Multiple Choice
Which of the following lists the elements Mg, Na, P, Si, and Ar in order of increasing atomic radius?
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10. Periodic Properties of the Elements
Periodic Trend: Atomic Radius
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Which group in the periodic table contains elements with the smallest atomic radius?
A
Group 1 (Alkali metals)
B
Group 17 (Halogens)
C
Group 2 (Alkaline earth metals)
D
Group 18 (Noble gases)
Verified step by step guidance1
Understand that atomic radius generally decreases from left to right across a period in the periodic table due to increasing nuclear charge pulling electrons closer to the nucleus.
Recognize that atomic radius generally increases down a group because additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.
Identify the groups mentioned: Group 1 (Alkali metals) are on the far left, Group 2 (Alkaline earth metals) are next to Group 1, Group 17 (Halogens) are near the right side, and Group 18 (Noble gases) are at the far right of the periodic table.
Apply the trend that elements in Group 18 have the highest effective nuclear charge in their period without gaining additional electron shells, resulting in the smallest atomic radius within that period.
Conclude that among the given options, Group 18 (Noble gases) contains elements with the smallest atomic radius because they are located at the far right of the periodic table and have a full outer shell, leading to a strong attraction between the nucleus and electrons.
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