Identify the errors in each of the following Lewis structures and draw the correct formula(6.6)

Verified step by step guidance

1. Identify the total number of valence electrons for each atom in the molecule: Carbon (C) has 4, Oxygen (O) has 6, Nitrogen (N) has 5, and each Hydrogen (H) has 1.
2. Calculate the total number of valence electrons in the molecule: 4 (C) + 6 (O) + 5 (N) + 4*1 (H) = 19 valence electrons.
3. Check the octet rule for each atom: Carbon and Nitrogen should have 8 electrons around them, while Oxygen should also have 8 electrons. Hydrogen should have 2 electrons.
4. Identify the errors in the structure: The structure shows a total of 20 electrons, which is incorrect. Additionally, the octet rule is not satisfied for Carbon and Nitrogen.
5. Redraw the Lewis structure ensuring the correct number of valence electrons and satisfying the octet rule for Carbon, Oxygen, and Nitrogen.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw and interpret Lewis structures is crucial for visualizing molecular geometry and predicting reactivity.

Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule. It is calculated by taking the number of valence electrons in an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. A correct Lewis structure minimizes formal charges across the molecule, leading to a more stable configuration.

Octet Rule

The octet rule states that atoms tend to form bonds in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule is fundamental in predicting how atoms will bond and interact in a molecule, particularly for main group elements.