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Ch.8 - Basic Concepts of Chemical Bonding
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.8 - Basic Concepts of Chemical Bonding문제 59
8장, 문제 59

Consider a Lewis structure for SO3 that satisfies the octet rule. Which of the following statements is or are true?
i. SO3 has three equivalent resonance structures.
ii. There are one shorter and two longer S—O bond lengths in SO3.
iii. The S atom in SO3 has a nonzero formal charge.

검증된 단계별 안내
1
Step 1: Draw the Lewis structure for \( \text{SO}_3 \). Start by counting the total number of valence electrons. Sulfur (S) has 6 valence electrons, and each oxygen (O) also has 6 valence electrons. Therefore, \( \text{SO}_3 \) has a total of \( 6 + 3 \times 6 = 24 \) valence electrons.
Step 2: Arrange the atoms with sulfur in the center and the three oxygen atoms surrounding it. Distribute the electrons to satisfy the octet rule for each atom. Initially, connect each oxygen to sulfur with a single bond, using 6 electrons (2 per bond).
Step 3: Distribute the remaining 18 electrons to complete the octets of the oxygen atoms. Each oxygen will need 6 more electrons to complete its octet, using up all 18 remaining electrons.
Step 4: Check the formal charges. The formal charge is calculated as: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \). Calculate the formal charges for sulfur and each oxygen atom.
Step 5: Consider resonance structures. Since the sulfur can form double bonds with each oxygen, there are three equivalent resonance structures where the double bond is with a different oxygen each time. This results in all S—O bonds being equivalent in length, and the formal charge on sulfur being zero.

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주요 개념

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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 help visualize the arrangement of electrons and the connectivity of atoms, allowing chemists to predict molecular geometry and reactivity. In the case of SO3, drawing its Lewis structure involves ensuring that the octet rule is satisfied for each atom, particularly the sulfur and oxygen atoms.
추천 영상:
가이드 코스
04:28
Lewis Dot Structures: Ions

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In SO3, resonance structures show that the double bonds between sulfur and oxygen can be distributed among the three S—O bonds, leading to equivalent structures. This concept is crucial for understanding the stability and properties of molecules that cannot be accurately represented by a single Lewis structure.
추천 영상:
가이드 코스
01:42
Resonance Structures

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 bonds, and the number of lone pair electrons. It helps assess the stability of a molecule and the distribution of electrons. In SO3, calculating the formal charge on the sulfur atom reveals whether it carries a charge, which is important for understanding the molecule's reactivity and resonance.
추천 영상:
가이드 코스
01:53
Formal Charge
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i. Benzene has two equivalent resonance structures.

ii. There are no nonbonding pairs in the Lewis structure for benzene.

iii. Benzene has three short and three long C—C bonds.

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