Using the lewis structures and hybridized orbitals of BF3 and BF4-, briefly expain why the BF bond length in BF4- is longer than the BF bond length in BF3 Show work
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A: Step 1: Addition of ethyl in benzene ring . Step 2: Elimination of fluorine. Step 3: Step 4:
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Q: 4. Give the reagents 요 a) 1.LAH 2. MeMgBr 3. H₂O PH 1. Me Br 1. Me Ms Br b) c) 20 LAH 2. H₂O 3.H20
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- What would happen to the energy of the s1s MO if theH atoms in H2 were pulled apart to a distance twice as longas its normal bond length?4. Describe thelocation of the maximumelectron density of o- and n-bonds. How is the difference in the spatial arrangementof the electron density of these bonds reflected on their strength?The lactic acid molecule, CH3CH1OH2COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many p and howmany s bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?
- Consider the Lewis structure shown below.(a) Does the Lewis structure depict a neutral molecule or anion? If it is an ion, what is the charge on the ion? (b) What hybridizationis exhibited by each of the carbon atoms? (c) Arethere multiple equivalent resonance structures for the species?(d) How many electrons are in the p system of the species?Which of the follcwing factors does not affect bond energy? O bond polarity O orbital hybridization O formal charge loss of overlapTlatch chemtcal terminelogy vzittecorrect definitiom is a measure of the tendency of an atom to A EectronegatVIEY attrart electrone BValence electrons Is used to show the bonding beween atome of a CEone nar motecute and the Ione pairs of eloctrons that may exist in the imolecule Bond that farms hetveen izo atoms where the electrons are unoqually distributed causing the molecuile to have a 3light electrieal dioole moment is called DLewis structure ENarpolar bond Bond that formIs between we atoms where the siecttons ate oqually distributed is caltad v Valerice elaconsthat ar notsharec wtaianuther atom are caled hathe Eltons l tha Stiferim
- The VSEPR model was developed before any xenon com-pounds had been prepared. Thus, these compounds provided anexcellent test of the model’s predictive power. What would youhave predicted for the shapes of XeF₂, XeF₄, and XeF₆?“Inert” xenon actually forms several compounds, especially with the highly electronegative elements oxygen and fluorine.The simple fluorides XeF₂, XeF₄, and XeF₆ are all formed by di-rect reaction of the elements. As you might expect from the sizeof the xenon atom, the Xe-F bond is not a strong one. Calcu-late the Xe-F bond energy in XeF₆, given that the heat of for-mation is 402 kJ/mol.Suppose a particular AB3 molecule has the resonance structureDoes this structure follow the octet rule? How many electron domains are therearound the A atom?
- The four bonds of carbon tetrachloride (CCl4) are polar, butthe molecule is nonpolar because the bond polarity is canceledby the symmetric tetrahedral shape. When other atoms substitutefor some of the Cl atoms, the symmetry is broken and the mol-ecule becomes polar. Use Figure to rank the fol-lowing molecules from the least polar to the most polar: CH₂Br₂,CF₂Cl₂, CH₂F₂, CH₂Cl₂, CBr₄, CF₂Bra which of these is an odd-electron molecule? O HBr O BrO O HOBгWhen given a complete Lewis structure; then how is the level of hybridization determined for each element in the complete Lewis structure?