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Chapter 13: Problem 13

Revise (as necessary) your checklist that can be used to determine if a Lewis structure for a molecule is correct.

Short Answer

Expert verified
To check if a Lewis structure for a molecule is correct, one can follow these steps: verify the sum of valence electrons, check the central atom, arrange remaining atoms, ensure the octets are complete, arrange any extra electrons, check individual formal charges and verify the presence of necessary multiple bonds.

Step by step solution

01

Verifying the Sum of Valence Electrons

Check the total number of valence electrons in the molecule. Valence electrons are those present in the outermost shell of an atom which can be involved in the formation of a bond. The total number of valence electrons should be equal to the sum of valence electrons of all individual atoms.
02

Checking the Central Atom

In general (but not always), the atom with the lowest electronegativity serves as the central atom. Central atoms are typically surrounded by other atoms and electron pairs. It's important to make sure this is represented accurately in the Lewis structure.
03

Placing the Remaining Atoms

Surround the central atom with the remaining atoms. Draw single bonds between the central atom and surrounding atoms. A single bond represents a pair of shared electrons.
04

Completing the Octets

Complete the octets of the atoms bonded to the central atom. This involves placing the remaining electrons as lone pairs on the atoms. The atoms (except hydrogen) should now have an octet of electrons.
05

Arranging Extra Electrons

If there are any leftover electrons after filling the octet of the central atom, place them on the central atom.
06

Checking Formal Charges

Check the formal charges of each atom. The formal charge is calculated as the number of valence electrons in the free atom, minus the number of lone pair electrons, and minus half the number of bonding electrons. The sum of all formal charges in the molecule should be zero, or match the overall charge of the molecule.
07

Verifying Multiple Bonds

If the central atom does not have a complete octet, form double or triple bonds as needed. After each modification, repeat the formal charge calculation to verify that the structure with the lowest formal charge is obtained.

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Most popular questions from this chapter

Without attempting to draw a Lewis structure, calculate the total number of valence electrons in each of these molecules: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)

What is the likely formula for a molecule composed of hydrogen atoms and one sulfur atom? Draw the Lewis structure for this molecule.

For each of the following neutral atoms give the core charge. a) Li. b) \(\quad \ddot{C l}\) c) He:

For \(\mathrm{N}_{2}\), is the sum of the bonding electrons and nonbonding electrons around each nitrogen atom consistent with the Lewis model?

Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms?
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