---
title: "The atomic numbers and experimental atomic radii of selected Period 2 elements are provided in the table below.  | Element | Atomic number (\\(Z\\)) | Valence shell | Atomic radius (\\(\\text{pm}\\)) | | :— | :— | :— | :— | | \\(\\text{Li}\\) | \\(3\\) | \\(n = 2\\) | \\(152\\) | | \\(\\text{N}\\) | \\(7\\) | \\(n = 2\\) | \\(75\\) | | \\(\\text{F}\\) | \\(9\\) | \\(n = 2\\) | \\(71\\) |  Which of the following statements best explains why an atom of \\(\\text{F}\\) has a smaller atomic radius than an atom of \\(\\text{Li}\\)?"
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url: "https://nerd-notes.com/ubq/119982/"
date_modified: "2026-08-21T08:31:29+00:00"
---

# The atomic numbers and experimental atomic radii of selected Period 2 elements are provided in the table below.

| Element | Atomic number (\(Z\)) | Valence shell | Atomic radius (\(\text{pm}\)) |
| :— | :— | :— | :— |
| \(\text{Li}\) | \(3\) | \(n = 2\) | \(152\) |
| \(\text{N}\) | \(7\) | \(n = 2\) | \(75\) |
| \(\text{F}\) | \(9\) | \(n = 2\) | \(71\) |

Which of the following statements best explains why an atom of \(\text{F}\) has a smaller atomic radius than an atom of \(\text{Li}\)?

The atomic numbers and experimental atomic radii of selected Period 2 elements are provided in the table below.

| Element | Atomic number (\(Z\)) | Valence shell | Atomic radius (\(\text{pm}\)) |
| :--- | :--- | :--- | :--- |
| \(\text{Li}\) | \(3\) | \(n = 2\) | \(152\) |
| \(\text{N}\) | \(7\) | \(n = 2\) | \(75\) |
| \(\text{F}\) | \(9\) | \(n = 2\) | \(71\) |

Which of the following statements best explains why an atom of \(\text{F}\) has a smaller atomic radius than an atom of \(\text{Li}\)?

- **A.** \(\text{F}\) has a smaller atomic radius because additional valence electrons increase electron-electron repulsions, which compresses the electron cloud inward toward the nucleus.
- **B.** \(\text{F}\) has a smaller atomic radius because \(\text{F}\) has a higher electronegativity, which causes the atom to attract its own electrons with greater covalent character.
- **C.** \(\text{F}\) has a smaller atomic radius because \(\text{F}\) has a greater nuclear charge while having the same number of core shielding electrons, resulting in a larger effective nuclear charge that draws the valence shell closer.
- **D.** \(\text{F}\) has a smaller atomic radius because \(\text{F}\) has more occupied subshells, which allows inner core electrons to exert a greater attractive pull on the outermost electrons.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119982/*