Concept explainers
Interpretation: The description of pi bonds should be matched for arrow 1, 2, and 3.
Concept introduction: Lewis structure is a representation of molecules in which dots are shown to represent unshared electrons and lines are shown to represent bonds. These lines and dots represent distribution of electrons in the molecule.
When one single structure is unable to describe all the properties of a single-molecule, a phenomenon called resonance comes into play. This arises when two or more than two Lewis structures are possible for one molecule. All such structures are called resonating structures and have same placement of atoms in them but these have different locations of bond pairs and lone pairs. The resonating structures are inter-convertible with each other. The resultant of all the resonating or contributing structures is called the resonance hybrid.
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Organic Chemistry: A Guided Inquiry
- Consider this Lewis structure in the curved arrows joke. Draw the resident structure obtained by moving electrons as indicated by the curved arrows.arrow_forwardGive correct detailed Solution with explanation needed of all options..don't give Handwritten answer .don't use Ai for answering thisarrow_forwardCan you explain why these Lewis Structures are wrong? I was told I was correct that BrF5 has 42 valence electrons, 10 bonding electrons, and 32 non bonding electrons, with 5 single bonds, and that O=CN- has 16 valence electrons, 8 bonding electrons, and 8 non bonding electrons, with 2 double bonds.arrow_forward
- In 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_forwardWould you help me, please? I struggled with my homeworkarrow_forwardWhich 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_forward
- Give 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_forward3. (a) Draw a resonance structure for Molecule 1 in Box B, which satisfies the octet for all non- hydrogen atoms. Hint you may want to use curved arrows to move electrons over the skeleton of Molecule 3 to help you find the resonance structure. H H H H Molecule 1 H H 3. (b) Fill in the table below for Molecule 1 Box B: Resonance Structure of Molecule 1 VSEPR electron pair geometry around atom Molecular geometry Approximate bond or shape around atom angles around atom N atom CH3 C atom CH C atoms 3. (c) Given the information that resonating electrons are delocalized and so are not used to determine VSEPR geometry, how will the table you filled in for 3.(b) change?arrow_forwardI would like to you help me with my homework because I struggled with step 6. Can you help me with step 6, please?arrow_forward
- Directions: 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_forwardAdd the appropriate curved arrows for bond formation /bond breakage. Show all nonbonding electrons. show assumed hydrogensarrow_forwardBoth individual bonds and whole molecules can be polar or non-polar. First, (i) explain what causes a bond (not a molecule) to be polar. Then, (ii) explain how a molecule can itself be non-polar even if it contains polar bonds. Finally, for each molecule in problem 2 above, (iii) state whether the molecule is polar or non-polar.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning