10. Periodic Properties of the Elements

Which ionization energy requires the most energy to remove an electron from an atom?

How many distinct ionization energy values are required to remove all electrons from a neutral aluminum (Al) atom?

Which of the following elements has the greatest first ionization energy?

When ionization energy is supplied to an atom, which of the following can be removed from the atom?

Which of the following is the correct value for the first ionization energy of doubly ionized lithium (Li^{2+}), where Z = 3? Use the formula E = -13.6 \(\text{ eV}\) imes Z^2 / n^2 for hydrogen-like ions, and recall that the first ionization energy is the energy required to remove the only electron from the n = 1 state.

Which of the following atoms has the highest ionization energy?

Which of the following elements has the highest ionization energy?

Which element has the lowest first ionization energy?

Which of the following best explains the decrease in first ionization energy when moving from nitrogen (N) to oxygen (O) across the periodic table?

Which of the following best describes the periodic trend for ionization energy across the periodic table?

Which of the following best describes the overall trend in ionization energy across the periodic table?

Which of the following elements has the largest first ionization energy?

As you move down a group in the periodic table, what happens to the ionization energy of the elements?

Which of the following elements requires the most energy to lose one electron (i.e., has the highest first ionization energy)?