Identify each statement as true or false.
a. Ionization energies are always negative quantities.
b. Oxygen has a larger first ionization energy than fluorine.
c. The second ionization energy of an atom is always greater than its first ionization energy.
d. The third ionization energy is the energy needed to ionize three electrons from a neutral atom.

검증된 단계별 안내

Ionization energy is the energy required to remove an electron from an atom or ion. It is always a positive quantity because energy must be supplied to overcome the attraction between the electron and the nucleus. Therefore, statement a is false.

The first ionization energy generally increases across a period from left to right due to increasing nuclear charge. Since fluorine is to the right of oxygen in the periodic table, fluorine has a larger first ionization energy than oxygen. Therefore, statement b is false.

The second ionization energy is the energy required to remove a second electron after the first has been removed. It is always greater than the first ionization energy because the electron is being removed from a positively charged ion, which has a stronger attraction to the remaining electrons. Therefore, statement c is true.

The third ionization energy refers to the energy required to remove a third electron after the first two have been removed, not the energy needed to remove three electrons simultaneously. Therefore, statement d is false.

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Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is always a positive value because energy must be supplied to overcome the attraction between the negatively charged electron and the positively charged nucleus. Therefore, the statement that ionization energies are always negative is false.

Trends in Ionization Energy

Ionization energy generally increases across a period in the periodic table due to increasing nuclear charge, which holds electrons more tightly. Conversely, it decreases down a group as additional electron shells are added, increasing distance from the nucleus. Thus, the statement regarding oxygen having a larger first ionization energy than fluorine is false, as fluorine has a higher ionization energy.

Successive Ionization Energies

Successive ionization energies refer to the energy required to remove additional electrons from an atom after the first has been removed. Typically, each successive ionization energy is greater than the previous one due to increased positive charge in the nucleus and reduced electron-electron repulsion. Therefore, the statement that the second ionization energy is always greater than the first is true, while the statement about the third ionization energy is misleading, as it refers to the energy needed to remove three electrons, not just the third ionization energy itself.