What is the electron configuration for the transition metal...

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. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right]$ Pt forms $+2$ and $+4$ oxidation states in compounds.

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. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right]$
Pt forms $+2$ and $+4$ oxidation states in compounds.

Key Concepts

Electron Removal Order in Metals

In transition metals, the process of ionization typically involves the removal of electrons from the s orbital before the (n-1)d orbitals. This order of removal is crucial for accurately determining the electron configuration of transition metal ions and understanding how different oxidation states are achieved.

Transition Metal Ions

Transition metal ions are species formed when transition metals lose electrons, often leading to partially filled d orbitals. The unique electron configurations of these ions are responsible for many of their characteristic properties including variable oxidation states, magnetism, and the ability to form colorful coordination complexes.

Coordination Chemistry

Coordination chemistry involves the study of compounds in which central metal ions are bonded to surrounding ligands. The arrangement and type of these ligands influence the electron configuration of the metal ion, affecting properties such as reactivity, geometry, and the degree of splitting of the d orbitals.

Electron Configuration

Electron configuration refers to the distribution of electrons in an atom's or ion's orbitals, following principles such as the Aufbau principle, Hund's rule, and the Pauli exclusion principle. In the context of transition metal ions, the electron configuration is adjusted from the neutral atom configuration by removing electrons according to specific rules upon ionization.

Oxidation States

The oxidation state of a transition metal in a complex is determined by balancing the overall charge of the coordination compound with the charges attributed to its ligands. This number indicates how many electrons have been removed from the metal atom, which in turn affects its electron configuration, particularly the occupancy of its d orbitals.

Transcript

00:01 Here the question is what is the electronic configuration for the transition metal ions in each of the following compounds.

00:10 So some complexes are given and in case of complexes first of all we have to identify the metal present in it and after that it's oxidation state.

00:22 Then only we can write the electronic configuration.

00:26 So first of all in case of a, the metal.

00:36 Is iron fe and it is this is cl4 and fe and this is 2 so minus 2 must be here minus 2 that means this should be a plus 2 oxidation state so fe is a plus 2 oxidation state and we know that what is the electronic configuration of fe.

01:15 First we are supposed to know the electronic configuration of the metal when it is neutral that means no ions are present no positive or negative charge then it's electronic configuration atomic number is 26 so it should be after organ up to organ electronic configuration will remain same and after that it should be 4 s2 3d6 and when it is a question of fe plus 2 oxidation state then up to ar it is same two electrons are removed from 4s orbital and then from 3d orbital so this should be 3 d5.

02:25 So this is the electronic configuration of the metal present in the a compound.

02:33 Now come to b compound.

02:35 B compound is again a complex, cobalt complex and in this cobalt complex cobalt is at plus two oxidation state.

02:51 So here again we are supposed to know what is the electronic configuration of cobalt first cobald is at plus two oxidation state cobalt electronic configuration depends upon its atomic number here also october it is same and after that 4 s2 3d 7 and when it is a question of cobalt 2 plus it should be ar and after that 4s remove electron and then 3d cell...

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