객관식
Why is it easier to remove an electron from a sodium (Na) atom than from a magnesium (Mg) atom?
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10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
객관식
Which of the following elements requires the most energy to lose one electron (i.e., has the highest first ionization energy)?
A
Neon (Ne)
B
Aluminum (Al)
C
Sodium (Na)
D
Potassium (K)
검증된 단계별 안내1
Understand that the first ionization energy is the energy required to remove one electron from a neutral atom in the gaseous state.
Recall the general trend of ionization energy in the periodic table: it increases across a period (left to right) and decreases down a group (top to bottom).
Identify the positions of the given elements in the periodic table: Potassium (K), Sodium (Na), Aluminum (Al), and Neon (Ne). Potassium and Sodium are in Group 1, Aluminum is in Group 13, and Neon is a noble gas in Group 18.
Apply the trend: since Neon is at the far right of its period and is a noble gas with a full valence shell, it has a much higher ionization energy compared to the metals listed, which are more willing to lose electrons.
Conclude that Neon requires the most energy to remove one electron because it has a stable electron configuration and is located at the top right of the periodic table among the given options.
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