10. Periodic Properties of the Elements

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

Which of the following best explains why smaller atoms generally have higher ionization energies?

How does the first ionization energy change as you move down a group and across a period in the periodic table?

Which of the following atoms in the ground state requires the least amount of energy to remove its valence electron?

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

Which of the following best describes the trend in ionization energy as you move down a group and across a period in the periodic table?

Why does fluorine have a higher ionization energy than iodine?

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?