Aqueous solution of two compounds `M_(1) - O - H and M_(2) - O - H` are prepared in two different beakers . If electronegativity of `M_(1) = 3.4, M_(2) = 1.2, 0 = 3.5 and H = 2.1`, then the nature of two solution will be respectively

Options

A. acidic , acidic
B. acidic basic
C. basic , basic
D. basic acidic

Answer

B

Explanation

As the electronegativity of metal increase the electron density in the O - H bond decreases . In order words O - H bond becomes weak and readily ionizes to liberate `H^(+)` Thus M-O- H behave as an acid.
Conversely as the elecronegativity of the metal decreases M- O bond becomes weak and readily ionizes to liberate `OH^(-)` Thus `M- O- H` behaves as a base. combining both the trends option (b) is correct.