Lewis Structure of Carbon Dioxide (CO2): A Double Bond Example

📚 Quick Study Guide

• ⚛️ Carbon dioxide ($CO_2$) consists of one carbon atom and two oxygen atoms.
• 🤝 Carbon needs four electrons to complete its octet, while oxygen needs two.
• 👯 This leads to the formation of two double bonds between the carbon atom and each oxygen atom ($O=C=O$).
• ✍️ The Lewis structure shows carbon as the central atom, double-bonded to each oxygen atom. Each oxygen atom has two lone pairs of electrons.
• ⚖️ The molecule is linear and nonpolar due to the symmetrical arrangement of the double bonds.

🧪 Practice Quiz

1. What is the central atom in the Lewis structure of carbon dioxide ($CO_2$)?
   1. Hydrogen
   2. Oxygen
   3. Carbon
   4. Nitrogen
2. How many double bonds are present in the Lewis structure of $CO_2$?
   1. 1
   2. 2
   3. 3
   4. 0
3. What is the molecular geometry of carbon dioxide?
   1. Bent
   2. Tetrahedral
   3. Linear
   4. Trigonal Planar
4. How many lone pairs of electrons are on each oxygen atom in $CO_2$?
   1. 1
   2. 2
   3. 3
   4. 0
5. What is the total number of valence electrons in carbon dioxide ($CO_2$)?
   1. 12
   2. 16
   3. 18
   4. 20
6. Which of the following statements is true regarding the polarity of $CO_2$?
   1. It is polar due to the electronegativity difference.
   2. It is nonpolar due to its symmetrical structure.
   3. It is ionic.
   4. It has a slight positive charge.
7. What type of bond exists between carbon and oxygen in $CO_2$?
   1. Single bond
   2. Double bond
   3. Triple bond
   4. Ionic bond