1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6
Iodine has the atomic number of 53. Its common ionic form has it gaining one electron which gives the orbital configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6.
electron configuration of iodine is
1s22s22p63s23p64s2 3d104p65s24d105p5
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
The electron configuration of iodine is [Kr]4d105s25p6.
[Kr] 4d10 5s2 5p5
or
2, 8, 18, 18, 7
[Kr] 5s^2 4d^10 5p^5
1s22s22p63s23p64s23d104p65s24d105p5
Barium loses electrons to obtain a stable octet, like any other metal.
Iodine's electron configuration is 2, 8, 18, 18, 7; bromine's is 2, 8, 18, 7. At the simplest level of modelling there is one more electron shell occupying space in an iodine atom than in one of bromine.
iodine has 7 electrons in the valence shell. and needs one more electron to attain stable noble gas configuration. So it gains one electron and forms iodide ion with charge of -1.
Fluorine, chlorine bromine and iodine have seven electrons in their valence shells, and they all need one electron to have stabilized electron configuration. Therefore they are grouped in Group 17 (halogen group) of periodic table.
The electron configuration of sulfur (long) is: 1s22s22p63s23p4. The electron configuration of sulfur (short) is: [He]3s23p4.
Iodine is the element with that configuration.
[Kr]
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
1s22s22p63s23p64s2 3d104p65s24d105p5
No, iodine has 5 electron shells. It has a total of 53 electrons and its electron configuration is [Kr] 5s2 4d10 5p5, indicating that it has 4 electron shells.
Iodine gains 1 electron to fill it's shell.
Chlorine has 17 electrons, therefore its electronic configuration is: 2, 8, 7
5
I: [kr] 5s^2 4d^10 5p^5
Iodine will gain one electron to form iodide anion which has the electronic configuration of the nearest noble gas (xenon): [Kr] 5s2 4d10 5p6 or 2, 8, 18, 18, 8.
Barium loses electrons to obtain a stable octet, like any other metal.
I- ion (iodine ion and not iodine) and xenon will have the same number of electrons (54 electrons)