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The element is sulfur with 16 electrons. It gains two electrons to form sulfide ion which has 18 electrons as that of argon.
sulfur
A species (element, cation or anion) should have eight valence electrons to have a noble gas electronic configuration. However element upto atomic number 4 may have 2 valence electrons and attain the electronic configuration of helium noble gas.
Sulphur is not iso-electronic with any noble gas. However sulphide ion (S2- ion) is iso-electronic with argon with 18 electrons.
Helium is the element in the noble geses family that does not have an octet. Helium is the element in the noble geses family that does not have an octet.
The element is sulfur with 16 electrons. It gains two electrons to form sulfide ion which has 18 electrons as that of argon.
sulfur
Sulfur will gain 2 electrons
Sulfur: The periodic column containing elements with two fewer electrons than the noble gases is column 16, in which oxygen, the lightest element, has a mass number of 16. Sulfur, the next element in this column, has a mass number of 32.
A species (element, cation or anion) should have eight valence electrons to have a noble gas electronic configuration. However element upto atomic number 4 may have 2 valence electrons and attain the electronic configuration of helium noble gas.
[Ne]3s23p4
Sulphur is not iso-electronic with any noble gas. However sulphide ion (S2- ion) is iso-electronic with argon with 18 electrons.
Helium is the element in the noble geses family that does not have an octet. Helium is the element in the noble geses family that does not have an octet.
An element can either gain or lose electrons to achieve a noble gas electron configuration. Such an electron configuration gives an atom of an element a full outer shell, thereby making that element's ion nonreactive. Metals tend to lose electrons, and become cations, whereas nonmetals tend to gain electrons, and become anions. The amount of electrons an element gains of loses is based on the group/family the element is found in on the Periodic Table.
The element is sulfur (S, #16). [Ne] means neon is the nearest noble gas with a lower atomic number. The 3s23p4 means electrons have filled the 3s2 sublevel, and 4 out of 6 possible locations in the 3p sublevel are occupied. Adding the number of electrons to neon (2+4+10) gets you 16, which identifies the element. Sulfur is in period 3, which corresponds to the unfilled level of electrons. The group is 16(6A). Sulfur is considered a p-block element, because its valence electrons partially fill the p sublevel.
Sulfur must to have an electrons octet.
Krypton