10. Periodic Properties of the Elements

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)?

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

Which of the following best describes how the first ionization energy changes within a group and across a period in the periodic table?

Why does ionization energy tend to decrease from top to bottom within a group on the periodic table?

Why does ionization energy generally increase as you move from left to right across a period in the periodic table?

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

Which pairs of elements within a period are exceptions to the general increase in first ionization energy across the period?

Which group in the periodic table is characterized by high ionization energies but very weak electron affinities?

Which of the following elements will have a lower ionization energy than scandium (Sc)?

Why does ionization energy decrease as you go down a group on the periodic table?