Concept explainers
Interpretation:
All valid resonance structures or diazomethane are to be drawn. It is to be determined which of these resonance structures contribute more to the resonance hybrid.
Concept introduction:
Resonance hybrid is the weighted average of all the resonance structures of a molecule or ion. The contribution of different resonance structures is not equal. More stable structures contribute more to the hybrid than less stable structures. Stability of a resonance structure depends on the number of bonds between each pair of atoms as well as the presence of any formal charge. Higher the total bond energy of a structure, more stable it is. A structure with no formal charges is most stable. As the number of atoms with formal charges increases, the stability of the structure decreases.
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- Diazomethane (CH2N2) is an important reagent for the methylation of some organic molecules. Complete Parts 1 and 2 below about this unique reagent. Draw the Lewis structure of diazomethane (CH2N2) that contains a formal charge on carbon and nitrogen. Be sure to include all lone pairs of electrons and formal charges.arrow_forwardIn the following Lewis structure of [(CH3)2OH]+, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). H H-C-O-C-H HHH - H I Η Η Η 0 0 + 2+ 2-arrow_forwardGive typed full explanation Look at figure 3-22 that shows the electron density that occurs abound the Si-O bond. This electron density map gives the "shape" of the O and Si atoms when they are bonded together. Think about the answer in Q9 and choose the best response below: (Select answer choice) a. This figure shows that the Si and O atoms, when they bond together, do not form spheres, which is due to the fact that the Si-O bond is strongly covalent and these shared electrons affect atomic shape. This change in shape limits the applicability of Pauling's Coordination principle since that principle is based on the geometry of perfect spheres. b. This figure shows that the Si and O atoms, when they bond together are close to perfect spheres, which is due to the fact that the Si-O bond is strongly covalent. This figure shows that Pauling's Coordination principle should apply very precisely to any substance that contains Si-O bonds c. This figure shows that the Si and O atoms, form in a…arrow_forward
- The structure at the right is a skeleton of an anion having the overall formula C6H,NO¯. The hydrogen atoms are not shown. (a) Draw a complete Lewis structure in which the -1 formal charge is on N. Include all H atoms and C. valence electrons. (b) Do the same for a Lewis structure with the -1 formal charge on O. (c) Do the same for a Lewis structure with the -1 formal charge on the C atom that is bonded to three other C atoms.arrow_forwardIn the following Lewis structure of [(CH3)2OH]*, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). H. H-C Н-С-О-С-Н C-H H HH 2- II 2-arrow_forwardClear 0 - s - O | A Lewis structure of SO2 is shown. - so, has one other resonance structure that does not violate the octet rule. A partically completed resonance structure of this molecule is shown. Complete the other resonance structure by dragging bonds and lone electron pairs to their appropriate positions. When complete, click Check.arrow_forward
- P2.9: Draw two different (minor) resonance contributors of the structure below (the flavin group of flavin adenine dinucleotide (FAD), a biochemical oxidation/reduction molecule) in which the oxygen indicated by an arrow bears a negative formal charge and one of the circled atoms bears a positive formal charge. Include curved arrows to account for the changing positions of electrons and pi bonds. R N Dolgt `N´ FAD H3C H3C Harrow_forward4) (a) For the following structure, using curved arOWs draw all resonance contributors (only those with an octet of electrons on all non-hydrogen atoms). Be sure to show all lone pairs and non-zero formal charge(s) where applicable. CH HC CH, CH2arrow_forwardDraw the Lewis dot structure of the conjugate base of cyclopentane by assuming all the atoms in the molecule obey the octet rule. Show all lone pairs and formal charges. Do no draw resonance structures.arrow_forward
- Which of the highlighted chemical bonds in the molecules below is longest? Shortest? In between? Which highlighted bond requires the highest energy to break? Lowest? In between? Answer these questions by completing the second and third columns in the table. compound H HICIO | H :C=0: :0: || H-C-H H length of highlighted bond choose one choose one - V choose one - ✓ energy of highlighted bond choose one choose one choose one X Śarrow_forwardDirections: Complete the data table below. It is not necessary to construct any models. Number of bonds & number of lone pairs around central atom Chemical Valence electrons name Formula Lewis structure NCI, N-5 3 bonds Nitrogen CI- 7(3) 20 lone pairs trichloride Si-4 S-6(2) Sis, Silicon disulfide Н-1 C- 4 HCN N-5 C-4 CF,CI, F-7(2) CI-7(2) Ge-4 Germane GeH, H-1(4) C-4 CSF, S-6 F-7(2) Selenium Se-6 dichloride SeCl, CI-7(2) AsF, As-5 F-7(3) arsenic trifluoride C-4(2) Br-7(2) Dibromoacetylene chlorine gas Cl: CI-7(2) dihydrogen monoxide DHMO CH,O C-4 H-1(2) O-6 carbon CF, C-4 tetrafluoride F-7(4)arrow_forwardIn the following compound, identify all carbon atoms that you expect will be different in electron density. Drag the appropriate partial charges to these carbon atoms. S+ ..arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning