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Answer 1

Answer:

Ionization Enthalpy

Ionization Enthalpy of elements is the amount of energy that an isolated gaseous atom requires to lose an electron in its ground state. Losing of electrons results in the formation of cations.

ionization

The first ionization energy of element A is the energy required by an atom to form A+ ions. The unit of ionization energy is given as KJ mol-1.

A (g) → A+ (g) + e–

In the same way, the second ionization energy is nothing but the energy that you need to remove the second electron from its valence shell. It is explained by the equation given below:

A+ (g) → A2+ (g) + e–

You need to provide a specific amount of energy to remove an electron from an atom. Hence, the ionization enthalpies of chemical elements are always positive. The second most outer electron will be more attracted to the nucleus than the first outer electron. Therefore, the second ionization energy will always be more than the first ionization energy. In the same way, third ionization enthalpy will be greater than the second one.

Factors for Ionization Enthalpies

The Ionization Energy depends on two factors, which are:

The force of attraction between electrons and the nucleus.

The force of repulsion between electrons.

The effective nuclear charge felt by the outermost electrons will be less than the actual nuclear charge. This is because the inner electrons will shield the outermost electrons by hindering the path of nuclear charge. This effect is known as the shielding effect. For example, In Na, the 3s1 electrons will be shielded by its core electrons (1s2, 2s2 and 2p6). Generally, shielding effect is more prominent when the inner orbitals are completely filled.