![General Chemistry](https://www.bartleby.com/isbn_cover_images/9781891389603/9781891389603_largeCoverImage.gif)
Concept explainers
(a)
Interpretation:
The Lewis formula of
Concept Introduction:
Lewis Structure: A Lewis structure shows a covalent bond as pair of electrons shared between two atoms.
Procedure to write Lewis formulas:
- The symbols of the atoms that are bonded together in the molecule next to one another are arranged.
- The total number of valence electrons in the molecule is calculated by adding the number of valence electrons for all the atoms in the molecules. If the species is an ion, then the charge of ion into account by adding electrons, if it is a negative ion or subtracting electrons if it is a positive ion.
- A two-electron covalent bond is represented by placing a line between the atoms, which are assumed to be bonded to each other.
- The remaining valence electrons as lone pairs about each atom are arranged so that the octet rule is satisfied for each other.
Formal charge (F.C): The charges that assigned to each atom in a molecule or ion by a set of arbitrary rules and don not actually represent the actual charges on the atoms are called as formal charges.
The formal charge is calculated using the formula,
The Lewis structure with zero formal charge or least separated formal charges is the preferred structure of the molecule.
(a)
![Check Mark](/static/check-mark.png)
Explanation of Solution
The total number of valence electrons in
Number of valence electrons in oxygen=
Number of valence electrons in chlorine=
Since there is a negative charge present in ion, one electron is added.
The total number of valence electrons is thirty-two.
One chlorine atom forms four bonds with oxygen that is eight electrons are used to form bonds and the remaining twenty-four atoms are used to satisfy the octet rule of oxygen atoms.
The Lewis formula is,
The formal charge for each atom is calculated as,
Formal charge on chlorine=
Formula charge on oxygen=
The Lewis formula is,
A large charge separation can be seen in the structure, this can be avoided by adding three pi bonds between oxygen and chlorine. The chlorine atom can expand the octet rule since it belongs to period three. The final Lewis structure is,
(b)
Interpretation:
The Lewis formula of
Concept Introduction:
Refer to part (a).
(b)
![Check Mark](/static/check-mark.png)
Explanation of Solution
The total number of valence electrons in
Number of valence electrons in oxygen=
Number of valence electrons in chlorine=
The total number of valence electrons is thirteen.
One chlorine atom forms a bond with oxygen atom that is two electrons are used to form bonds and the remaining nine electrons are used to satisfy the octet rule of oxygen and chlorine atoms.
The Lewis formula is,
The formal charge for each atom is calculated as,
Formal charge on chlorine=
Formula charge on oxygen=
The Lewis formula is,
(c)
Interpretation:
The Lewis formula of
Concept Introduction:
Refer to part (a).
(c)
![Check Mark](/static/check-mark.png)
Explanation of Solution
The total number of valence electrons in
Number of valence electrons in oxygen=
Number of valence electrons in chlorine=
Since there is a negative charge present in ion, one electron is added.
The total number of valence electrons is twenty-six.
One chlorine atom forms three bonds with oxygen that is six electrons are used to form bonds and the remaining twenty atoms are used to satisfy the octet rule of oxygen atoms.
The Lewis formula is,
The formal charge for each atom is calculated as,
Formal charge on chlorine=
Formula charge on oxygen=
The Lewis formula is,
A large charge separation can be seen in the structure, this can be avoided by adding two pi bonds between oxygen and chlorine. The chlorine atom can expand the octet rule since it belongs to period three. The final Lewis structure is,
(d)
Interpretation:
The Lewis formula of
Concept Introduction:
Refer to part (a).
(d)
![Check Mark](/static/check-mark.png)
Explanation of Solution
The total number of valence electrons in
Number of valence electrons in oxygen=
Number of valence electrons in chlorine=
The total number of valence electrons is nineteen.
One chlorine atom forms two bonds with oxygen atom that is four electrons are used to form bonds and the remaining fifteen atoms are used to satisfy the octet rule of oxygen atoms.
The Lewis formula is,
The formal charge for each atom is calculated as,
Formal charge on chlorine=
Formula charge on oxygen=
The Lewis formula becomes,
A large charge separation can be removed, by adding two pi bonds between chlorine and oxygen. Since chlorine belongs to third period, it can expand the octet rule. The final Lewis structure is,
(e)
Interpretation:
The Lewis formula of
Concept Introduction:
Refer to part (a).
(e)
![Check Mark](/static/check-mark.png)
Explanation of Solution
The total number of valence electrons in
Number of valence electrons in oxygen=
Number of valence electrons in chlorine=
Since there is a negative charge present, one electron is added.
The total number of valence electrons is fourteen.
One chlorine atom forms a bond with oxygen atom that is two electrons are used to form bonds and the remaining twelve atoms are used to satisfy the octet rule of oxygen and chlorine atoms.
The Lewis formula is,
The formal charge for each atom is calculated as,
Formal charge on chlorine=
Formula charge on oxygen=
The Lewis formula is,
Want to see more full solutions like this?
Chapter 7 Solutions
General Chemistry
- In the drawing areas below, draw the two most expected stable conformations of the following molecule: ייון Be sure your drawings make it possible to distinguish between the conformations. After you've drawn the conformations, answer the question below the drawing areas. Х S : ☐ ☑ 5arrow_forwardDraw the structure of the organic reactant, and write the chemical formula of the reagent used to form the given product. Click and drag to start drawing a structure. + T ☑ OH NO₂ NO2arrow_forwardNonearrow_forward
- Safari File Edit View History Bookmarks Window Help く < mylabmastering.pearson.com Wed Feb 12 8:44 PM ✩ + Apple Q Bing Google SignOutOptions M Question 36 - Lab HW BI... P Pearson MyLab and Mast... P Course Home Error | bartleby b Answered: If the biosynth... Draw a free-radical mechanism for the following reaction, forming the major monobromination product: ScreenPal - 2022 CHEM2... Access Pearson 2 CH3 Br-Br CH H3 Draw all missing reactants and/or products in the appropriate boxes by placing atoms on the canvas and connecting them with bonds. Add charges where needed. Electron- flow arrows should start on the electron(s) of an atom or a bond and should end on an atom, bond, or location where a new bond should be created. Include all free radicals by right-clicking on an atom on the canvas and then using the Atom properties to select the monovalent radical. ▸ View Available Hint(s) 0 2 DE [1] H EXP. CONT. H. Br-Br H FEB 12arrow_forwardPlease correct answer and don't use hand ratingarrow_forwardNonearrow_forwardQ1: For each molecule, assign each stereocenter as R or S. Circle the meso compounds. Label each compound as chiral or achiral. + CI Br : Н OH H wo་ཡིག་ཐrow HO 3 D ။။ဂ CI Br H, CI Br Br H₂N OMe R IN I I N S H Br ជ័យ CI CI D OHarrow_forwardPlease correct answer and don't use hand ratingarrow_forwardNonearrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)