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The solid anhydrous solid \(CoC{l_2}\)is blue in color. Because it readily absorbs water from the air, it is used as a humidity indicator to monitor if equipment (such as a cell phone) has been exposed to excessive levels of moisture. Predict what product is formed by this reaction, and how many unpaired electrons this complex will have.

Short Answer

Expert verified

The product is \(\left( {{\rm{Co}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}{\rm{C}}{{\rm{l}}_6}} \right)\) and it has \(3\) unpaired electrons.

Step by step solution

01

of 2: Given information

  • The solid anhydrous\(CoC{l_2}\)which absorbs water from the air:

\({\rm{CoC}}{{\rm{l}}_2} + 2{{\rm{H}}_2}{\rm{O}} \to {\rm{CoC}}{{\rm{l}}_2} \cdot 2{{\rm{H}}_2}{\rm{O}}\)

  • It is blue colour and the product is exposed to the moisture:

\({\rm{CoC}}{{\rm{l}}_2} \cdot 2{{\rm{H}}_2}{\rm{O}} \overset{moisture}{\rightarrow}{\rm{CCoCl}}{l_2} \cdot 6{{\rm{H}}_2}{\rm{O}}\)

which is pink color, and the final product is:

\({\rm{CoC}}{{\rm{l}}_2} \cdot 6{{\rm{H}}_2}{\rm{O}} \to \left( {{\rm{Co}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}{\rm{C}}{{\rm{l}}_2}} \right)\)and it is purple in colour.

  • The central atom is the transition metal which is attached with \(6\)water molecules.
  • Also there are\(2C{l^ - }ions\), which means the coordination sphere has positive charge\(\left( {{2^ + }} \right):{\left( {{\rm{Co}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{2 + }}\)
  • Let us determine the oxidation state of \(Co\) as we use \(x\)for the oxidation state of\(Co\).
  • As we already know that the general oxidation state of water is\(0\), we can determine the oxidation state of\(Co\) like this:

\(\begin{aligned}{}x + (6 \cdot 0) = + 2\\x = + 2\end{aligned}\)

  • It means the oxidation state of\(Co\) is\( + 2.\)
  • As per the periodic table, the atomic number of\(Co\)is\(27\)and its electronic configuration is\((Ar)3{d^7}4{s^2}\).
  • In oxidation state of \(C{o^{2 + }}\)the electronic configuration is: \((Ar)3{d^7}4{s^0}\)Which means the number of \(d\)-electrons in \({\rm{C}}{{\rm{o}}^{2 + }}\)is \(7\).
02

of 2: Analysis

  • The ligand contributes a pair of electrons to the metal and since \({{\rm{H}}_2}{\rm{O}}\)is a weak field ligand hence, it causes smaller splitting.
  • The magnitude of pairing energy\(\left( P \right)\)is bigger than crystal field splitting energy in octahedral field:\(P > {\Delta _o}\),which means the electron pairs donated by ligand go to the outermost orbitals.
  • From the crystal field diagram we can see that has \(3\)unpaired electrons.

Result

The product is \(\left( {{\rm{Co}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}{\rm{C}}{{\rm{l}}_6}} \right)\) and it has \(3\) unpaired electrons.

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Most popular questions from this chapter

The standard reduction potential for the reaction \({(Co{({H_2}O)_6})^{3 + }}(aq) + {e^ - } \to {(Co{({H_2}O)_6})^{2 + }}(aq)\)is about 1.8 V. The reduction potential for the reaction \({(Co{(N{H_3})_6})^{3 + }}(aq) + {e^ - } \to {(Co{(N{H_3})_6})^{2 + }}(aq)\) is +0.1 V. Calculate the cell potentials to show whether the complex ions, \({(Co{({H_2}O)_6})^{2 + }}\) and/or\({(Co{(N{H_3})_6})^{2 + }}\), can be oxidized to the corresponding cobalt (III) complex by oxygen.

Give the oxidation state of the metal for each of the following oxides of the first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than one oxidation state. It is possible to write these compound formulas in the equivalent format MOโˆ™M2O3, to permitestimation of the metalโ€™s two oxidation states.)

(a) Sc2O3

(b) TiO2

(c) V2O5

(d) CrO3

(e) MnO2

(f) Fe3O4

(g) Co3O4

(h) NiO

(i) Cu2O

Predict the products of each of the following reactions. (Note: In addition to using the information in this chapter, also use the knowledge you have accumulated at this stage of your study, including information on the prediction of reaction products.)

\(\begin{aligned}(a)Fe(s) + {H_2}S{O_4}(aq) \to \\(b)FeC{l_3}(aq) + NaOH(aq) \to \\(c)Mn{(OH)_2}(s) + HBr(aq) \to \\(d)Cr(s) + {O_2}(g) \to \\(e)M{n_2}{O_3}(s) + HCl(aq) \to \\(f)Ti(s) + xs{F_2}(g) \to \end{aligned}\)

Give the oxidation state of the metal, number of \(d\)electrons, and the number of unpaired electrons predicted for \(\left( {Co{{\left( {N{H_3}} \right)}_6}} \right)C{l_3}. \)

Name each of the compounds or ions given in \(Exercise 19.28,\)including the oxidation state of the metal.

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