Ceseum, 55Cs, has just 1 '6s' electron: 2, 8, 18, 18, 8, 1 electrons in the 1st to 6st shell respectevely.
Cesium is in the 6th row of the periodic table. Therefore Cesium must have one electron in the 6s orbital.
[Xe]6s^2
The condensed electron configuration of polonium is [Xe] 6s^2 4f^14 5d^10 6p^4.
The first ionization potential of Boron is 800 kJ/mol, Barium is 502.9 J/mol The essential difference is that in boron the electron being removed is in a 2p orbital in Barium it is in a 6s orbital. A rationalization is that the 6s electron is on average further away from the core, is better shielded than in B.
Mercury easily shares its valence electrons
Cesium is in the 6th row of the periodic table. Therefore Cesium must have one electron in the 6s orbital.
[Xe]6s^2
[Ar]3d^10 4s^2 4p^3 (the numbers after the "^" should be written like exponents)
the condensed electron configuration for Lu is [Xe] 6s^2 4f^14 5d^1
the condensed electron configuration for Lu is [Xe] 6s^2 4f^14 5d^1
The condensed electron configuration of polonium is [Xe] 6s^2 4f^14 5d^10 6p^4.
The first ionization potential of Boron is 800 kJ/mol, Barium is 502.9 J/mol The essential difference is that in boron the electron being removed is in a 2p orbital in Barium it is in a 6s orbital. A rationalization is that the 6s electron is on average further away from the core, is better shielded than in B.
-40 = 8-6s -40 - 8 = 6s -48 = 6s 8 = s
Mercury easily shares its valence electrons
It may be the Aufbau Principle if you are looking for specifics. or just an electron configuration with 1s, 2s, 2p, 3s, 3p, 3d, etc.
Long-hand version: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^1 Short-hand version: [Xe] 6s^1 Note: The "^" symbol means the the following number is in the form of a superscript.
Both cesium and barium have their outermost electrons in the 6s sublevel, Cs with 1 and Ba with 2, but barium has one more proton in the nucleus than does cesium, and this produces a greater effective nuclear charge and more attraction for the outermost electrons. This in turn pulls the two electrons in the 6s sublevel of barium slightly closer to the nucleus compared to the one 6s electron in cesium.