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…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 70QRT

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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?
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…
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Carbon monoxide, CO, is isoelectronic to N2. (a) Draw aLewis structure for CO that satisfies the octet rule. (b) Assumethat the diagram in Figure 9.46 can be used to describethe MOs of CO. What is the predicted bond order forCO? Is this answer in accord with the Lewis structure youdrew in part (a)? (c) Experimentally, it is found that thehighest energy electrons in CO reside in a σ-type MO. Isthat observation consistent with Figure 9.46? If not, whatmodification needs to be made to the diagram? How doesthis modification relate to Figure 9.43? (d) Would you expectthe π2p MOs of CO to have equal atomic orbital contributionsfrom the C and O atoms? If not, which atom wouldhave the greater contribution?
Draw the Lewis structures for each of the following ionsor molecules. Identify those in which the octet rule is notobeyed; state which atom in each compound does not followthe octet rule; and state, for those atoms, how manyelectrons surround these atoms: (a) PH3, (b) AlH3, (c) N3-,(d) CH2Cl2, (e) SnF62-.
Ozone (O3) has a nonzero dipole moment. In the moleculeof O3, one of the oxygen atoms is directly bonded to theother two, which are not bonded to each other.(a) Based on this information, state which of the following structures are possible for the ozone molecule:symmetric linear, nonsymmetric linear (for example,different OUO bond lengths), and bent. (Note: Evenan OUO bond can have a bond dipole if the twooxygen atoms are bonded to different atoms or if onlyone of the oxygen atoms is bonded to a third atom.)(b) Use the VSEPR theory to predict which of the structures of part (a) is observed.
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Using the bond triangle concept, state the probable combination of bonding in K3As and AsF3

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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