My textbook was talking about valence electrons and discussing how they are the outermost electrons, etcI understand that partBut then the textbook states: quot;For C,N,O, and F of the periodic table, the valence electrons belong to the second shellWith eight electrons, this shell is completely filledFor Si, P, S and Cl in period 3 of the Periodic table, the valence electrons belong to the 3rd shellThis shell is only partially filled with 8 electrons; the 3s and 3p orbitals are completeyl filled, but the 5 3d orbitals can take an additional 10 electrons.quot;I understand that there is still room in the 3rd shell to accomodate for 10 more electrons, I get that partBut I was just confused as to why they excluded the elements Na, Mg, and Al from the 3rd periodDon't those belong to the 3rd shell as well?Thanks for your help! Just confused on the wording more than the concept I guess.
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yes, the elements Na, Mg, and Al have their valence electrons in the 3rd period as wellyour author, at this point is focusing attention upon those elements which take additional electrons into their outside shell, filling that outside shell up to 8 electrons, in so doing forming negative ions sulfur with 6 valence electrons, takes 2 more e-, forms sulfide S^-2 chlorine with 7 valence electrons, takes 1 more e-, forms chloride Cl^-1 on the other hand, the elements Na, Mg, and Al are elements which usually lose valence electrons, in so doing become positive ions sodium with 1 valence electron, loses that 1 e-, forms Na^+1 Magnesium with 2 valence electrons, loses those 2 e-, forms Mg^+2 Aluminum with 3 valence electrons, loses those 3 e-, forms Al^+3
