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Chapter 23: Problem 7

Give the highest oxidation states for scandium to copper.

Short Answer

Expert verified
The maximum oxidation states from Scandium to Copper are: Sc(+3), Ti(+4), V(+5), Cr(+6), Mn(+7), Fe(+6), Co(+3), Ni(+4), Cu(+4).

Step by step solution

01

Identify the elements

Firstly, scandium (Sc), titanium (Ti), vanadium (V), chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni), copper (Cu). These are the transition metals from scandium to copper.
02

Identify common oxidation states

Next, scandium (Sc) has a common oxidation state of +3. Titanium (Ti) most commonly shows +4. Vanadium (V) has a maximum oxidation state of +5. Chromium (Cr) can go up to +6. Manganese (Mn) has a highest oxidation state of +7. Iron (Fe) can show oxidation state up to +6 (though +3 and +2 are more common), Cobalt (Co) can show oxidation state up to +3. Nickel (Ni) generally exhibits +2, but can go up to +4. Copper (Cu) shows a common oxidation of +2 with a maximum of +4.
03

Present the results

The oxidation states for each transition metal from Scandium to Copper are as follows: Sc(+3), Ti(+4), V(+5), Cr(+6), Mn(+7), Fe(+6), Co(+3), Ni(+4), Cu(+4).

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Most popular questions from this chapter

A student has prepared a cobalt complex that has one of the following three structures: \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]\) \(\mathrm{Cl}_{3},\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2},\) or \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .\) Explain how the student would distinguish between these possibilities by an electrical conductance experiment. At the student's disposal are three strong electrolytes \(-\mathrm{NaCl}, \mathrm{MgCl}_{2},\) and \(\mathrm{FeCl}_{3}-\) which may be used for comparison purposes.

Draw structures of all the geometric and optical isomers of each of the following cobalt complexes: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+},(\mathrm{b})\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\)

Explain the following facts: (a) Copper and iron have several oxidation states, whereas zinc has only one. (b) Copper and iron form colored ions, whereas zinc does not.

Suggest a method that would allow you to distinguish between \(c i s-\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\) and trans\(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\)

Complete the following statements for the complex ion \(\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{-}:\) (a) The oxidation number of Cr is _____ (b) The coordination number of Cr is _____ . (c)_____ is a bidentate ligand.
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