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- 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 ŚChoose the letter of tye correct answer. If the answer is not found on the choices, write letter E and identify the correct answer.KCl Express your answer as an ion.
- dicting the mts of pure Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. chemical symbol, chemical formula or Lewis structure substance boiling point н :0: A H-C-C-F: (Choose one) E H B F2 (Choose one) e H H-C-F: (Choose one)e H H:0: (Choose one) B D. H C-C -0-H H. Explanation Check O2022 McGraw Hill LLC. Al Rights Reserved. Terms of Use I Privacy Center Accessibility DII V12 S0 F9 F10 F7 FB esc F4 F5 F2 F3 & @ #3 2$ %3D 8Total Valence Electrons: Hydrocyanic acid Val E. = - ½ BE = -NBE = FC = НCN Remaining Electrons: Val E. = - ½ BE = - NBE = FC = Resonance Structures? How many?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…
- What is delocalization energy? How is it related to resonance energy? Answer by selecting all true statements. 00 Resonance energy is a term used in VB theory. Resonance energy and delocalization energy are term that describe different conditions. Resonance energy is a term used in MO theory. Resonance energy and delocalization energy are essentially the same thing. Resonance energy and delocalization energy represent the additional stability associated with a spreading out of electron density. Delocalization energy is a term used in VB theory. Delocalization energy is a term used in MO theory. Resonance energy and delocalization energy represent the additional stability associated with concentrating electron density.b Draw the additional resonance structure(s) of the structure below? H3C-N+ Include all valence lone pairs in your answer. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. Separate resonance structures using the → symbol from the drop-down menu. ● ? Ⓡ ChemDoodle Sn [FCalculate Kb for each of the following ions: CN-, F-, CH3COO-, HCO3
- I got this marked wrong on an assignment, but I'm not sure why. Please help me find the correct resonance structure.Which of the following choices depicts the correct resonance arrows to show the conversion between the Q resonance form to the R resonance form?1. They result in less electron-electron repulsion because the electrons in a lone pair are more localized. They result in greater electron-electron repulsion because the electrons in a lone pair are less localized. They result in less electron-electron repulsion because the electrons in a lone pair are more localized. They result in greater electron-electron repulsion because the electrons in a lone pair are more localized. They result in less electron-electron repulsion because the electrons in a lone pair are less localized. 2. Compounds following the general formula C, H2n-2 are considered because Saturated, each carbon is bonded to exactly four hydrogen atoms. Saturated, each carbon is bonded to exactly four atoms. Unsaturated, each carbon is bonded to exactly four hydrogen atoms. Unsaturated, each carbon is bonded to exactly four atoms.
