Concept explainers
Interpretation:
The incorrect statement from the given options needs to be selected.
Concept introduction:
Atomic size decrease on moving from left to right in a period. Electronegativity increases on moving from left to right in a period, the ionic radius of negatively charged ion is more than the atomic radius of the same atom and the ionization energy decreases down the group.

Answer to Problem 2STP
The incorrect statement is A.
Explanation of Solution
In the periodic table, the atomic size decrease from left to right. Sodium and Magnesium both belong to third period but sodium belongs to group I and magnesium belongs to group II, which means, sodium comes first on moving from left to right. So, atomic radius of Sodium is more than atomic radius of magnesium. So, statement A is incorrect.
Carbon (C) and Boron (B) both belong to third period but Carbon belongs to group 14 and boron belongs to group 13. On moving left to right in the periodic table, electro negativity increases. So, carbon is more electronegative than boron. So, option B is correct
The ionic radius of negatively charged ion is greater than the atomic radius of the same element. So, ionic radius of
Ionization energy decreases down the group and increase along a period. Potassium and Rubidium both belongs to Group I but Potassium is in 4th period and Rubidium is in 5th period. So, potassium has greater first ionization enthalpy than Rubidium. So, option D is correct.
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