Textbook Question
Choose the element with the higher first ionization energy from each pair. d. P or Sn
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Ch.8 - Periodic Properties of the Elements
Chapter 8, Problem 76
Arrange these elements in order of decreasing first ionization energy: Cl, S, Sn, Pb.
Verified step by step guidance1
Understand that first ionization energy is the energy required to remove the outermost electron from a neutral atom in the gaseous state.
Recall that ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.
Identify the positions of the given elements in the periodic table: Cl (Chlorine) and S (Sulfur) are in the same period, while Sn (Tin) and Pb (Lead) are in the same group.
Compare Cl and S: Since Cl is to the right of S in the same period, Cl has a higher first ionization energy than S.
Compare Sn and Pb: Since Sn is above Pb in the same group, Sn has a higher first ionization energy than Pb.
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