Multiple Choice
Which ionization energy requires the most energy to remove an electron from an atom?
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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 many distinct ionization energy values are required to remove all electrons from a neutral aluminum (Al) atom?
- Multiple ChoiceWhich of the following elements has the greatest first ionization energy?
- Multiple ChoiceWhen ionization energy is supplied to an atom, which of the following can be removed from the atom?
- Multiple ChoiceWhich of the following is the correct value for the first ionization energy of doubly ionized lithium (Li^{2+}), where Z = 3? Use the formula E = -13.6 ext{ eV} imes Z^2 / n^2 for hydrogen-like ions, and recall that the first ionization energy is the energy required to remove the only electron from the n = 1 state.
- Multiple ChoiceWhich of the following atoms has the highest ionization energy?
- Multiple ChoiceWhich of the following elements has the highest ionization energy?
- Multiple ChoiceWhich element has the lowest first ionization energy?
- Multiple ChoiceWhich of the following best explains the decrease in first ionization energy when moving from nitrogen (N) to oxygen (O) across the periodic table?
- Multiple ChoiceWhich of the following best describes the periodic trend for ionization energy across the periodic table?
- Multiple ChoiceWhich of the following best describes the overall trend in ionization energy across the periodic table?
- Open Question
What trend in ionization energy do you see as you move down a group?
1views - Multiple ChoiceWhich of the following elements has the largest first ionization energy?
- Multiple ChoiceAs you move down a group in the periodic table, what happens to the ionization energy of the elements?
- Multiple ChoiceWhich of the following elements requires the most energy to lose one electron (i.e., has the highest first ionization energy)?