None Using the lewis structures and hybridizedorbitals of BF3 and BF4-, briefly expainwhy the BF bond length in BF4- is longerthan the BF bond length in BF3Show work

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Answered: Using the lewis structures and…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 20CTQ

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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?
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?
Tlatch 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
Which of the follcwing factors does not affect bond energy? O bond polarity O orbital hybridization O formal charge loss of overlap
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1) Which of the following elements are capable of forming compounds in which the indicated atom can have more than 4 valence e- pairs? In each case, explain why and why not.
“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.
a which of these is an odd-electron molecule? O HBr O BrO O HOBг
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, CF₂Br
The structure of borazine, B3N3H6, is a six-membered ringof alternating B and N atoms. There is one H atom bondedto each B and to each N atom. The molecule is planar.(a) Write a Lewis structure for borazine in which the formalcharge on every atom is zero. (b) Write a Lewis structurefor borazine in which the octet rule is satisfied forevery atom. (c) What are the formal charges on the atomsin the Lewis structure from part (b)? Given the electronegativitiesof B and N, do the formal charges seem favorableor unfavorable? (d) Do either of the Lewis structuresin parts (a) and (b) have multiple resonance structures?(e) What are the hybridizations at the B and N atoms inthe Lewis structures from parts (a) and (b)? Would you expectthe molecule to be planar for both Lewis structures?(f) The six B¬N bonds in the borazine molecule are allidentical in length at 1.44 Å. Typical values for the bondlengths of B¬N single and double bonds are 1.51 Å and1.31 A°, respectively. Does the value of the B¬N…
Explain below ? The resonance hybrid is more stable than any resonance structurebecause it delocalizes electron density over a larger volume.

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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