9. Think of 3 examples, (not the same ones as ppt), ofexceptions to the octet rule and explain why they are exceptions.1.2.3.10. Draw Lewis structures for molecular oxygen and ozone(03). Use these structures to explain why one is more reactivethan the other and which will have a longer bond length. Includeresonance structures.11. Write the Lewis Structure for each molecule/ion and includeresonance structures.a. CHO₂b. SO3c. NO₁₂

Answered: 9. Think of 3 examples, (not the same…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

answer these questions from here
Draw the lewis structure with formal charges. If the lewis structure has resonance please show all possible resonance structures. 4. SO3
Determine if the structural formula below is an acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. :0: CH3 CH-C-Ö-CH–CH3 A. This is not the correct Lewis structure. B. No, All atoms do not have a zero formal charge, therefore this is not the correct Lewis structure. C. All atoms have a zero formal charge, therefore this is the correct Lewis structure. D. Oxygen has a formal charge of 1+.
and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. astered -- -- ——... Formal Charge S 01 02 03 A .0% 2- 2. The best Lewis structure for SO3²- is S :0: B :0: ....———— C
Considering the structure on the far left as the original resonance structure, which of the subsequent resonance structures (A-D) is implausible. Explain why you believe the resonance structure to be implausible.
We can draw three inequivalent Lewis structures for the arsenite ion , AsO,". The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. 3- As As. :O: :0: B Formal Charge As 01 02 03 2. The best Lewis structure for AsO is ot Submit Answer Try Another Version 2 item attempts remaining Previous Next Email Instructor Cengage Learning | Cengage Technical Support -ö: O0 0
Consider the following Lewis structure. Note, all valence electrons are shown. a. Assign formal charges to any atoms that that have a formal charge.b. Draw another Lewis structure that is a more important contributor to the actual structure than the one shown. c. Listed to the right are some typical C-N bond lengths. From the choices below, circle the best estimate for the carbon-nitrogen bond in the actual structure above. (a)1.46 A (b) 1.43 A (c) 1.26 A (d) 1.36 A (e) 1.12 A
A newly discovered element Bm has 6 valence electrons. How many total valence electrons are in the BmH2 molecule, a molecule that Bm forms with hydrogen? Draw a valid Lewis Structure for the molecule BmH2 that Bm forms with hydrogen and use the Lewis structure to determine the number of lone pairs of electrons around the central Bm atom in this molecule. What is the formal charge of Bm in BmH2? (Number and sign) What is the hybridization of Bm according to the hybrid orbital model?
Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. Molecule A: Cl 2 Molecule B: CCI 4 · Molecule C: NH 3 34. In the box provided in your answer booklet, draw the electron-dot (Lewis) structure for the NH 3 molecule. [1] 35. Explain why CCI 4 is classified as a nonpolar molecule. (1] 36. Explain why-NIshas stronger-intermolecular forces of attraction than Ct2. f} 37. Explain how the bonding in KCl is different from the bonding in molecules A, B, and C. [1]
Answer 1 2 3
1. For the compounds cited below, provide the following: A. XeF2 B. O3 (ozone) C. CH20 (formaldehyde or methanal) 1. Total valence electrons 2. Number of bonding electrons in the skeletal formula 3. Number of lone pairs 4. Number of bonding pairs to satisfy octet rule, if necessary. 5. Lewis Structure with appropriate polar arrows II. Complete the table below: NUMBER OF MOLECULE OR ION ELECTRON NUMBER OF NONBONDING GROUPS MOLECULAR SHAPE/MOLECULE GEOMETRY ELECTRON GROUP DESIGNATION/ ARRANGEMENT/ELECTRON NUMBER OF BONDING GROUPS GROUPS GEOMETRY NOTATION XeF2 O3 (ozone) CH20 (formaldehyde or methanal)
Follow the Octet rule and draw Lewis structures of the following covalent, ionic compounds and ions. (do not draw resonance structures) Please draw your Lewis diagrams in a separate paper and upload the answer sheet to the quiz- 6 submission folder. a. SO2 b. AICI4 c. H3O* d. SrO

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS