By the trend it is Na...(Bigger the farther left and bigger towords the bottom)
Mg has a larger atomic radius than Na. This is because atomic radius generally increases as you move down a group in the Periodic Table, and Mg is below Na in the same group. Additionally, Mg has more energy levels and electrons compared to Na, contributing to its larger atomic radius.
bromine - atomic radius = 115 pm
calcium - atomic radius = 180 pm
so calcium is larger
Sodium has a larger atomic radius than aluminum.
chlorine. across a period the size decreases
Mg2+ has the smaller ionic radius compared to Ca2+ because as you move down a group in the periodic table, the ionic radius increases due to the addition of electron shells. Mg and Ca are in the same group, but Ca has more electron shells than Mg, resulting in a larger ionic radius for Ca2+.
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.
Sodium (Na) is the largest element among Mg (magnesium), S (sulfur), Na (sodium), and Cl (chlorine) when comparing their atomic radii. Sodium has the largest atomic radius because it is located in the third period of the periodic table, whereas magnesium is smaller due to being in the second period.
There are many elements with atomic radii larger than that of P. Several examples would be Si, Al, Mg, and Na.
Na+ is smaller than Na.
Sodium has a larger atomic radius than aluminum.
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.
Postassium, K, has a larger radius than sodium, Na, because it is in the next period on the table but in the same group as sodium.
Ca, Mg, Be, Fr, Cs, Rb, K, Na, Li, H
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.
Mg2+ has the smaller ionic radius compared to Ca2+ because as you move down a group in the periodic table, the ionic radius increases due to the addition of electron shells. Mg and Ca are in the same group, but Ca has more electron shells than Mg, resulting in a larger ionic radius for Ca2+.
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.
The larger radius is from 'In'.
Sodium (Na) is the largest element among Mg (magnesium), S (sulfur), Na (sodium), and Cl (chlorine) when comparing their atomic radii. Sodium has the largest atomic radius because it is located in the third period of the periodic table, whereas magnesium is smaller due to being in the second period.