Based on the formal charge, determine how many lone pairs are on each indicated atom.
(a)

Verified step by step guidance

1. Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons). This formula will help us determine the number of lone pairs on the indicated atom.
2. Step 2: Identify the valence electrons for the indicated atom. Refer to the periodic table to determine the number of valence electrons for the atom in question.
3. Step 3: Count the bonding electrons around the indicated atom. These are the electrons shared in covalent bonds. Each bond contributes two electrons.
4. Step 4: Count the non-bonding electrons (lone pairs) around the indicated atom. These are the electrons not involved in bonding. Use the formal charge formula to solve for the number of non-bonding electrons.
5. Step 5: Divide the non-bonding electrons by two to determine the number of lone pairs on the indicated atom. Verify your result by ensuring the formal charge matches the given or expected value.

Key Concepts

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 specific 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.

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 provide a visual representation of the arrangement of electrons, allowing for the determination of formal charges and the identification of lone pairs on specific atoms.