Which statement best describes the difference between the first ionization energy and the second ionization energy of an element?

• A. The first ionization energy is always greater than the second ionization energy for any element.
• B. The first ionization energy is the energy required to remove the first electron from a neutral atom, while the second ionization energy is the energy required to remove a second electron from the resulting ion.
• C. The second ionization energy refers to the energy needed to add an electron to a neutral atom.
• D. Both the first and second ionization energies are equal for all elements in the same period.

Answer: (B)

Verified step by step guidance

1. Understand the concept of ionization energy: Ionization energy is the amount of energy required to remove an electron from an atom or ion in the gaseous state.
2. Identify the first ionization energy: This is the energy needed to remove the first electron from a neutral atom, turning it into a positively charged ion (cation).
3. Identify the second ionization energy: This is the energy required to remove a second electron from the already positively charged ion formed after the first electron was removed.
4. Recognize that the second ionization energy is generally higher than the first because removing an electron from a positively charged ion requires more energy due to increased effective nuclear charge attracting the remaining electrons.
5. Compare the given statements by matching these definitions and concepts to determine which statement correctly describes the difference between the first and second ionization energies.