10. Periodic Properties of the Elements

Why does ionization energy decrease as you move down a group in the periodic table?

Which of the following best explains the deviations from the general trend in first ionization energy across a period?

Which of the following is closest to the first ionization energy of a xenon (Xe) atom?

Which of the following statements correctly describes periodic trends in ionization energy?

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

Which of the following best describes the trend in ionization energy as you move from left to right across a period in the periodic table?

Rank the following elements in order of increasing first ionization energy: Na, Mg, Al.

Which of the following best describes the trend in ionization energy as you move from left to right across a period on the periodic table?

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 ext{ 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?