Which part of Figure P21.1 best describes the periodic trend...

Name: Problem 1, Chapter 21: Chemistry The Science in Context
Uploaded: 2020-05-21T16:36:33-08:00
Duration: 3 min 30 s
Channel: Katrina Olenwine
Description: Which part of Figure P21.1 best describes the periodic trend in monatomic cation radii moving up or down a group or across a period in the periodic table? (Arrows point in the direction of increasing radii.) (FIGURE CAN'T COPY)

Which part of Figure P21.1 best describes the periodic trend in monatomic cation radii moving up or down a group or across a period in the periodic table? (Arrows point in the direction of increasing radii.) (FIGURE CAN'T COPY)

Key Concepts

Periodic Trends

Periodic trends are systematic variations in the properties of elements, such as atomic and ionic radii, as one moves across a period or down a group in the periodic table. These trends arise from underlying changes in nuclear charge and electron configurations, allowing prediction of how properties change from one element to another.

Atomic and Ionic Radii

Atomic and ionic radii describe the relative sizes of atoms and their ions. For ions, particularly monatomic cations, the removal of electrons typically leads to a contraction of the electron cloud. The trends in these radii as you move across periods or down groups are central to understanding how chemical properties evolve in the periodic table.

Effective Nuclear Charge

Effective nuclear charge is the net attractive force experienced by electrons after accounting for the shielding provided by inner electron shells. As effective nuclear charge increases, electrons are drawn closer to the nucleus, resulting in a smaller atomic or ionic radius. This concept is key to explaining why radii decrease across a period and vary down a group.

Electron Shielding

Electron shielding refers to the phenomenon where inner electrons reduce the full attractive effect of the nucleus on the outer electrons. This reduction in effective nuclear charge makes outer electrons less tightly bound, which contributes to larger ionic radii, especially when comparing elements moving down a group where more electron shells are present.

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