Chemistry, 20.07.2019 09:30 krocker58

Draw the structure of co32−. include all lone pairs of electrons and formal charges.

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Answer from: crismelycalderon1904

The Lewis structure for the carbonate ion is attached as shown. The lone pairs are the electron dots around the oxygen elements. The formula for the formal charge is also given. Using the formula, the formal charge for each element of the compound was determined as shown.
Draw the structure of co32−. include all lone pairs of electrons and formal charges.

Draw the structure of co32−. include all lone pairs of electrons and formal charges.

Answer from: DominaterDreemurr

The Lewis structure for ${\mathbf{CO}}_{\mathbf{3}}^{{\mathbf{2 - }}}$ is attached in the image.

Further Explanation:

Lewis structures are simple representations where the arrangement of electrons are around an individual atom of an element in a molecule is shown. Electrons are shown by dots and bonded electrons are shown by straight lines between two atoms. They are also called Lewis dot structures.In covalent compounds, the geometry, polarity, and reactivity are predicted by these structures.

Lewis structure of ${\text{CO}}_3^{ - 2}$ (Refer to the structure in the attached image):

The total number of valence electrons of ${\text{CO}}_3^{ - 2}$ is calculated as,

Total valence electrons = [(1) (Valence electrons of C) + (3) (Valence electrons of O) + Charge on anion]

$\begin{aligned}{\text{Total valence electrons}}\left({{\text{TVE}}} \right)&= \left[ {\left( {\text{1}} \right)\left( 4 \right) + \left( {\text{4}} \right)\left( 6 \right) + 2} \right]\\&= 30\\\end{aligned}$

Formal charge:

It is the charge that an atom acquires in a molecule by considering that the chemical bonds are shared equally between the two atoms, irrespective of their electronegativities.

The formula to calculate the formal charge on an atom is as follows:

${\mathbf{Formal charge=}}\left[ \begin{gathered}\left[ \begin{gathered}{\mathbf{total number of valence electrons }}\hfill\\{\mathbf{in the free atom}} \hfill \\\end{gathered} \right]{\mathbf{ }} -\\\left[ {{\mathbf{total number of non - bonding electrons}}} \right] - \\\frac{{\left[ {{\mathbf{total number of bonding electrons}}} \right]}}{{\mathbf{2}}} \\\end{gathered} \right]$ ......(1)

C forms two single bonds with two oxygen atoms and one double bond with one oxygen atom

The total number of valence electrons in free carbon atom is 4.

The total number of non-bonding electrons in carbon is 0.

The total number of bonding electrons in carbon is 8.

Substitute these values in equation (1) to find the formal charge on carbon.

$\begin{aligned}{\text{Formal charge on Carbon}} &= \left[ {4 - 0 - \frac{8}{2}} \right]\\&= 0\\\end{aligned}$

For oxygen atoms,

Total number of valence electrons in free oxygen atom is 6.

The total number of non-bonding electrons in O is 4.

The total number of bonding electrons in O is 4.

Substitute these values in equation (1) to find the formal charge on green O.

$\begin{aligned}{\text{Formal charge on green O}}&=\left[ {6 - 4 - \frac{4}{2}} \right]\\&= 0\\\end{aligned}$

Total number of valence electrons in free oxygen atom is 6.

The total number of non-bonding electrons in O is 6.

The total number of bonding electrons in O is 2.

Substitute these values in equation (1) to find the formal charge on red O.

$\begin{aligned}{\text{Formal charge on red O}}&= \left[ {6 - 6 - \frac{2}{2}} \right]\\&=- 1\\\end{aligned}$

Total number of valence electrons in free oxygen atom is 6.

The total number of non-bonding electrons in O is 6.

The total number of bonding electrons in O is 2.

Substitute these values in equation (1) to find the formal charge on red O.

$\begin{aligned}{\text{Formal charge on red O}}&= \left[ {6 - 6 - \frac{2}{2}} \right]\\&=- 1\\\end{aligned}$

Carbon atom has 4 valence electrons, and oxygen atom has 6 valence electrons. The green-colored oxygen atoms form one double bond with carbon atom, two lone pairs are present on it. Both red-colored oxygen atom forms one single bond with the carbon atom, and six lone pairs are present on them. Therefore the Lewis structure of ${\mathbf{CO}}_{\mathbf{3}}^{{\mathbf{2 - }}}$ is attached in the image.

Learn more:

1. Draw the Lewis structure of Butanal:

2. Draw the Lewis structure of bromide ion:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Chemical Compounds

Keywords: lewis structures, formal charges, carbonate ion, oxygen, carbon, geometry and polarity.

Answer from: Quest

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Answer from: Quest

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