/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 76 Why are all diatomic molecules l... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 76

Why are all diatomic molecules linear, regardless of the number of valence electron pairs on the atoms involved?

Short Answer

Expert verified
All diatomic molecules are linear because they consist of only two connected atoms, allowing for only one possible shape. Regardless of the number of valence electron pairs on each atom, the linear shape remains the same, as the structure is determined by the bonding between the atoms and the repulsion forces between electron pairs, according to the Valence Shell Electron Pair Repulsion (VSEPR) theory.

Step by step solution

01

Understanding diatomic molecules

A diatomic molecule consists of two atoms bonded together. Since there are only two atoms, there is no possibility for different geometries to form. The molecule must have a linear shape, as the atoms lie directly next to each other in a straight line.
02

Lewis structures and molecular shape

To better visualize the electron configuration in diatomic molecules, we can use Lewis structures. These structures represent atoms and their valence electrons as symbols and dots, respectively. In diatomic molecules, a single bond (or double or triple bond) connects the two atoms, leading to a linear shape. Regardless of the number of valence electron pairs on each atom, the linear shape remains the same, as the structure is determined by the bonding between the two atoms.
03

Valence shell electron pair repulsion (VSEPR) theory

The VSEPR theory is used to predict the shape of a molecule based on the repulsion forces between electron pairs in the valence shell of an atom. According to this theory, electrons will arrange themselves to minimize the repulsion forces. In a diatomic molecule, there are only two atoms and one bond. Therefore, there is no possibility of varying the angles between the atoms, leading to a linear shape.
04

Summarizing why diatomic molecules are linear

In conclusion, all diatomic molecules are linear because they consist of two connected atoms, allowing for only one possible shape. This observation holds true regardless of the number of valence electron pairs on the individual atoms involved, as the bonding and repulsion forces between the atoms dictate the linear arrangement.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following molecules contain polar covalent bonds? a. phosphorus, \(P_{4}\) b. oxygen, \(\mathrm{O}_{2}\) c. ozone, \(\mathrm{O}_{3}\) d. hydrogen fluoride, HF

For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species. a. Na or \(\mathrm{Na}^{+}\) c. \(\mathrm{Mg}\) or \(\mathrm{Mg}^{2+}\) b. F or \(\mathrm{F}^{-}\) d. \(\mathrm{S}\) or \(\mathrm{S}^{2-}\)

For the indicated atom in each of the following molecules, give the number and the arrangement of the electron pairs around that atom. a. \(\mathrm{C}\) in \(\mathrm{CCl}_{4}\) b. Ge in \(\mathrm{GeH}_{4}\) c. \(\mathrm{B}\) in \(\mathrm{BF}_{3}\)

For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom. a. \(\mathrm{P}\) in \(\mathrm{PH}_{3}\) b. \(\mathrm{Cl}\) in \(\mathrm{ClO}_{4}^{-}\) c. \(\mathrm{O}\) in \(\mathrm{H}_{2} \mathrm{O}\)

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. sulfate ion, \(\mathrm{SO}_{4}^{2-}\) b. phosphate ion, \(\mathrm{PO}_{4}^{3-}\) c. sulfite ion, \(\mathrm{SO}_{3}^{2-}\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.