Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경

Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

문제 106

9장, 문제 106

Place the following molecules and ions in order from smallest to largest bond order: N22+, He2+, Cl2 H2-, O22-.

검증된 단계별 안내

Bond order is calculated using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.

Determine the molecular orbital configuration for each species.

For N2^{2+}, remove two electrons from the highest occupied molecular orbitals of N2.

For He2^{+}, remove one electron from the highest occupied molecular orbital of He2.

For Cl2 and H2^{-}, use their respective molecular orbital configurations to calculate bond order.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

13m

주요 개념

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

Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms. It is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. A higher bond order indicates a stronger bond and typically a shorter bond length. Understanding bond order is essential for comparing the stability and size of different molecules and ions.

Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. This theory helps predict the bond order and stability of molecules by considering the distribution of electrons in bonding and antibonding orbitals. It is particularly useful for understanding diatomic molecules and ions, as it provides insight into their electronic structure and reactivity.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom or molecule's orbitals. For diatomic molecules, the arrangement of electrons in molecular orbitals determines their bond order and stability. Understanding the electron configuration of the given species is crucial for determining their bond orders and comparing their sizes, as it directly influences their chemical properties and behavior.

관련 실천

교과서 질문

One of the molecular orbitals of the H2- ion is sketched below:

(a) Is the molecular orbital a s or p MO? Is it bonding or antibonding?

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교과서 질문

One of the molecular orbitals of the H2- ion is sketched below: (d) Compared to the H¬H bond in H2, the H¬H bond in H2- is expected to be which of the following: (i) Shorter and stronger, (ii) longer and stronger, (iii) shorter and weaker, (iv) longer and weaker, or (v) the same length and strength?

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교과서 질문

The highest occupied molecular orbital of a molecule is abbreviated as the HOMO. The lowest unoccupied molecular orbital in a molecule is called the LUMO. Experimentally, one can measure the difference in energy between the HOMO and LUMO by taking the electronic absorption (UV-visible) spectrum of the molecule. Peaks in the electronic absorption spectrum can be labeled as π_2p-π_2p*, σ_s-σ_2s*, and so on, corresponding to electrons being promoted from one orbital to another. The HOMO-LUMO transition corresponds to molecules going from their ground state to their first excited state. (c) The electronic absorption spectrum of the N₂ molecule has the lowest energy peak at 170 nm. To what orbital transition does this correspond?

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교과서 질문

Molecules that are brightly colored have a small energy gap between filled and empty electronic states (the HOMOLUMO gap; see Exercise 9.104). Suppose you have two samples, one is lycopene which is responsible for the red color in tomato, and the other is curcumin which is responsible for the yellow color in turmeric. Which one has the larger HOMO-LUMO gap?

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교과서 질문

Azo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azobenzene, C12H10N2. A closely related substance is hydrazobenzene, C12H12N2. The Lewis structures of these two substances are

(Recall the shorthand notation used for benzene.) (b) How many unhybridized atomic orbitals are there on the N and the C atoms in each of the substances? How many unhybridized atomic orbitals are there on the N and the C atoms in hydrazobenzene?

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교과서 질문

(Recall the shorthand notation used for benzene.) (c) Predict the N¬N¬C angles in each of the substances.

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