**Use formal charge to choose the best Lewis structure for CH3SeOCH3**

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## Question “Use formal charge to choose the best Lewis structure for CH3SeOCH3”

Use formal charge to choose the best Lewis structure for CH_{3}SeOCH_{3}.

## Answer

These steps are required to create the Lewis structures of molecular compounds.

(1) The correct skeleton structure should be first written.

(2) Once you have written the skeleton structure, calculate the total number of electrons by adding the valence electrons for each atom in the compound.

(3) All electrons must be distributed so that each atom has complete octets.

(4) To give an octet to any atom that is missing one, double or triple bond the atom.

And,

These rules will help you determine the best Lewis structure without formal charges:

(1) All formal charges must be omitted from a neutral molecule.

(2) The sum of all formal charges in an ion must equal the charge for the ion.

The following formula determines the form of an atom’s formal charge:

…… (1)

(a)

Calculate the formal charge for each atom in the given structure using equation (1). The sum of all formal charges must equal zero according to the rule for correct Lewis structure.

Substitute 1 for all Hydrogen Atoms for the number of valence electrons; zero for non-bonding electrons; and 2 for bonding electrons

Thus,

Substitute 4 for the number of valence electrons for first Carbon atom. Zero for non-bonding electrons; 10 for bonding electrons.

Thus,

Substitute 4 for the number of valence electrons for second Carbon atom. Zero for non-bonding electrons. 8 for bonding electrons.

Thus,

Substitute 6 for Oxygen atom for the number of valence electrons. 6 for non-bonding electrons. 4 for bonding electrons.

Thus,

For Sulphur atom substitute 6 for the number of valence electrons, 0 for non-bonding electrons, and 10 for bonding electrons

Thus,

Now calculate the sum of all formal fees as follows:

**This is not the correct Lewis structure for**

(b)

Calculate the formal charge for each atom in the given structure (1). The sum of all formal charges must equal zero according to the rule for correct Lewis structure.

Substitute 1 for all Hydrogen Atoms for the number of valence electrons; zero for non-bonding electrons; and 2 for bonding electrons

Thus,

Substitute 4 for the number of valence electrons for both Carbon atoms, and zero for non-bonding electrons.

Thus,

Substitute 6 for Oxygen atom for the number of valence electrons. 4 for non-bonding electrons. 4 for bonding electrons.

Thus,

Substitute 6 for the number of valence electrons for Sulphur, 2 for non-bonding electrons, and 8 for bonding electrons for Sulphur.

Thus,

The total formal charge is therefore also zero.

**This is the correct Lewis structure for**

**.**

(c)

This structure is incorrect because oxygen atoms must be attached by two other atoms using a single bond. If it is attached only to one atom, then the bond must have a double bond.

This is where oxygen is linked to Sulphur via a single bond.

**This is not the correct Lewis structure for**

**.**

(d)

This structure is incorrect because oxygen atoms must be attached by single bonds to each other. If it is attached to one atom, then the bond must consist of a double bond.

This is where oxygen is linked to Sulphur via a single bond. One of the five bonds for carbon atoms is 5 but carbon can only make 4 bonds.

**This is not the correct Lewis structure for**

**.**

## Conclusion

Above is the solution for “**Use formal charge to choose the best Lewis structure for CH3SeOCH3**“. We hope that you find a good answer and gain the knowledge about this topic of **science**.