Question

Arrange in the order of increasing basicity (NO2, K20, ZnO):
A) $N{O_2} < ZnO < {K_2}0$
B)${K_2}0 < ZnO < N{O_2}$
C)$N{O_2} < {K_2}0 < ZnO$
D)${K_2}0 < N{O_2} < ZnO$

Answer 1

To answer this question the periodic properties of the elements from the different groups should be known. The periodic properties have opposite trends between left to right and top to bottom. The elements of a definite row contain the same number of orbits. The elements of the same column have the same chemical behaviors.

Complete step by step answer:
In the periodic table, all the elements are arranged by the atomic numbers. Generally, on the left side of the periodic table, elements are metallic in nature. Moving from left to right the metallic character decreases and the non-metallic character increases. At the extreme left elements are non-metallic in nature
In general, the electropositive character of the oxide’s central atom will determine whether the oxide will be acidic or basic. The more electropositive the central atom, the more basic the oxide. The more electronegative the central atom, the more acidic the oxide.
Now in the given oxides, nitrogen is at the right side of the periodic table so it is non-metal and forms acidic oxides. Therefore, the basicity of this oxide will be the least. Transition metal like zinc is in the middle so it will form less basic oxide but potassium is at the extreme left side so it will form the most basic oxide.
Therefore, considering the position of the element in the periodic table and the metallic character the basicity order of the oxide is,
$N{O_2} < ZnO < {K_2}0$
So, the correct option is A.

Note: As we move from left to right in the periodic table, the atomic size of the atom goes on decreasing. This is because more and more electrons are added to the same valence shell. This causes a greater nuclear charge attracting more and more electrons. This increases the net nuclear force of attraction as we move from left to right in the period.