Create an orbital diagram that represents the ground state of In+3 .

Electronic configuration and orbital diagrams provide locations of electrons in various orbitals. In3+ is a cation with 46 electrons. Its electronic configuration is [Kr] 4d10. The orbital diagram can be prepared using up and down arrows to show the electron spin.

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In3+ is the symbol for the cation of element Indium. This element has an atomic number of 49, which means there are 49 electrons in it.

The electronic configuration provides us the distribution of electrons in orbitals. The atomic orbitals can be defined as the spatial regions, around the atomic nucleus where the electrons are likely to be found. The atomic orbitals can be s, p, d, and f. Each of these orbitals can only accommodate a certain maximum number of electrons. s orbital can accommodate only 2 electrons, while p can accommodate 6 electrons. Similarly, one can find a maximum of 10 electrons and 14 electrons in d and f orbitals, respectively.

For the given question, the electronic configuration of Indium can be written as: 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2, 5p1.

In the case of the cation, In3+, 3 electrons have been lost by the Indium atom to achieve this oxidation state. The loss of 3 electrons will leave a total of 46 electrons in the ion, which needs to be distributed in the various orbitals.

The 3 electrons will be lost from the outermost orbitals, i.e., 5s and 5p and thus, the electronic configuration of In3+ will be written as:

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10

Orbital diagrams indicate which orbitals are completely and/or partially filled with the spin of the electrons indicated using up and down arrows. The orbital diagram of In3+ will be given as:

1s `uarr` `darr`

2s `uarr` `darr`

2p `uarr` `darr` `uarr` `darr` `uarr` `darr`

3s `uarr` `darr`

3p `uarr` `darr` `uarr` `darr` `uarr` `darr`

3d `uarr` `darr` `uarr` `darr` `uarr` `darr` `uarr` `darr` `uarr` `darr` ` `

4s `uarr` `darr`

4p `uarr` `darr` `uarr` `darr` `uarr` `darr`

4d `uarr` `darr` `uarr` `darr` `uarr` `darr` `uarr` `darr` `uarr` `darr` ` `

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