JEE MainChemistryClassification of Elements and Periodicity in Properties
Elements X, Y, and Z belong to the third period of the periodic table and have atomic numbers 11 , 14 , and 17 , respectively. Which of the following correctly describes the relative chemical reactivity of these elements and the acid-base nature of the oxides formed by X and Z?
Options
- AThe chemical reactivity is highest for X and Z and lowest for Y; the oxide of X is basic while that of Z is ac
- BThe chemical reactivity steadily increases from X to Z; the oxide of X is basic while that of Z is acidic.
- CThe chemical reactivity steadily decreases from X to Z; the oxide of X is acidic while that of Z is basic.
- DThe chemical reactivity is highest for X and Z and lowest for Y; the oxide of X is acidic while that of Z is b
Correct answer
A. The chemical reactivity is highest for X and Z and lowest for Y; the oxide of X is basic while that of Z is ac
Step-by-step solution
The elements with atomic numbers 11 , 14 , and 17 in the third period are Sodium (Na), Silicon (Si), and Chlorine (Cl), respectively. Across a period, chemical reactivity is highest at the two extremes (excluding noble gases) and lowest in the centre. Thus, X (Group 1) and Z (Group 17) are highly reactive, while Y (Group 14) is less reactive. The nature of oxides changes from strongly basic on the left to strongly acidic on the right. Therefore, the oxide of X (Na) is basic, and the oxide of Z (Cl) is acidic. Answe