Questions: Which of the following represents a covalent molecule? SELECT ALL THAT APPLY a O₂ b Cl₂ c He d CO₂

Transcript text: Which of the following represents a covalent molecule? SELECT ALL THAT APPLY a $\mathrm{O}_{2}$ b $\mathrm{Cl}_{2}$ c He d $\mathrm{CO}_{2}$

Solution

Solution Steps

Step 1: Understanding Covalent Molecules

Covalent molecules are formed when two or more non-metal atoms share electrons to achieve a full outer shell, resulting in a stable molecule. This type of bonding typically occurs between non-metal elements.

Step 2: Analyzing Each Option

Option a: $\mathrm{O}_{2}$
Oxygen ($\mathrm{O}_{2}$) is a diatomic molecule where two oxygen atoms share electrons, forming a covalent bond. Thus, $\mathrm{O}_{2}$ is a covalent molecule.
Option b: $\mathrm{Cl}_{2}$
Chlorine ($\mathrm{Cl}_{2}$) is another diatomic molecule where two chlorine atoms share electrons, forming a covalent bond. Therefore, $\mathrm{Cl}_{2}$ is a covalent molecule.
Option c: He
Helium (He) is a noble gas and exists as a single atom. It does not form covalent bonds because it already has a full outer electron shell.
Option d: $\mathrm{CO}_{2}$
Carbon dioxide ($\mathrm{CO}_{2}$) consists of one carbon atom double-bonded to two oxygen atoms. These are covalent bonds, making $\mathrm{CO}_{2}$ a covalent molecule.