Chapter 2: Problem 4

Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the \(1 s\) orbital. Explain the difference without using actual numbers from the text.

Short Answer

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The second ionization energy of helium is significantly higher than its first ionization energy due to the stronger attraction between the remaining electron in the \(1s\) orbital and the nucleus. When the first electron is removed, the electron shielding effect is reduced, and the remaining electron experiences a greater nuclear charge, making it harder to remove. Thus, the second ionization energy requires more energy for the second electron removal compared to the first electron removal.

Step by step solution

Review the concept of ionization energy

Ionization energy is the required energy to remove an electron from an atom or ion. The greater the ionization energy, the more difficult it is to remove an electron from an atom. There are two types of ionization energy: first ionization energy and second ionization energy. The first ionization energy corresponds to the energy required to remove one electron from an atom, while the second ionization energy is the energy required to remove a second electron from the ion.

Consider electron shielding in the 1s orbital

In the 1s orbital, there are two electrons. When the first electron is removed, the remaining electron will experience less electron shielding. This means that the remaining electron will have a stronger interaction with the nucleus, and will be more difficult to remove.

Examine the effect of nuclear charge on ionization energies

Helium has a nuclear charge of +2, which means that there are two protons in its nucleus. When the first electron is removed, the remaining electron experiences a stronger nuclear charge. As a result, the second ionization energy will be higher than the first ionization energy, because the remaining electron will be more strongly attracted to the nucleus and harder to remove.

Discuss the difference in ionization energies without using numbers

The second ionization energy of helium is significantly higher than its first ionization energy because the remaining electron in the 1s orbital experiences a greater nuclear charge and less shielding from other electrons. This stronger attraction to the nucleus leads to a higher energy requirement for the second electron removal compared to the first electron removal.

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Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the \(1 s\) orbital. Explain the difference without using actual numbers from the text.

Short Answer

Step by step solution

Review the concept of ionization energy

Consider electron shielding in the 1s orbital

Examine the effect of nuclear charge on ionization energies

Discuss the difference in ionization energies without using numbers

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