Draw the Lewis Dot Structure for CO 2 compound.

Draw the Lewis dot structure for c l 2 compound, so that's carbon dioxide. So we're gonna say the total number of valence electrons is carbons in group 4 a, so it has 4 valence electrons. Oxygen's in group 6 a, and there's 2 of them, so that's 12. So we have a total of 16 electrons. Carbon's gonna go in the center. We're gonna draw single bonds to the oxygens, add enough electrons to the surrounding elements so they're following the octet rule. At this present moment, we've used all 16 of our electrons because we have 2, 4, 6, 8, 10, 12, 14, 16 electrons. The oxygens are happy because they're following the octet rule, but there's something wrong. The carbon itself is not following the octet rule. It only has around it 4 electrons. It needs 4 more to get to the octet rule. Also remember that carbon wants to make 4 bonds. Here it's only making 2. So to rectify this, to correct this error, we're going to take a lone pair from each oxygen and use it to make a double bond. So carbon dioxide would actually look like this. I'm taking a lone pair from each oxygen and helping to make a double bond on each side of carbon. So this would be the correct way of drawing carbon dioxide, not this way up above. In this way, we're using all 16 of our valence electrons, oxygen is making its ideal number of bonds in 2, Carbon is making its ideal number of bonds in 4. Each oxygen also has 2 lone pairs on it.

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10. Chemical Bonding

Lewis Dot Structures: Multiple Bonds

Introduction to Chemistry

10. Chemical Bonding

Lewis Dot Structures: Multiple Bonds

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Multiple Choice

Draw the Lewis Dot Structure for CO₂ compound.

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Identify the total number of valence electrons in the CO2 molecule. Carbon (C) has 4 valence electrons, and each Oxygen (O) has 6 valence electrons. Therefore, the total number of valence electrons is 4 + 6 + 6 = 16.

Determine the central atom in the molecule. Carbon is typically the central atom because it can form multiple bonds and is less electronegative than oxygen.

Arrange the atoms with carbon in the center and oxygen atoms on either side. This forms the basic skeleton of the molecule: O-C-O.

Distribute the valence electrons around the atoms to satisfy the octet rule. Start by placing a pair of electrons between each carbon and oxygen atom to form a bond. Then, distribute the remaining electrons to complete the octets of the oxygen atoms.

Form double bonds between the carbon and each oxygen atom to ensure that all atoms have complete octets. This involves sharing additional pairs of electrons between carbon and each oxygen, resulting in the final Lewis structure with double bonds: O=C=O.