The electron configuration of sulfur is [Ne]3s23p4.
1s22s22p63s23p4
1s^2 2s^2 2p^6 3s^2 3p^4
1s2 2s2 2p6 3s2 3p4
Sulfide, S2-
The electron configuration of selenium for a 2- ion is [Kr]4s2.3d10.4p6.
The electronic configuration of sulfur ion (S)2- is: 1s22s22p63s23p6.
It has 2 electrons in the first shell, and 8 in the second as it gains an electron to form an ion so the configuration is 2,8.
Electron configuration of radium:Ra: [Rn]7s2Ra(2+): 1s2.2s2.2p6.3s2.3p6.3d10.4s2.4p6.4d1o.4f14.5s2.5p6.5d10.6s2.6p6.
The electron configuration of thaliium III ion is [XE] 4f14 5d10.
Sulfur atoms will gain two electrons in order to achieve a noble gas electron configuration. A sulfide ion has the formula S2-.
Argon
Sulfide, S2-
The abbreviated electron configuration for Pt is [Xe] 6s1 4f14 5d9. also, the configuration for Pt2+ ion is [Xe] 4f14 5d8
The electron configuration of selenium for a 2- ion is [Kr]4s2.3d10.4p6.
The electronic configuration of sulfur ion (S)2- is: 1s22s22p63s23p6.
1s2, 2s2 2p6, 3s2 3p6 The sulfur ion has 16 electrons but sulfide has a charge of negative 2, increasing its electron count by two for a total of 18 electrons, giving it the same electron configuration as Argon (this means it is also isoelectronic with Argon)
sulfur has 16 electrons with a neutral charge the most common ion formed is the sulfide ion, with a negative 2 charge to get a negative 2 charge, it gains 2 electrons, thus fulfilling the octet rule and acquiring the electron configuration of argon
Al3+
Al3+
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.