The transition metal ion in the first compound is Fe. b. The transition metal ion in the second compound is Co. c. The transition metal ion in the third compound is Ta. d. The transition metal ion in the fourth compound is Pt (appearing twice).
02

Determine the oxidation state of the transition metal ion

a. In \(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2}\mathrm{O}\right)_{2} \mathrm{Cl}_{4}\right]\), the oxidation state of Fe is +2. b. In \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{NH}_{2}\mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\right] \mathrm{I}_{2}\), the oxidation state of Co is +3. c. In \(\mathrm{Na}_{2}\left[\mathrm{TaF}_{7}\right]\), the oxidation state of Ta is +5. d. In \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\mathrm{I}_{2}\right]\left[\mathrm{PtI}_{4}\right]\): - For the \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\mathrm{I}_{2}\right]\), the oxidation state of Pt is +2. - For the \(\left[\mathrm{PtI}_{4}\right]\), the oxidation state of Pt is +4.
03

Determine the electron configuration of transition metal ions

Now that we have the oxidation state of the transition metal ions, we can find their electron configurations using the periodic table. a. Fe has an atomic number of 26 and an electron configuration of: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 4s^2\] In the +2 oxidation state, Fe loses 2 electrons, giving the electron configuration: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^6\] b. Co has an atomic number of 27 and an electron configuration of: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^7 4s^2\] In the +3 oxidation state, Co loses 3 electrons, giving the electron configuration: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^6\] c. Ta has an atomic number of 73, and an electron configuration of: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^3 6s^2\] In the +5 oxidation state, Ta loses 5 electrons, giving the electron configuration: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^0 6s^2\] d. Pt has an atomic number of 78, and an electron configuration of: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^9 6s^1\] In the +2 oxidation state, Pt loses 2 electrons as: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^8 6s^1\] In the +4 oxidation state, Pt loses 4 electrons as: \[1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 4f^14 5s^2 5p^6 5d^7\]

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Most popular questions from this chapter

Iron is present in the earth's crust in many types of minerals. The iron oxide minerals are hematite \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\) and magnetite \(\left(\mathrm{Fe}_{3} \mathrm{O}_{4}\right) .\) What is the oxidation state of iron in each mineral? The iron ions in magnetite are a mixture of \(\mathrm{Fe}^{2+}\) and Fe \(^{3+}\) ions. What is the ratio of \(\mathrm{Fe}^{3+}\) to \(\mathrm{Fe}^{2+}\) ions in magnetite? The formula for magnetite is often written as $\mathrm{FeO} \cdot \mathrm{Fe}_{2} \mathrm{O}_{3} .$ Does this make sense? Explain.

Nickel can be purified by producing the volatile compound nickel tetracarbonyl. Nickel is the only metal that reacts with carbon monoxide at room temperature. Assuming this compound is overall neutral, what is the oxidation state of Ni in the compound? Deduce the formula of the compound.

The equilibrium constant \(K_{\mathrm{a}}\) for the reaction $$\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \\\ \quad\quad\quad\quad\quad\quad\quad\quad\quad \mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{2+}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)$$ is \(1.0 \times 10^{-5}\) a. Calculate the pH of a 0.10\(M\) solution of $\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$ b. Will a 1.0\(M\) solution of cobalt(Il) nitrate have a higher or lower pH than a 1.0\(M\) solution of cobalt (III) nitrate? Explain. c. \(\mathrm{Co}^{3+}\) complex ions are generally low-spin cases, whereas \(\mathrm{Co}^{2+}\) complex ions are generally high-spin cases. Explain. If this is the situation, how many unpaired electrons are present in \(\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) and \(\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+} ?\)

Acetylacetone (see Exercise \(45,\) part a), abbreviated acacH, is a bidentate ligand. It loses a proton and coordinates as acac\(^-\) as shown below: Acetylacetone reacts with an ethanol solution containing a salt of europium to give a compound that is 40.1\(\% \mathrm{C}\) and 4.71\(\% \mathrm{H}\) by mass. Combustion of 0.286 \(\mathrm{g}\) of the compound gives 0.112 $\mathrm{g} \mathrm{Eu}_{2} \mathrm{O}_{3} .$ Assuming the compound contains only \(\mathrm{C}, \mathrm{H},\) O, and Eu, determine the formula of the compound formed from the reaction of acetylacetone and the europium salt. (Assume that the compound contains one europium ion.)

Draw all the geometrical isomers of \(\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{BrCl}^{+1}\) . Which of these isomers also have an optical isomer? Draw the various isomers.

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