CHEMISTRY >CUSTOM<
CHEMISTRY >CUSTOM<
8th Edition
ISBN: 9781309097182
Author: SILBERBERG
Publisher: MCG/CREATE
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 10, Problem 10.17P

(a)

Interpretation Introduction

Interpretation:

Lewis structure for a resonance form of each ion of BrO3 with the lowest possible formal charges is to be drawn. Also, the oxidation number of the atom is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

Formula to calculate the formal charge of the atom is as follows:

  Formalcharge=(numberofvalenceelectrons)((numberofnon-bondingelectrons)+(12)(numberofbondingelectrons))        (1)

The formula to calculate the oxidation number of an atom is as follows:

  Oxidationnumber=(numberofvalenceelectrons)((numberofnon-bondingelectrons)+(numberofbondingelectrons))        (2)

(a)

Expert Solution
Check Mark

Answer to Problem 10.17P

The possible Lewis structures for a resonance form of each ion of BrO3 with the lowest possible formal charges are,

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  1

The oxidation numbers of Br is +5 and the oxidation number of oxygen is 2.

Explanation of Solution

Lewis structures for a resonance form of BrO3 is,

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  2

For structure I:

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  3

Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 6 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.

  Formalcharge=(7)((2)+(12)(6))=+2

Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each oxygen atom.

  Formalcharge=(6)((6)+(12)(2))=1

For structure II:

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  4

Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 8 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.

  Formalcharge=(7)((2)+(12)(8))=+1

Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.

  Formalcharge=(6)((6)+(12)(2))=1

Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on the double bonded oxygen atom.

  Formalcharge=(6)((4)+(12)(4))=0

For structure III:

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  5

Substitute 7 for valence electrons, 2 for the number of nonbonded electrons and 10 for the number of bonding electrons in equation (1) to calculate the formal charge on Br atom.

  Formalcharge=(7)((2)+(12)(10))=0

Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for number of bonding electrons in equation (1) to calculate the formal charge on the single bonded oxygen atom.

  Formalcharge=(6)((6)+(12)(2))=1

Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on each double bonded oxygen atom.

  Formalcharge=(6)((4)+(12)(4))=0.

Therefore, structure II has the more acceptable and reasonable distribution of formal charges.

The oxidation numbers of Br is +5 and the oxidation number of oxygen is 2.

Conclusion

BrO3 has three possible resonating structures. Structure II is more acceptable and has a more distributed formal charge.

(b)

Interpretation Introduction

Interpretation:

Lewis structure for a resonance form of each ion of SO32 with the lowest possible formal charges is to be drawn. Also, the oxidation number of the atom is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

Formula to calculate the formal charge of the atom is as follows:

  Formalcharge=(numberofvalenceelectrons)((numberofnon-bondingelectrons)+(12)(numberofbondingelectrons))        (1)

The formula to calculate the oxidation number of an atom is as follows:

  Oxidationnumber=(numberofvalenceelectrons)((numberofnon-bondingelectrons)+(numberofbondingelectrons))        (2)

(b)

Expert Solution
Check Mark

Answer to Problem 10.17P

The possible Lewis structures for a resonance form of each ion of SO32 with the lowest possible formal charges are,

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  6

The oxidation numbers of. S is +4 and the oxidation number of oxygen is 2.

Explanation of Solution

Lewis structure for a resonance form of SO32 is,

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  7

For structure I:

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  8

Substitute 6 for valence electrons, 2 for the number of nonbonded electrons and 6 for the number of bonding electrons in equation (1) to calculate the formal charge on S atom.

  Formalcharge=(6)((2)+(12)(6))=+1

Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each oxygen atom.

  Formalcharge=(6)((6)+(12)(2))=1

For structure II:

CHEMISTRY >CUSTOM<                     , Chapter 10, Problem 10.17P , additional homework tip  9

Substitute 6 for valence electrons, 2 for the number of nonbonded electrons and 8 for the number of bonding electrons in equation (1) to calculate the formal charge on S atom.

  Formalcharge=(6)((2)+(12)(8))=0

Substitute 6 for valence electrons, 6 for nonbonded electrons and 2 for the number of bonding electrons in equation (1) to calculate the formal charge on each single bonded oxygen atom.

  Formalcharge=(6)((6)+(12)(2))=1

Substitute 6 for the value of valence electrons, 4 for the number of nonbonded electrons and 4 for the number of bonding electrons in equation (1) to calculate the formal charge on the double bonded oxygen atom.

  Formalcharge=(6)((4)+(12)(4))=0.

Therefore, structure II has the more acceptable and reasonable distribution of formal charges.

The oxidation numbers of. S is +4 and the oxidation number of oxygen is 2.

Conclusion

SO32 has two possible resonating structures.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 10 Solutions

CHEMISTRY >CUSTOM<

Ch. 10.2 - Prob. 10.6AFPCh. 10.2 - Prob. 10.6BFPCh. 10.2 - Prob. 10.7AFPCh. 10.2 - Prob. 10.7BFPCh. 10.2 - Prob. 10.8AFPCh. 10.2 - Prob. 10.8BFPCh. 10.3 - Prob. 10.9AFPCh. 10.3 - Prob. 10.9BFPCh. 10.3 - Prob. B10.1PCh. 10.3 - Prob. B10.2PCh. 10 - Prob. 10.1PCh. 10 - When is a resonance hybrid needed to adequately...Ch. 10 - Prob. 10.3PCh. 10 - Prob. 10.4PCh. 10 - Draw a Lewis structure for (a) SiF4; (b) SeCl2;...Ch. 10 - Draw a Lewis structure for (a) ; (b) C2F4; (c)...Ch. 10 - Prob. 10.7PCh. 10 - Prob. 10.8PCh. 10 - Prob. 10.9PCh. 10 - Draw Lewis structures of all the important...Ch. 10 - Prob. 10.11PCh. 10 - Draw Lewis structures of all the important...Ch. 10 - Prob. 10.13PCh. 10 - Prob. 10.14PCh. 10 - Draw the Lewis structure with lowest formal...Ch. 10 - Draw the Lewis structure with lowest formal...Ch. 10 - Prob. 10.17PCh. 10 - Prob. 10.18PCh. 10 - Prob. 10.19PCh. 10 - Prob. 10.20PCh. 10 - These species do not obey the octet rule. Draw a...Ch. 10 - These species do not obey the octet rule. Draw a...Ch. 10 - Molten beryllium chloride reacts with chloride ion...Ch. 10 - Prob. 10.24PCh. 10 - Prob. 10.25PCh. 10 - Phosgene is a colorless, highly toxic gas that was...Ch. 10 - If you know the formula of a molecule or ion, what...Ch. 10 - In what situation is the name of the molecular...Ch. 10 - Prob. 10.29PCh. 10 - Prob. 10.30PCh. 10 - Consider the following molecular shapes. (a) Which...Ch. 10 - Use wedge-bond perspective drawings (if necessary)...Ch. 10 - Prob. 10.33PCh. 10 - Determine the electron-group arrangement,...Ch. 10 - Determine the electron-group arrangement,...Ch. 10 - Prob. 10.36PCh. 10 - Prob. 10.37PCh. 10 - Prob. 10.38PCh. 10 - Prob. 10.39PCh. 10 - Determine the shape, ideal bond angle(s), and the...Ch. 10 - Prob. 10.41PCh. 10 - Determine the shape around each central atom in...Ch. 10 - Prob. 10.43PCh. 10 - Prob. 10.44PCh. 10 - Prob. 10.45PCh. 10 - Prob. 10.46PCh. 10 - Arrange the following ACln species in order of...Ch. 10 - State an ideal value for each of the bond angles...Ch. 10 - Prob. 10.49PCh. 10 - Prob. 10.50PCh. 10 - Prob. 10.51PCh. 10 - Prob. 10.52PCh. 10 - How can a molecule with polar covalent bonds not...Ch. 10 - Prob. 10.54PCh. 10 - Consider the molecules SCl2, F2, CS2, CF4, and...Ch. 10 - Consider the molecules BF3, PF3, BrF3, SF4, and...Ch. 10 - Prob. 10.57PCh. 10 - Prob. 10.58PCh. 10 - Prob. 10.59PCh. 10 - Prob. 10.60PCh. 10 - Prob. 10.61PCh. 10 - Prob. 10.62PCh. 10 - Prob. 10.63PCh. 10 - Prob. 10.64PCh. 10 - Prob. 10.65PCh. 10 - Prob. 10.66PCh. 10 - When SO3 gains two electrons, forms. (a) Which...Ch. 10 - The actual bond angle in NO2 is 134.3°, and in it...Ch. 10 - Prob. 10.69PCh. 10 - Propylene oxide is used to make many products,...Ch. 10 - Prob. 10.71PCh. 10 - Prob. 10.72PCh. 10 - Prob. 10.73PCh. 10 - Prob. 10.74PCh. 10 - Prob. 10.75PCh. 10 - Prob. 10.76PCh. 10 - Prob. 10.77PCh. 10 - A gaseous compound has a composition by mass of...Ch. 10 - Prob. 10.79PCh. 10 - Prob. 10.80PCh. 10 - Prob. 10.81PCh. 10 - Prob. 10.82PCh. 10 - Pure HN3 (atom sequence HNNN) is explosive. In...Ch. 10 - Prob. 10.84PCh. 10 - Prob. 10.85PCh. 10 - Oxalic acid (H2C2O4) is found in toxic...Ch. 10 - Prob. 10.87PCh. 10 - Hydrazine (N2H4) is used as a rocket fuel because...Ch. 10 - Prob. 10.89PCh. 10 - Prob. 10.90PCh. 10 - Prob. 10.91PCh. 10 - Consider the following molecular shapes: Match...Ch. 10 - Prob. 10.93PCh. 10 - Prob. 10.94PCh. 10 - Prob. 10.95PCh. 10 - Phosphorus pentachloride, a key industrial...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY