Multiple Choice
Which of the following best explains why smaller atoms generally have higher ionization energies?
79
views
10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
Back10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
- Multiple ChoiceHow does the first ionization energy change as you move down a group and across a period in the periodic table?66views
- Multiple ChoiceWhich of the following atoms in the ground state requires the least amount of energy to remove its valence electron?72views
- Multiple ChoiceWhich of the following elements has the lowest first ionization energy?64views
- Multiple ChoiceWhich of the following best describes the trend in ionization energy as you move down a group and across a period in the periodic table?69views
- Multiple ChoiceWhy does fluorine have a higher ionization energy than iodine?132views
- Multiple ChoiceWhy does ionization energy decrease as you move down a group in the periodic table?83views
- Multiple ChoiceWhich of the following best explains the deviations from the general trend in first ionization energy across a period?76views
- Multiple ChoiceWhich of the following is closest to the first ionization energy of a xenon (Xe) atom?73views
- Multiple ChoiceWhich of the following statements correctly describes periodic trends in ionization energy?67views
- Multiple ChoiceWhich of the following atoms has the largest first ionization energy?69views
- Multiple ChoiceWhich of the following best describes the trend in ionization energy as you move from left to right across a period in the periodic table?75views
- Multiple ChoiceRank the following elements in order of increasing first ionization energy: Na, Mg, Al.76views
- Multiple ChoiceWhich of the following best describes the trend in ionization energy as you move from left to right across a period on the periodic table?59views
- Multiple ChoiceWhich ionization energy requires the most energy to remove an electron from an atom?71views