---
title: "The complete Lewis diagrams for ethene, \\(\\text{C}_2\\text{H}_4\\), and ethyne, \\(\\text{C}_2\\text{H}_2\\), are shown below.  Which of the following correctly identifies the hybridization of each carbon atom in ethyne and the total number of \\(\\sigma\\) and \\(\\pi\\) bonds in one molecule of ethyne?"
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url: "https://nerd-notes.com/ubq/119770/"
date_modified: "2026-08-21T08:12:17+00:00"
---

# The complete Lewis diagrams for ethene, \(\text{C}_2\text{H}_4\), and ethyne, \(\text{C}_2\text{H}_2\), are shown below.

Which of the following correctly identifies the hybridization of each carbon atom in ethyne and the total number of \(\sigma\) and \(\pi\) bonds in one molecule of ethyne?

The complete Lewis diagrams for ethene, \(\text{C}_2\text{H}_4\), and ethyne, \(\text{C}_2\text{H}_2\), are shown below.

Which of the following correctly identifies the hybridization of each carbon atom in ethyne and the total number of \(\sigma\) and \(\pi\) bonds in one molecule of ethyne?

![Two Lewis diagrams are shown side by side in grayscale on a plain white background. On the left is the Lewis diagram for ethene, labeled below with the formula \(\text{C}_2\text{H}_4\). It consists of two central \(\text{C}\) atom symbols connected to each other by a double line representing a double bond. Each \(\text{C}\) atom is also bonded to two \(\text{H}\) atom symbols with single lines arranged at approximately \(120^\circ\) angles, with no lone pairs on any atom. On the right is the Lewis diagram for ethyne, labeled below with the formula \(\text{C}_2\text{H}_2\). It consists of two central \(\text{C}\) atom symbols connected by three parallel horizontal lines representing a triple bond. Each \(\text{C}\) atom is bonded to one terminal \(\text{H}\) atom symbol by a single horizontal line in a linear arrangement, with no lone pairs on any atom. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787299937-f9qi5E.jpg)

- **A.** Hybridization of each \(\text{C}\) atom: \(sp^2\) ; Total number of bonds: \(3\ \sigma\) and \(2\ \pi\)
- **B.** Hybridization of each \(\text{C}\) atom: \(sp\) ; Total number of bonds: \(3\ \sigma\) and \(2\ \pi\)
- **C.** Hybridization of each \(\text{C}\) atom: \(sp\) ; Total number of bonds: \(1\ \sigma\) and \(2\ \pi\)
- **D.** Hybridization of each \(\text{C}\) atom: \(sp^2\) ; Total number of bonds: \(1\ \sigma\) and \(2\ \pi\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119770/*