Which of the following orders is wrong? [C.B.S.E. 2002] (a) NH3<PH3<AsH3 - Acidic □(b) Li<Be<B<C

step 1 Question is which of the following order is the wrong way. So in the first option we have acidic

Which of the following orders is wrong? [C.B.S.E. 2002] (a)...

Which of the following orders is wrong? [C.B.S.E. 2002] (a) $\mathrm{NH}_{3}<\mathrm{PH}_{3}<\mathrm{AsH}_{3}$ - Acidic $\square$ (b) $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}-I E_{1}$ (c) $\mathrm{Al}_{2} \mathrm{O}_{3}<\mathrm{MgO}<\mathrm{Na}_{2} \mathrm{O}<\mathrm{K}_{2} \mathrm{O}-$ Basic $\square$ (d) $\mathrm{Li}^{+}<\mathrm{Na}^{+}<\mathrm{K}^{+}<\mathrm{Cs}^{+}-$ Ionic radius $\square$

Which of the following orders is wrong? [C.B.S.E. 2002]
(a) $\mathrm{NH}_{3}<\mathrm{PH}_{3}<\mathrm{AsH}_{3}$ - Acidic
$\square$
(b) $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}-I E_{1}$
(c) $\mathrm{Al}_{2} \mathrm{O}_{3}<\mathrm{MgO}<\mathrm{Na}_{2} \mathrm{O}<\mathrm{K}_{2} \mathrm{O}-$ Basic
$\square$
(d) $\mathrm{Li}^{+}<\mathrm{Na}^{+}<\mathrm{K}^{+}<\mathrm{Cs}^{+}-$ Ionic radius
$\square$

Key Concepts

Ionic Radius

Ionic radius refers to the size of an ion in a crystal lattice or in solution. The ionic radius generally increases down a group as additional electron shells are added, despite the increasing nuclear charge because of the shielding of inner electrons. Trends in ionic radii are essential for understanding ionic bonding, coordination geometry, and crystal structures.

Acid-Base Character of Compounds

The acid-base character of compounds, including hydrides and metal oxides, depends on the nature of the element and its electronegativity. Generally, non-metal hydrides tend to be acidic and metal oxides tend to be basic. These tendencies are influenced by the position of the element in the periodic table and the resulting differences in electron distribution and bond polarity.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It generally increases across a period and decreases down a group due to increasing nuclear charge and electron shielding. However, deviations can occur because of the electron configuration, such as the lower ionization energy of certain elements where a new subshell begins, leading to exceptions in the expected order.

Periodic Trends

Periodic trends are the patterns observed across different elements when arranged in the periodic table. These include trends in ionization energy, atomic and ionic radii, electronegativity, and acid-base behavior. Understanding these trends helps in predicting and rationalizing the chemical and physical properties of elements.

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