Textbook Question
(b) Would you expect it to require more or less energy to remove a 3s electron from the chlorine atom, as compared with a 2p electron?
10. Periodic Properties of the Elements
Periodic Trend: Effective Nuclear Charge
Multiple Choice
Which group on the periodic table has the highest effective nuclear charge experienced by its valence electrons?
A
Noble gases (Group 18)
B
Alkali metals (Group 1)
C
Alkaline earth metals (Group 2)
D
Halogens (Group 17)
Verified step by step guidance1
Understand the concept of effective nuclear charge (Z_eff), which is the net positive charge experienced by valence electrons after accounting for the shielding effect of inner electrons.
Recall that effective nuclear charge increases across a period (left to right) on the periodic table because the number of protons increases while shielding remains relatively constant.
Recognize that within a group (top to bottom), effective nuclear charge experienced by valence electrons generally decreases due to increased shielding from additional inner electron shells.
Identify the groups in question: Alkali metals (Group 1), Alkaline earth metals (Group 2), Halogens (Group 17), and Noble gases (Group 18), all located in the same period or across periods.
Conclude that noble gases (Group 18) have the highest effective nuclear charge among these groups because they are at the far right of the periodic table in their respective periods, with the greatest number of protons and minimal additional shielding for their valence electrons.
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