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)
It would be [Ne] 3s2 3p6 which now has the same configuration as Ar, i.e. is isoelectric with argon.
S2-, sulfide ion: 1s2, 2s2 2p6, 3s2 3p6
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6
A sulfide ion is 1s22s22p63s23p6
onions
[Ne]3s23p6
The electron configuration is [Ar]3d2.4s2.
The noble gas krypton has the same electron configuration as an ion of bromine, Br-.
Na+ and neon are isoelectronic.
why is an iron ion attracted to a sulfide ion but not to a zinc ion
Sulfide is divalent ion. it is S2-
it is 2,8,8
2.8 There's a slight confusion if it is 2.8.3. well you see that is the electron arrangement of aluminium ATOM not ion. Hope this helps!
The nuclear charge is the same for both species, but the eight valence electrons in the sulfide ion experience a greater amount of electron-electron repulsion than do the six valence electrons in the neutral sulfur atom. This extra repulsion in the sulfide ion increases the average distance between the valence electrons, so the electron cloud around the sulfide ion has the greater radius.
16 protons and 18 electrons
1s22s22p6
Na+ ion and neon are isoelectronic.
Argon
16 protons and 18 electron
Neon has the same electron configuration as Na+ ion
The electron configuration is [Ar]3d2.4s2.
The noble gas krypton has the same electron configuration as an ion of bromine, Br-.
Argon