Which of the following statements correctly describes a trend in the periodic table related to the atomic number, atomic radius, and noble gases?

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Atomic radius increases down a group, while noble gases have the largest atomic radius in their period.

Atomic radius decreases across a period, and noble gases have the smallest atomic radius compared to other elements in their period.

Atomic radius increases across a period, and noble gases have the largest atomic radius in the group.

Noble gases always have a larger atomic radius than the alkali metals in the same period.

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Answer

When you travel across a period from left to right, the atomic number rises, the atomic radius shrinks, and the noble gases sit at the far right end of each period. This happens because each new element adds one more proton and electron to the same shell, pulling the electrons closer to the nucleus. The smaller radius means the outer electrons feel a stronger pull, so the element is less reactive. For example, sodium (atomic number 11) has a larger radius than argon (atomic number 18), the noble gas that caps period 3. Thus the trend is: higher atomic number → smaller radius, with noble gases marking the end.

Detailed Explanation

Across a period, atomic radius decreases because more protons pull electrons closer. Other options are incorrect because The radius does increase down a group, but noble gases are not the largest; The radius does not increase across a period; it shrinks.

Key Concepts

atomic number

atomic radius

noble gases

Topic

Periodic Table Structure

Difficulty

hard level question

Cognitive Level

understand

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