객관식
What is the general trend in first ionization energy as we move down a column (group) in the periodic table?
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10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
객관식
Which of the following atoms has the highest first ionization energy, making it the most difficult to remove an electron?
A
Ne (Neon)
B
K (Potassium)
C
Na (Sodium)
D
Li (Lithium)
검증된 단계별 안내1
Understand that the first ionization energy is the energy required to remove the outermost electron from a neutral atom in the gas phase.
Recall that ionization energy generally increases across a period (left to right) in the periodic table because the nuclear charge increases, pulling electrons closer and making them harder to remove.
Recall that ionization energy generally decreases down a group (top to bottom) because electrons are farther from the nucleus and are shielded by inner electrons, making them easier to remove.
Identify the positions of the given elements: Li, Na, and K are all in Group 1 (alkali metals) and increase in atomic number down the group, while Ne is a noble gas at the end of the same period as Li.
Conclude that Neon (Ne), being a noble gas with a full valence shell and located at the far right of the period, has the highest first ionization energy among the options, making it the most difficult to remove an electron.
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