1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
The noble gas electron configuration for barium is [Xe] 6s2.
The atom with an electron configuration ending in 5s2 is Barium (Ba), a chemical element with atomic number 56. In its ground state, Barium has two electrons in the 5s orbital.
The element with the noble gas notation Xe6s2 is Barium (Ba), as Xenon (Xe) represents the 5s and 5p orbitals of the previous noble gas configuration, and the 6s represents the outermost electron shell of Barium.
Barium forms a +2 charge, along with all other group 2 metals.
Hydrogen electron configuration will be 1s1.
The electron configuration for neutral Barium is [Xe] 6s2. Barium plus 2 means it has lost 2 electrons, so the electron configuration for Barium plus 2 would be [Xe].
The condensed ground state electron configuration for Barium is [Xe] 6s^2. This indicates that Barium has a full inner electron shell (represented by the noble gas configuration of Xenon) and two electrons in the outermost 6s orbital.
The element with an outermost electron configuration of 6s2 is Barium (Ba). It is classified as an alkaline earth metal on the periodic table.
The noble gas electron configuration for barium is [Xe] 6s2.
Two electrons
I assume you mean the Nobel gas electron configuration abbreviation for barium.[Ne] 6s2=======
This electron configuration is for osmium (Os).
Barium has 2 electrons in its outermost shell. To achieve a noble gas electron configuration similar to xenon, which has 8 electrons in its outermost shell, barium would need to give up 2 electrons. This would leave barium with a full outer shell and a stable electron configuration.
All alkaline earth metals have electron configurations ending in s2; 6s2 would be the alkaline earth metal in period 6 of the PTE, which is barium.
The atom with an electron configuration ending in 5s2 is Barium (Ba), a chemical element with atomic number 56. In its ground state, Barium has two electrons in the 5s orbital.
The element E is likely barium (Ba), as its electron configuration is Kr 5s2. The fluoride compound of barium would be BaF2, with barium losing its two valence electrons to form a 2+ cation and fluoride gaining one electron to form a 1- anion.
Barium forms an ion with a 2+ charge because it has 2 valence electrons in its outer shell. By losing these 2 electrons, barium achieves a stable electron configuration similar to a noble gas, which is energetically favorable.