What is the electronic configuration of the most electropositive element in the Periodic Table?

The most electropositive element in the Periodic Table is cesium (Cs), which can be found in Group 1 of the alkali metals. The electronic configuration of cesium is derived from the arrangement of electrons in its atomic orbitals. The atomic number of cesium is 55, and the electron configuration reflects the distribution of its 55 electrons.

The correct electronic configuration is [Xe] 6s1. This indicates that cesium has a core electron configuration that reflects all the electrons in xenon (the noble gas preceding cesium in the periodic table), followed by one additional electron in the 6s orbital. The presence of this single electron in the highest energy level (6s) contributes to cesium's high electropositivity; it readily loses this electron to form positive ions.

Understanding that Group 1 elements are characterized by having a single electron in their outermost shell helps illustrate why cesium, and therefore the configuration [Xe] 6s1, is established as the most electropositive element. The other choices include different configurations that either misrepresent the number of electrons that cesium possesses or involve higher energy levels that do not apply to the placement of cesium in the periodic table.