None Se=öClick to edit moleculeDraw the Lewis structure of SeO: (by following the octet rule on all atoms) andthen determine the ideal bonding angle(s) of the central atom.Give detailed Solutionwith explanation neededwith structure, avoidhandwritten SolutionA109.5°B180°C120°D60°E30°

Step 1: VSEPR tableFormulaHybridizationIdeal bond…

Answered: Se =ö Click to edit molecule Draw the…

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 114QRT

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The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.
7.84 Which of the following molecules is least likely to actually exist OF4,SF4,SeF4 , or TeF4 ? Why?
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
Assign formal charges to all atoms in the following Lewis diagrams. (a) SO42 (b) S2O32 (c) SbF3 (d) SCN
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-.
Some chemists believe that satisfaction of the octet ruleshould be the top criterion for choosing the dominant Lewisstructure of a molecule or ion. Other chemists believe thatachieving the best formal charges should be the top criterion.Consider the dihydrogen phosphate ion, H2PO4-, inwhich the H atoms are bonded to O atoms. (a) What is thepredicted dominant Lewis structure if satisfying the octetrule is the top criterion? (b) What is the predicted dominantLewis structure if achieving the best formal charges is the topcriterion?
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…
Consider the Lewis structure for the polyatomic oxyanionshown here, where X is an element from the third period(Na - Ar). By changing the overall charge, n, from 1- to2- to 3- we get three different polyatomic ions. For each ofthese ions (a) identify the central atom, X; (b) determine theformal charge of the central atom, X; (c) draw a Lewis structurethat makes the formal charge on the central atom equalto zero.
(a) State whether or not the bonding in each substance islikely to be covalent: (i) iron, (ii) sodium chloride, (iii) water,(iv) oxygen, (v) argon. (b) A substance XY, formed from twodifferent elements, boils at -33 °C. Is XY likely to be a covalentor an ionic substance?
Sulfuric acid is prepared by oxidizing sulfur to sulfur dioxide and then to sulfur trioxide. Although sulfur trioxide reacts with water to form sulfuric acid it forms a mist of find droplets of H2 S04 with water vapor that is hard to condense. Instead sulfur trioxide is first dissolved in 98% sulfuric acid to form oleum. On treatment with water concentrated sulfuric acid can be generated. Write equations for all the steps and draw Lewis structures of sulfuric acid and oleum.
Three main group elements, X, Y and Z, from three different groups inthe Periodic Table, each form a neutral trifluoride, i.e. XF3, YF3 andZF3. (a) To which three groups of the Periodic Table could the elementsX, Y and Z belong? Are any of these atoms X, Y or Zhypervalent in the trifluorides formed? (b) Use VSEPR theory to deduce the shapes of the molecules XF3,YF3 and ZF3, showing full working, and sketch these shapes (c) Only two of the three trifluorides have a non-zero dipole moment.For these molecules to which groups of the Periodic Table do thecentral atoms belong?
(a) Using the electronegativities of Br and Cl, estimate thepartial charges on the atoms in the Br¬Cl molecule. (b) Usingthese partial charges and the atomic radii given in Figure7.8, estimate the dipole moment of the molecule. (c) Themeasured dipole moment of BrCl is 0.57 D. If you assume thebond length in BrCl is the sum of the atomic radii, what arethe partial charges on the atoms in BrCl using the experimentaldipole moment?

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