In: Chemistry
a) Atomic radius of Ca is larger than the atomic radius of Mg because as we move down the group, number of shells increases, screening effect increases and thus, the distance between nucleus and outer electron increases.
Screening effect is the screening of outer electrons by inner electrons due to which outer electrons are less attracted. The number of protons and hence positive charges also increases but the effect of first two is more than the latter. Hence size increases.
b)Atomic size Of K is larger than the atomic radius of Ca.In this, number of electrons are added to the same shell from K to Ca. But number of protons are increasing. Thus, the attraction between outer electrons and nucleus increases and hence size increases.
c) atomic number of S = 16 = number of protons = number of electrons
In S2-, number of electrons = 18 but number of protons = 16
In Cl-, number of protons = 17 and number of electrons = 18
Thus, in both S2- and Cl- ,number of electrons are same = 18
but number of protons in Cl- are more than the number of protons in S2-
Thus, attraction is more in case of Cl- than in S2-
Hence size of Cl- is less than the size of S2-
or size of S2- is less than the size of Cl-
d) Zr3+, number of protons = 40, number of electrons = 37
In Zr4+, number of protons = 40,number of electrons = 36
Thus, number of elctrons in case of Zr4+ is less than the number of electrons in Zr3+
So, attraction in case of Zr4+ is more than in Zr3+
Hence, ionic radius of Zr3+ is larger than the ionic radius of Zr4+