Well, darling, that electron configuration belongs to the halogen group on the Periodic Table. They're a bunch of highly reactive elements just looking to snatch up an electron to achieve a full outer shell. Watch out for these troublemakers!
F = #9, 9 electrons 1s2, 2s2, 2p5 Cl = #17 , 17 electrons 1s2, 2s2, 2p6, 3s2, 3p5 Notice both end in s2, p5. That is why they have similar properties. Both only need 1 electron to complete the octet ( s2 p6 in the outer shell, very stable)
The valence electron configuration for Group 6A elements is ns^2 np^4. This means that Group 6A elements have 6 valence electrons in their outermost shell.
All of the elements in the Alkaline Earth Metals group have the valence shell electron S2. -Hope this helps
Group numbers are used in the periodic table to indicate the number of valence electrons in an element. The generic outer electron configuration for a neutral atom can be determined by looking at the group number: Group 1 elements have 1 valence electron and end in s1, group 2 elements have 2 valence electrons and end in s2, group 13 elements end in s2p1, etc.
All alkaline earth metals have electron configurations ending in s2; 6s2 would be the alkaline earth metal in period 6 of the PTE, which is barium.
Elements in Group 2 of the periodic table will have an electron configuration that ends in s2. This group includes elements such as beryllium, magnesium, and calcium. They have two electrons in their outermost s sublevel.
All noble gases have the electron configuration s2p6.
In the modern periodic table, these elements belong to group 17. These elements have s2 p5 electron configuration. Hence they need one more electron from an electron donor to fulfill its valence shell to obtain noble gas configuration.The elements in the group 7A has 7 electrons in their outermost energy level. They gain 1 electron to get the noble gas configuration. The elements in the group 7A are called halogens.
F = #9, 9 electrons 1s2, 2s2, 2p5 Cl = #17 , 17 electrons 1s2, 2s2, 2p6, 3s2, 3p5 Notice both end in s2, p5. That is why they have similar properties. Both only need 1 electron to complete the octet ( s2 p6 in the outer shell, very stable)
s2,s2 p6.s1
Krypton (Kr) has the same electron configuration as S2, which is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6.
All elements in group 1 have 1 valence electron.
1s22s22p6
The valence electron configuration for Group 6A elements is ns^2 np^4. This means that Group 6A elements have 6 valence electrons in their outermost shell.
Sulfide, S2-
The cation S2- is called sulfide ion. It has a charge of -2 and is formed when sulfur gains two electrons to achieve a stable electron configuration.
phosphorus has 15 protons and electrons: 1 s2 2 s2, 2 p6 3 s2, 3 p3 This adds up to a total of 15 electrons.