CO32- Lewis structure

The CO₃^2- Lewis structure represents a carbonate ion consisting of one carbon atom and three oxygen atoms. The carbon atom forms one double bond and two single bonds with the three oxygen atoms. Among these, the oxygen atom that shares a double bond has two lone pairs, while the two oxygen atoms that share single bonds have three lone pairs each. The two oxygen atoms attached by single bonds carry a negative charge of -1.

To draw an accurate CO₃^2- Lewis structure, start by sketching a rough structure of the molecule and indicating the locations of any lone pairs on the atoms. Then, determine the formal charges on the atoms and minimize them by converting any available lone pairs to chemical bonds. Repeat this step until all charges are minimized, ensuring that the octet rule is satisfied for both the central atom and the surrounding atoms. Following these steps results in a stable CO₃^2- Lewis structure that depicts the arrangement of atoms and electrons in the molecule.

Alternative method: Lewis structure of CO₃^2-

Rough sketch

The first step in drawing the CO₃^2- Lewis structure is to determine the total number of valence electrons in the molecule. This can be calculated by multiplying the valence electrons of each atom. Carbon is located in group 14 of the periodic table and has four valence electrons, while oxygen, belonging to group 16, has six valence electrons. In CO₃^2-, which consists of one carbon atom and three oxygen atoms, the total valence electrons can be calculated as follows: the valence electrons of one carbon atom are 4 × 1 = 4, and the valence electrons of three oxygen atoms are 6 × 3 = 18. Since CO₃^2- carries a negative (-2) charge, two more electrons need to be added, bringing the total number of valence electrons to 24.

Learn how to find: Carbon valence electrons and Oxygen valence electrons

The second step in drawing the CO₃^2- Lewis structure is to determine the total number of electron pairs in the molecule. This is done by dividing the total number of valence electrons by two. In the case of CO₃^2-, which has a total of 24 valence electrons, the number of electron pairs is calculated as 24 ÷ 2 = 12. This means that there are a total of 12 electron pairs in the CO₃^2- molecule that need to be distributed among the atoms to form a stable Lewis structure.

Once the total number of electron pairs has been determined, the next step in drawing the CO₃^2- Lewis structure is to identify the central atom. The least electronegative atom is typically placed in the center, and in the case of CO₃^2-, carbon is less electronegative than oxygen. Therefore, carbon should be placed in the center and the oxygen atoms should be arranged around it. With this in mind, a rough sketch of the CO₃^2- Lewis structure can be drawn.

Lone pair

After sketching the CO₃^2- Lewis structure, the next step is to indicate the location of lone pairs on the atoms. Based on the calculation, it has been determined that there are a total of 12 electron pairs in the CO₃^2- molecule. Since three C – O bonds, utilizing six electron pairs, have already been marked in the sketch, the remaining nine electron pairs need to be indicated as lone pairs on the atoms.

It’s worth noting that both carbon and oxygen are period 2 elements, which means they can accommodate a maximum of eight electrons in their outermost shell.

To ensure the correct distribution of electrons and to satisfy the octet rule, it is important to start indicating the lone pairs from the outer atoms. In the case of CO₃^2-, the outer atoms are oxygen. Therefore, each oxygen atom must have three lone pairs, while the central carbon atom should not have any lone pair as all nine electron pairs are utilized. Carefully mark the lone pairs on the sketch according to this arrangement to create a stable Lewis structure.

Formal charge

The formal charges for the atoms in CO₃^2- can be calculated using the following formula: Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons. For the carbon atom, the formal charge can be calculated as 4 – 0 – ½ (6) = +1. Similarly, for each oxygen atom, the formal charge can be calculated as 6 – 6 – ½ (2) = -1.

Atom	Valence electron	Nonbonding electron	Bonding electron	Formal charge
Carbon	4	0	6	+1
Oxygen	6	6	2	-1

Once the formal charges have been determined, mark them on the sketch of the molecule accordingly to indicate the charge on each atom.

The current Lewis structure of CO₃^2- is not stable as both carbon and oxygen atoms have charges. In order to stabilize the structure, it is necessary to reduce the charges by converting lone pairs to bonds.

To minimize the formal charges in the CO₃^2- molecule, it is necessary to create a new C – O bond by converting a lone pair of one of the oxygen atoms to a bonding pair with the central carbon atom.

Final structure

The final structure of CO₃^2- comprises a central carbon atom linked to three oxygen atoms. In this arrangement, the carbon atom forms one double bond with one oxygen atom and single covalent bonds with the remaining two oxygen atoms to satisfy the octet rule. Within this configuration, the double-bonded oxygen atom maintains two lone pairs, while the two single-bonded oxygen atoms each retain three lone pairs. This arrangement represents the most stable state for the ion because it results in a formal charge of zero on the carbon and the double-bonded oxygen, and a formal charge of -1 on each of the two single-bonded oxygen atoms. As a result, this specific electronic distribution serves as the definitive and most accurate Lewis representation of the carbonate ion.

To complete the representation, draw square brackets around the entire Lewis structure and place a “2-” sign as a superscript outside the upper right bracket. This notation signifies that the negative charge is a property of the whole ion.

Next: PF₆^– Lewis structure

External video

• CO32- Lewis Structure – How to Draw the Lewis Structure for CO3 2- (Carbonate Ion) – YouTube • Wayne Breslyn

External links

• Draw a Lewis structure for CO32 – Homework.Study.com
• Carbonate (CO32-) Formal Charge – Chemistry Learner
• What is the Lewis structure of CO3 2-? – Quora
• Draw the Lewis structure for carbonate (CO32−) – Chegg
• Lewis Dot of Carbonate CO32- – Kent’s Chemistry
• What is the Lewis structure of CO3 2-? – Quora
• How many resonance structures are there for CO₃^2-? – Socratic
• Chemical Bonding: CO32- Lewis Structure – The Geoexchange
• What is co3 2- lewis structure? – Brainly
• For CO32, carbonate ion, draw the Lewis structure (by counting valence electrons of each atom) – Course Hero
• structure of (CO3)2- – Laurence Lavelle
• Draw the Lewis structure for CO32- including any valid resonance structures – Numerade
• Draw the Lewis structure for the carbonate ion (CO32; carbon is the central atom) and any relevant resonance structures – Bartleby
• Carbonate Ion | CO3-2 | CID 19660 – National Institutes of Health (.gov)
• How many equivalent Lewis structures are there for CO32-? – Answers
• Lewis Structure for CO32- | Carbonate ion – Chemistry School
• 9.4: Resonance Lewis Structures – Chemistry LibreTexts