Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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- Write Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, NH2 (b) Bicarbonate ion, HCO3 (c) Carbonate ion, CO32 (d) Nitrate ion, NO3 (e) Formate ion, HCOO (f) Acetate ion, CH3COOarrow_forwardCarbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).arrow_forwardConsider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forward
- Unshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs.Use the structural formulas below to determine the number of unshared pairs at each designated atom.Be sure your answers are consistent with the formal charges on the formulas.arrow_forwardUnshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs.Use the structural formulas below to determine the number of unshared pairs at each designated atom.Be sure your answers are consistent with the formal charges on the formulas.arrow_forwardComplete the Lewis structure of N4O by adding the missing bonds, lone pairs, and non-zero formal charges. Draw the structure that has the minimal formal charges. Cº NNN- -N- HUZ OS FAJ - Н с N P CI Br Iarrow_forward
- The following is a skeleton of a molecular anion having the overall formula C7H6NO–. The H atoms are not shown. Starting with the structure drawn below, complete the Lewis structure by adding all H atoms, valence electrons, and π bonds. This structure will have a –1 formal charge on the oxygen.arrow_forwardFor each of the following, draw resonance structures, assign formal charges to the atoms in each structure, and determine relative contributions of each structure to the overall electronic structure. a) CIO2 b) CI3POarrow_forwardP3- ion is a linear ion composed of 3 phosphorus atoms. Draw 3 resonance structures of this ion. Show the individual formal charges of all atoms. Indicate which structure is the best one.arrow_forward
- An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of zero. H Н—N—С- -о—с—Н H H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges. Click and drag to start drawing a structure.arrow_forwardDraw two different Lewis structures for ClO3-, one which all atoms follow the octet rule and one where the chlorine has an expanded octet. Determine the formal charge on all atoms for each structure. Which do you think is the better Lewis structure? Explain your reasoning.arrow_forwardUnshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. CH3 CH₂ CH3 a H₂C C-C C The number of unshared pairs at atom a is | The number of unshared pairs at atom b is The number of unshared pairs at atom c is | -H The number of unshared pairs at atom a is The number of unshared pairs at atom b is The number of unshared pairs at atom c is | Submit Answer Retry Entire Group 1 more group attempt remainingarrow_forward
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