---
title: "Electronegativity values for selected elements are shown in the table below.  | Element | Electronegativity | | :— | :— | | \\(\\text{H}\\) | \\(2.1\\) | | \\(\\text{C}\\) | \\(2.5\\) | | \\(\\text{Cl}\\) | \\(3.0\\) | | \\(\\text{F}\\) | \\(4.0\\) |  Which of the following statements best compares the polarity of the \\(\\text{C}-\\text{F}\\) bond to the \\(\\text{C}-\\text{Cl}\\) bond, and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/123489/"
date_modified: "2026-09-28T11:59:55+00:00"
---

# Electronegativity values for selected elements are shown in the table below.

| Element | Electronegativity |
| :— | :— |
| \(\text{H}\) | \(2.1\) |
| \(\text{C}\) | \(2.5\) |
| \(\text{Cl}\) | \(3.0\) |
| \(\text{F}\) | \(4.0\) |

Which of the following statements best compares the polarity of the \(\text{C}-\text{F}\) bond to the \(\text{C}-\text{Cl}\) bond, and provides the correct justification?

Electronegativity values for selected elements are shown in the table below.

| Element | Electronegativity |
| :--- | :--- |
| \(\text{H}\) | \(2.1\) |
| \(\text{C}\) | \(2.5\) |
| \(\text{Cl}\) | \(3.0\) |
| \(\text{F}\) | \(4.0\) |

Which of the following statements best compares the polarity of the \(\text{C}-\text{F}\) bond to the \(\text{C}-\text{Cl}\) bond, and provides the correct justification?

- **A.** The \(\text{C}-\text{F}\) bond is more polar than the \(\text{C}-\text{Cl}\) bond because the higher ionization energy of fluorine results in the complete transfer of a valence electron from carbon to fluorine.
- **B.** The \(\text{C}-\text{F}\) bond is more polar than the \(\text{C}-\text{Cl}\) bond because the larger difference in electronegativity causes the shared electron density to be shifted more toward the \(\text{F}\) atom.
- **C.** The \(\text{C}-\text{Cl}\) bond is more polar than the \(\text{C}-\text{F}\) bond because the chlorine atom has a larger electron cloud that is more polarizable than that of the fluorine atom.
- **D.** The \(\text{C}-\text{Cl}\) bond is more polar than the \(\text{C}-\text{F}\) bond because chlorine has a larger atomic radius, resulting in a longer bond that increases the separation of full ionic charges.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123489/*