Question

draw the lewis structure for co₂. draw the molecule by placing atoms on the grid and connecting them with bonds. include all lone pairs of electrons.

Explanation:

Step1: Determine Valence Electrons

Carbon (C) has 4 valence electrons, and each Oxygen (O) has 6 valence electrons. For \( \ce{CO2} \), total valence electrons: \( 4 + 2\times6 = 16 \).

Step2: Arrange Atoms

Place C in the center, with two O atoms on either side (linear arrangement).

Step3: Form Bonds

Connect C to each O with a double bond (each double bond uses 4 electrons: 2 from C, 2 from O). After two double bonds (\( \ce{C=O} \) bonds), each O has 2 remaining lone pairs (4 electrons per O, since 4 are used in the double bond; \( 6 - 2 = 4 \), or 2 lone pairs). The C has no lone pairs (4 electrons used in two double bonds, \( 4 - 4 = 0 \)).

Step4: Draw Structure

On the grid, place C in the middle. Place one O on the left and one on the right. Use the double - bond tool (the double - line icon) to connect C to each O. Then, use the lone - pair tool (the icon with two dots) to add two lone pairs to each O.

Answer:

The Lewis structure of \( \ce{CO2} \) has a central C atom double - bonded to two O atoms (\( \ce{O=C=O} \)), with each O atom having two lone pairs of electrons. When drawing on the grid: place C in the center, O on left and right, connect C - O with double bonds, and add two lone pairs (four electrons) to each O.