Want this question answered?
By the trend it is Na...(Bigger the farther left and bigger towords the bottom)
chlorine. across a period the size decreases
Mg. Mg has 2 valence electrons while Na only has 1 valence electron. Mg+2 also has a smaller ionic radius than Na+. Metallic bonds are stronger when metals have more valence electrons and smaller ion size. The metallic bond will be stronger for Mg. Thus, Mg will have the higher melting point.
Ca, Mg, Be, Fr, Cs, Rb, K, Na, Li, H
Na+ is smaller than Na.
Both Mg and Na have the same outer energy level (shell). Mg has one proton more than NA and one electron more. The charge on th eouter shell the effective nuclear charge is reduced by the inner core electrons, which are the ame in both cases So the pull experienced by the valence electrons towards the nucleus is more in the case of Mg than Na. Hence Mg has slightly smaller size (radius) than Na.
a) Sc,Ti,V,Crb) Na,K,Rb,Csc) B,Si,As,Ted) F,Cl,Br,Ie) Na,Mg,Al,SiThe correct answer of these options is a) Sc,Ti,V,Cr because they are the closest elements to each other in the periodic table.
Na has a higher atomic radius then Na+, since it still has it's outer electron (3s).
There are many elements with atomic radii larger than that of P. Several examples would be Si, Al, Mg, and Na.
NA
Potassium has the largest atomic radius.
The neutral atom of potassium has the largest radius.