Palladium Electron Configuration: 7 Facts You Should Know!

Electronic configuration is the electronic distribution among the atomic orbitals of element representing different energy level. Let us study Palladium’s electronic configuration.

The atomic number of palladium is 46,and the electronic configuration of Pd is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10. It belongs d- block, period 5 and group 10 of elements. A precious metal that was discovered in 1803 by the English has a silvery-white color and a beautiful appearance.

Electronic configuration, nomenclature, and schematic diagram of Palladium will be discussed in this article, in addition to the ground and excited state of the element that is relevant to it.

How to write palladium electron configuration

The correct configuration of Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10, and it can be determined using the steps mentioned below.

  • First, one needs to determine the element’s period. Here Pd, which is a member of the 5 periods. It tells us the total number of shells that were found.
  • The next thing that needs to be done is to figure out how many electrons an element has based on its atomic number. Pd does in fact has a total of 46 electrons.
  • After that, the electron sequence model, also called the “yellow brick road” model, will be used to fill in the complete orbitals in accordance with the electrons that are accessible.
  • The order of rising energy level is 1s 2s 2p and so on, and since Pd has 46 electrons, the configuration of Pd is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d10 5s2.
  • Then calculate the remaining number of electrons, and fill a single electron in each subshell and again start to form the first subshell. In this case we are left with 8 electrons and the next available sub-shell is d, as it has 10 subshells, so initially 5 electrons will be filled, which will leave 3 electrons. After filling the remaining 3 electrons in the first three subshells, the last two subshells will be left. This yield 5d8.
  • This yields the predicted electronic configuration of Pd 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d8.
  • However, the energy of 5d<5s, so for the formation of a stable compound 5d files first then 5s. The correct configuration of Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10.

Palladium electron configuration diagram

The electron configuration is drawn as follows using the octet rule, where the first two electrons were filled followed by 8 and 18 and the remaining 18 were filled in the last orbital which yields 2, 8, 18, and 18 configurations.

Electronic configuration of Pd

Palladium electron configuration notation

The electronic configuration notation of Pd is written as [Kr] 4d10, where Kr represents the electronic configuration of krypton as a noble gas which is 36, followed by the representation of the remaining 10 electrons in the 4d sub-shell.

Palladium unabbreviated electron configuration

The unabbreviated electronic configuration of Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10. As it contains 46 electrons so its unabbreviated electron configuration is the same as the electronic configuration.

Ground state Palladium electron configuration

The standard ground state configuration of Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10.

The excited state of Palladium electron configuration

Pd shows two excited states and is characterized by the shifting of electrons from 4d to 5s subshell.

  • First excited state confugration of Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d9
  • The second excited state confugration of the element is Pd = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d8.

Ground state Palladium orbital diagram

The atomic orbital diagram for the outermost shell of Pd in the ground state is shown below.

Outermost shell electronic configuration of Pd


We are now capable of computing the electrical configuration of Pd, which is denoted by the notation [Kr] 4d10. While we have previously talked about the ground state and the excited state of the element, the configuration of the excited state shifts to [Kr] 4d8 which exhibits diamagnetic behavior in the ground state.

Deepak Poddar

A polymer scientist, teacher, and consultant, Dr. Deepak Poddar is the Guest Faculty in the Department of Chemistry at the Netaji Subhas University of Technology, Delhi. An alumnus of the University of Delhi (B.Sc.) and CIPET, Ahmedabad (M.Sc.), He received Ph.D. in Chemistry (specializing in Biomaterials) from the University of Delhi, India, under the guidance of Professor Purnima Jain. His research area spans biomaterials, polymer functionalization, nanomaterials, and tissue engineering. He emphasizes a multi-disciplinary approach to solving problems and believes in solid collaborative efforts

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