Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.
(a)

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Identify the formal charge on each atom in the molecule. Recall that formal charge is calculated using the formula:

Formal Charge = (Valence Electrons) - (Non-Bonding Electrons) - (1/2 × Bonding Electrons)

Determine the number of valence electrons for each atom based on its position in the periodic table. For example, oxygen has 6 valence electrons, nitrogen has 5, etc.

Using the formal charge and the number of valence electrons, calculate the number of lone pair electrons for each atom. Lone pairs are the non-bonding electrons that remain after accounting for bonding electrons.

Draw the Lewis structure of the molecule, ensuring that the total number of electrons matches the sum of the valence electrons for all atoms in the molecule. Place lone pairs on atoms to satisfy their formal charges and the octet rule (if applicable).

Double-check the structure to ensure that the formal charges on all atoms are consistent with the given information and that the total charge of the molecule matches the overall charge (if any).

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주요 개념

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Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated by taking the number of valence electrons in the free atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms.

Lone Pairs

Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a single atom. They play a crucial role in determining the geometry and reactivity of molecules, as they can influence the shape and polarity of the molecule due to their repulsive interactions with bonding pairs.

Electron Pair Geometry

Electron pair geometry refers to the spatial arrangement of all electron pairs (bonding and lone pairs) around a central atom. Understanding this geometry is essential for predicting molecular shapes and angles, which are determined by the repulsion between electron pairs according to VSEPR (Valence Shell Electron Pair Repulsion) theory.

Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs. (a)