Potential Energy

Ionization energy (IE) refers to the energy required to remove an electron from an atom or molecule in the gas phase. For group 13 elements, the trend in ionization energies is influenced by the atomic size, effective nuclear charge, and electron shielding. - Boron (B): Boron has the smallest atomic size in group 13 and a relatively high effective nuclear charge due to fewer electron shells compared to elements further down the group. Therefore, boron has the highest ionization energy among the group 13 elements. - Indium (In): Indium is located lower in group 13 compared to Boron, and it has a larger atomic radius and more electron shielding. As a result, it has a lower ionization energy. - Aluminum (Al): Aluminum is in the middle of the group and has ionization energy lower than that of Boron but higher than that of Indium and Thallium. - Thallium (Tl): Thallium is at the bottom of the group, with a very large atomic size and considerable electron shielding. This leads to a much lower ionization energy compared to Boron. Thus, the maximum ionization energy is observed for Boron (B), and the minimum ionization energy is observed for Thallium (Tl). Therefore, the correct answer is (2) B, Tl.

Let's analyze both statements: - Statement 1: Alcohol is prepared from alkyl halide in the presence of aqueous KOH by elimination. This statement is incorrect. When an alkyl halide is treated with aqueous KOH, the reaction follows an or mechanism, leading to the substitution of the halogen by a hydroxyl group, resulting in the formation of an alcohol. This is not an elimination reaction. In fact, elimination occurs when alcoholic KOH is used. - Statement 2: Alkenes are prepared from alkyl halide with alcoholic KOH by -elimination. This statement is correct. When an alkyl halide is treated with alcoholic KOH, a -elimination reaction occurs, resulting in the formation of an alkene. Alcoholic KOH favors the elimination reaction, where a hydrogen atom and a halogen are removed from adjacent carbons to form a double bond. Thus, the correct option is (4) Statement-1 is false and Statement-2 is true.

Ionization energy (IE) refers to the energy required to remove an electron from an atom or molecule in the gas phase. For group 13 elements, the trend in ionization energies is influenced by the atomic size, effective nuclear charge, and electron shielding. - Boron (B): Boron has the smallest atomic size in group 13 and a relatively high effective nuclear charge due to fewer electron shells compared to elements further down the group. Therefore, boron has the highest ionization energy among the group 13 elements. - Indium (In): Indium is located lower in group 13 compared to Boron, and it has a larger atomic radius and more electron shielding. As a result, it has a lower ionization energy. - Aluminum (Al): Aluminum is in the middle of the group and has ionization energy lower than that of Boron but higher than that of Indium and Thallium. - Thallium (Tl): Thallium is at the bottom of the group, with a very large atomic size and considerable electron shielding. This leads to a much lower ionization energy compared to Boron. Thus, the maximum ionization energy is observed for Boron (B), and the minimum ionization energy is observed for Thallium (Tl). Therefore, the correct answer is (2) B, Tl.