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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 95a
8장, 문제 95a

The following three Lewis structures can be drawn for N2O:
(a) Using formal charges, which of these three resonance forms is likely to be the most important?

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1
Identify the three possible Lewis structures for N2O. Each structure should have a different arrangement of single, double, or triple bonds between the nitrogen and oxygen atoms.
Calculate the formal charge for each atom in each of the three Lewis structures. The formal charge can be calculated using the formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \).
Compare the formal charges across the three structures. The most stable structure typically has the smallest formal charges on each atom, ideally as close to zero as possible.
Consider the electronegativity of the atoms involved. Oxygen is more electronegative than nitrogen, so it is preferable for oxygen to have a negative formal charge if any atom must have one.
Select the resonance structure with the most favorable formal charges and distribution, taking into account both the magnitude of the charges and the electronegativity of the atoms.

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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 use dots to represent valence electrons and lines to represent bonds. Understanding how to draw and interpret Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
추천 영상:
가이드 코스
04:28
Lewis Dot Structures: Ions

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 electrons. It helps in determining the most stable resonance structure by minimizing the formal charges across the molecule. A lower formal charge on atoms generally indicates a more stable structure.
추천 영상:
가이드 코스
01:53
Formal Charge

Resonance Structures

Resonance structures are different Lewis structures that represent the same molecule, differing only in the arrangement of electrons. They illustrate the delocalization of electrons within a molecule, which can affect its stability and reactivity. The true structure of the molecule is a hybrid of these resonance forms, and the most significant contributors are those with the lowest formal charges.
추천 영상:
가이드 코스
01:42
Resonance Structures
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교과서 질문

Mothballs are composed of naphthalene, C10H8, a molecule that consists of two six-membered rings of carbon fused along an edge, as shown in this incomplete Lewis structure:(a) Draw all of the resonance structures of naphthalene. How many are there?

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교과서 질문

The following three Lewis structures can be drawn for N2O:

(b) The N—N bond length in N2O is 1.12 Å, slightly longer than a typical N≡N bond; and the N—O bond length is 1.19 Å, slightly shorter than a typical N═O bond (see Table 8.4). Based on these data, which resonance structure best represents N2O?

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교과서 질문

The hypochlorite ion, ClO-, is the active ingredient in bleach. The perchlorate ion, ClO4-, is a main component of rocket propellants. Draw Lewis structures for both ions. (b) What is the formal charge of Cl in the perchlorate ion, assuming the Cl—O bonds are all single bonds?

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교과서 질문

The triiodide ion, I3-, exists, whereas the corresponding ion with fluorine, F3-, does not. The I3- ion has a linear structure in which two outer I atoms are each bonded to a central I atom. Although I3- is a known ion, F3- is not.

c. Which of the following statements about the existence of I3- versus the nonexistence of F3- is or are true?

i. The Lewis structure of I3- shows 12 electrons around the central I atom.

ii. Elements from the second row of the periodic table generally do not form hypervalent molecules and ions.

iii. An I atom can form a hypervalent molecule or ion more readily than an F atom because of the larger size of the I atom.


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교과서 질문

Structures A, B, and C show the connectivity of the atoms in three different molecules that are isomers of C3H4O. By completing the Lewis structures of these molecules, complete the information in the following table:

Isomer A Isomer B Isomer C

Number of single bonds

Number of double bonds

Number of triple bonds

Number of nonbonding pairs

교과서 질문

Mothballs are composed of naphthalene, C10H8, a molecule that consists of two six-membered rings of carbon fused along an edge, as shown in this incomplete Lewis structure:

(b) Do you expect the C—C bond lengths in the molecule to be similar to those of C—C single bonds, C ═C double bonds, or intermediate between C—C single and C ═C double bonds?

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