/*! 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 47 Give the bond order for each bon... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 47

Give the bond order for each bond in the following molecules or ions. (a) \(\mathrm{CH}_{2} \mathrm{O}\) (c) \(\mathrm{NO}_{2}^{+}\) (b) \(\mathrm{SO}_{3}^{2-}\) (d) NOCl

Short Answer

Expert verified
(a) 2; (b) 1.33; (c) 2; (d) N=O: 2, N-Cl: 1.

Step by step solution

01

Lewis Structure of Formaldehyde ( \mathrm{CH}_2\mathrm{O} )

Draw the Lewis structure for formaldehyde. Carbon forms a double bond with oxygen and single bonds with each hydrogen. The structure resembles: \( H_2C=O \).
02

Determine Bond Order in CH2O

In \( \mathrm{CH}_2\mathrm{O} \), there is one carbon-oxygen double bond. Therefore, the bond order is 2.
03

Lewis Structure of Nitronium Ion (\(\mathrm{NO}_2^+\))

Draw the Lewis structure for \( \mathrm{NO}_2^+ \). Nitrogen forms a double bond with each oxygen, and there are no lone pairs on nitrogen. The structure is linear.
04

Determine Bond Order in NO2+

In \( \mathrm{NO}_2^+ \), there are two equivalent \( \mathrm{N} = \mathrm{O} \) double bonds. The bond order is 2 for both \( \mathrm{N} = \mathrm{O} \) bonds.
05

Lewis Structure of Sulfite Ion (\(\mathrm{SO}_3^{2-}\))

Draw the Lewis structure for \( \mathrm{SO}_3^{2-} \). Sulfur is bonded to three oxygens with one double bond and two single bonds. Resonance structures indicate that each \( \mathrm{S} - \mathrm{O} \) bond is equivalent.
06

Determine Bond Order in SO32-

In \( \mathrm{SO}_3^{2-} \), average the one double and two single bonds over three bonds. The bond order is \( \frac{1+1+2}{3} = \frac{4}{3} \approx 1.33 \).
07

Lewis Structure of Nitrosyl Chloride (\(\mathrm{NOCl}\))

Draw the Lewis structure for \( \mathrm{NOCl} \). Nitrogen forms a double bond with oxygen and a single bond with chlorine.
08

Determine Bond Order in NOCl

In \( \mathrm{NOCl} \), the \( \mathrm{N} = \mathrm{O} \) bond order is 2, and the \( \mathrm{N} - \mathrm{Cl} \) bond order is 1.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lewis structures
Lewis structures are diagrams that represent the arrangement of electrons in a molecule. They help us understand the valence electrons and how atoms bond in a compound. By using dots to symbolize electrons, and lines to indicate convalent bonds, Lewis structures offer a visual representation of a molecule's atomic configuration.
To draw a Lewis structure:
  • Count the total valence electrons available from all the atoms.
  • Use lines to make single bonds between atoms.
  • Complete the octet for outer atoms, and for the central atom if applicable.
  • Apply double or triple bonds if needed to satisfy the octet rule.
These steps create a clearer picture of how atoms share electrons to form molecules.
covalent bonds
Covalent bonds are formed when two atoms share electrons to attain a full outer electron shell. This sharing allows each atom to achieve greater stability, similar to the nearest noble gas configuration. Covalent bonds are a fundamental aspect of how elements combine.
Key characteristics include:
  • Shared pairs of electrons between atoms.
  • Bond strength is influenced by the number of shared pairs (single, double, or triple bonds).
  • Covalent bonds can form between atoms of the same element or different elements.
  • Nonmetals typically form covalent bonds.
Understanding covalent bonds helps explain why certain molecules have specific shapes and properties.
chemical bonding
Chemical bonding involves the interaction between atoms that leads to the formation of molecules. It is a core concept in chemistry that explains how atoms come together. There are various types of chemical bonding, including:
  • Covalent bonds: Involves sharing of electron pairs.
  • Ionic bonds: Transfer of electrons from one atom to another.
  • Metallic bonds: Free movement of electrons within a metal lattice.
Chemical bonding shapes physical and chemical properties of molecules, such as solubility, melting point, and conductivity.
resonance structures
Resonance structures illustrate the different ways atoms can be arranged in a molecule without changing its overall connectivity. These structures highlight the delocalized movement of electrons. Key aspects of resonance include:
  • Resonance structures have the same arrangement of atoms but different distributions of electrons.
  • The true structure of a molecule is a hybrid of its resonance forms.
  • Resonance provides greater stability to a molecule, as electrons are spread over multiple atoms.
  • Commonly seen in molecules with pi bonds and lone pairs.
Understanding resonance structures enhances comprehension of molecular stability and bonding scenarios.

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

Describe the formation of KF from K and F atoms using Lewis symbols. Is bonding in KF ionic or covalent?

Draw a Lewis structure for each of the following molecules. (a) Methanol, \(\mathrm{CH}_{3} \mathrm{OH}\) (C is the central atom) (b) Vinyl chloride, \(\mathrm{H}_{2} \mathrm{C}=\mathrm{CHCl}\), the molecule from which PVC plastics are made. (c) Acrylonitrile, \(\mathrm{H}_{2} \mathrm{C}=\mathrm{CHCN}\), the molecule from which materials such as Orlon are made. (EQUATION CAN'T COPY)

Define "bond dissociation energy." Does the enthalpy change for a bond- breaking reaction [e.g., \(\mathrm{C}-\mathrm{H}(\mathrm{g}) \longrightarrow \mathrm{C}(\mathrm{g})+\mathrm{H}(\mathrm{g})]\) always have a positive sign, always have a negative sign, or vary? Explain briefly.

Consider a series of molecules in which carbon is bonded by single bonds to atoms of second-period elements: \(\mathrm{C}-\mathrm{O}, \mathrm{C}-\mathrm{F}, \mathrm{C}-\mathrm{N}, \mathrm{C}-\mathrm{C},\) and \(\mathrm{C}-\mathrm{B} .\) Place these bonds in order of increasing bond length.

Give the periodic group number and number of valence electrons for each of the following atoms. (a) \(\mathrm{C}\) (d) Si (b) \(\mathrm{Cl}\) (e) Se (c) \(\mathrm{Ne}\) (f) \(\mathrm{Al}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

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.