Question

ich o. the following reaction requires more energy?
(A) Cs → Cs +e
(B) Cl- - Cl +e
19 F-+F+e
(D) Mg + Mg+ e​

Answer 1

Answer:

D

Explanation:

because mg has required more energy

Answer 2

Answer:c

Explanation:The minimum energy required to remove one electron from a neutral gaseous atom in its ground state to form a gaseous ion is called ionization energy or ionization enthalpy.

X(g)→X+(g)+e−

The energy required for removing one electron is called first ionization potential and smaller ionization enthalpy which is easier to convert an atom into its positive ion.

(A) Cs(g)→Cs+(g)+e−

In this reaction, the amount of energy required removing one electron from a neutral gaseous cesium atom, and the energy is called ionization energy. From the shielding effect by electrons, Cesium exhibits lower ionization energy than other elements in the periodic table.

(B) Cl−(g)→Cl(g)+e−

(C) F−(g)→F(g)+e−

From the above two reactions, the energy required for removing an electron from F− greater than Cl− , because the outermost electron in chlorine is farther from the nucleus than the outermost electron in fluorine. Hence, F− has larger ionization energy means it requires more energy than Cl− .

(D) Mg−(g)→Mg(g)+e−

Mg is an electropositive element which is not possible to form a negative ion.

Hence, the reaction C requires more energy than all the above reactions.