Multiple Choice
Which of the following best explains why smaller atoms generally have higher ionization energies?
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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?35views
- Multiple ChoiceWhich of the following atoms in the ground state requires the least amount of energy to remove its valence electron?41views
- Multiple ChoiceWhich of the following elements has the lowest first ionization energy?33views
- 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?41views
- Multiple ChoiceWhy does fluorine have a higher ionization energy than iodine?76views
- Multiple ChoiceWhy does ionization energy decrease as you move down a group in the periodic table?42views
- Multiple ChoiceWhich of the following best explains the deviations from the general trend in first ionization energy across a period?48views
- Multiple ChoiceWhich of the following is closest to the first ionization energy of a xenon (Xe) atom?43views
- Multiple ChoiceWhich of the following statements correctly describes periodic trends in ionization energy?41views
- Multiple ChoiceWhich of the following atoms has the largest first ionization energy?36views
- 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?49views
- Multiple ChoiceRank the following elements in order of increasing first ionization energy: Na, Mg, Al.48views
- 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?34views
- Multiple ChoiceWhich ionization energy requires the most energy to remove an electron from an atom?39views