1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 OR [Xe] 6s2 4f14 5d10
electron configuration: 2, 8, 18, 32, 18, 2
Mercury has the atomic number of 80 with the orbital configuration of [Xe] 4f14 5d10 6s2. With a net charge of 2+, there are two fewer electrons, leaving the configuration of [Xe] 4f14 5d10.
The electron configuration for oxygen is [He]2s2.2p4.The electron configuration for sulfur is [Ne]3s2.3p4.
The electronic configuration of einsteinium is: [Rn]5f11.7s2.
Mercury has no unpaired electrons. It has a fully filled 5d10 shell and its electron configuration is [Xe] 4f14 5d10 6s2.
none ? because if they did ...they would BE mercury ?...
The electron configuration for sulfur is [Ne]3s2.3p4.The electron configuration for mercury is [Xe]4f14.5d10.6s2.
electron configuration: 2, 8, 18, 32, 18, 2
The element mercury (Hg, atomic number 80) has the electron configuration [Xe] 4f14 5d10 6s2
The ground state electron configuration of mercury (Hg), which has an atomic number of 80, is [Xe] 4f² 5d⁹ 6s². This configuration indicates that mercury has a filled xenon core, followed by two electrons in the 6s subshell, nine in the 5d subshell, and two in the 4f subshell.
The noble gas configuration of mercury is [Xe] 4f^14 5d^10 6s^2. Mercury is in the same period as xenon (Xe) on the periodic table, so it can achieve stability by adopting the electron configuration of xenon.
Mercury has the atomic number of 80 with the orbital configuration of [Xe] 4f14 5d10 6s2. With a net charge of 2+, there are two fewer electrons, leaving the configuration of [Xe] 4f14 5d10.
The electronic configuration of mercury is [Xe] 4f14 5d10 6s2 This may help answer the qustion, which is difficult to understand
The electron configuration for oxygen is [He]2s2.2p4.The electron configuration for sulfur is [Ne]3s2.3p4.
The electron configuration for beryllium, Be, is 1s22s2.
A cation has a depleted electron configuration.
The electronic configuration of einsteinium is: [Rn]5f11.7s2.