Calculate the formal charge of the indicated atom in the following molecules or ions.
(f)

검증된 단계별 안내

Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons).

Step 2: Identify the atom in question. In this case, the atom is the oxygen circled in blue.

Step 3: Determine the number of valence electrons for oxygen. Oxygen is in Group 16 of the periodic table, so it has 6 valence electrons.

Step 4: Count the non-bonding electrons (lone pairs) on the oxygen atom. From the structure, there are 4 non-bonding electrons (two lone pairs).

Step 5: Count the bonding electrons. The oxygen atom is involved in a single bond with the carbon atom, which contributes 2 bonding electrons. Use the formula to calculate the formal charge.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, 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.

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 are essential for visualizing the arrangement of electrons and understanding how formal charges are distributed among atoms in a molecule.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. Knowing the number of valence electrons for each atom is crucial for calculating formal charges and drawing accurate Lewis structures.

Calculate the formal charge of the indicated atom in the following molecules or ions. (f)