Question

The rule for the ms quantum number is that it can only be + ½ and – ½. In other words, electrons can only have two possible spins. The shape of the periodic table and the resulting chemical bonding depend on the electron configurations predicted by these quantum numbers. Imagine what the periodic would look like if ms could have three values, + ½ and – ½ and 0. In other words, electrons can now have three spins. What would the periodic table look like? What would be the new noble gas? What sort of ionic compounds would form? What sort of covalent molecules would form?

Answer 1

It we have m, values +Y2;0,8-Y2, then each orbital containing 3-electrons. Nonnally total no of electrons in shell is an2 , but, it we have 3 possible values then it will be [302]. ie K, L, M, N Sbeul woteising 3, 12, 22) 48 elelemss- respectively. For 4th period we have 48,3 d, 4P 150-electrons. will be like of total (1x2)+(6x3) + (3x3) ie a7 eledross- will be there. Adding of each electrons make new elemeet. Hence oth period will have 27 elements, First period having is configuration, bence it should- containing 3-elements instead of having zelenests. So, the first noble gas having atomic number 3 and haling en eleethods Celest syl zor electronic configuration will- be is3 and second noble gas cestigaration will be - 183 2 $ 2p9 C4 electoras). Stability of second period will tell about basis 12 electrons filled on not instead of helling like octel Rale in so carb maninum cevolency will be 6. The moleule having less than Gelectros can lose electrons and show ionic compound. The molecule can make avalest bord having 6 bond manunum fon seed period .