Answer:
The second ionization energy of an atom is always greater than its first ionization energy.
Explanation:
Ionization energies are always negative quantities. FALSE. Ionization energies are always positive because they represent the energy that has to be added to a neutral gaseous atom to remove 1 electron. By convention, energy absorbed goes with the positive sign.
X(g) + 1 I.E. ⇒ X(g)⁺ + 1 e⁻
Oxygen has a larger first ionization energy than fluorine. FALSE. First ionization energy (1 I.E) is the energy required to remove 1 electron from a neutral gaseous atom. First ionization energy for Oxygen is 13.61 eV and for Fluorine is 17.42 eV, that is, more energy is required to remove an electron from F than from O.
The second ionization energy of an atom is always greater than its first ionization energy. TRUE. The energy required to remove 1 electron from a +1 cation (second ionization energy) is always greater than the first ionization energy because of the attraction between the cation and the electron.
X(g)⁺ + 2 I.E. ⇒ X(g)⁺² + 1 e⁻
The third ionization energy is the energy needed to ionize three electrons from a neutral atom. FALSE. The third ionization energy (3 I.E.) is the energy required to remove 1 electron from a +2 cation.
X(g)⁺² + 3 I.E. ⇒ X(g)⁺³ + 1 e⁻
The ionization energy is the energy required to remove electrons from an atom.
One of the important periodic trend is ionization energy. Ionization energy refers to the energy required to remove an electron from an atom and it decreases down the group and increases across the period. The following is true regarding ionization energy;
A neutral atom can have as many values of ionization energy as there are electrons in the atom. The second ionization energy is is always greater than the first ionization energy and so on since more energy is required to remove electrons from a positively charged specie.
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