10. Periodic Properties of the Elements

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

Which of the following elements has the largest ionization energy?

Which of the following atoms has the highest ionization energy?

Which of the following is closest to the first ionization energy of a rubidium (Rb) atom?

Which element has the lowest first ionization energy?

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

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

Which of the following best explains why ionization energy decreases as you move down a group in the periodic table?

Which observation about ionization energies provides evidence for the quantization of electron energies in atoms?

Among the elements of the main group, the first ionization energy increases in which direction on the periodic table?

What happens to the ionization energy of elements as you move from left to right across a period in the periodic table?

Which reaction below represents the first ionization of o?

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

Which of the following best explains the general trends and exceptions observed in ionization energy across the periodic table?