Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity

Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 74QAP: Consider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four...

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Consider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than 109.5? Explain your reasoning.
In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.
Methyl isocyanate, CH3NCO, was made infamous in 1984when an accidental leakage of this compound from a storagetank in Bhopal, India, resulted in the deaths of about3800 people and severe and lasting injury to many thousandsmore. (a) Draw a Lewis structure for methyl isocyanate.(b) Draw a ball-and-stick model of the structure,including estimates of all the bond angles in the compound.(c) Predict all the bond distances in the molecule.(d) Do you predict that the molecule will have a dipolemoment? Explain.
The structural formulas for ethanol, CH3CH2OH, and propene, CH;CH=CH,2, are нн H Н—С—С—0—н H-C-C=C-H нн H H H Ethanol Propene (a) Complete the Lewis structure for each molecule showing all valence electrons. (b) Using the VSEPR model, predict all bond angles in each molecule.
2. Consider the following molecules or ions: CIOF5, NOBr, NH2F, and XeO2F3+. Answer the following questions based on the Lewis structures and VSEPR theory prediction of their molecular shapes. (a) Which one has only bond angles of 109.5°? (b) Which one has only bond angles of 120°? (c) Which one has bond angles of 90 and 180°? (d) Which one has bond angles of 90, 120, and 180°?
2. Consider the following molecules or ions: H2O, SF4, IF4", and COF2. Answer the following questions based on the Lewis structures and VSEPR theory prediction of their molecular shapes. (a) Which one has only bond angles of 109.5°? (b) Which one has only bond angles of 120°? (c) Which one has bond angles of 90 and 180°? (d) Which one has bond angles of 90, 120, and 180°?
For molecule CN2 2- , give Lewis structure, Valence Shell Electron pairs, bonding electron pairs, nonbonding electron pairs, VSEPR formula, bond angle, and molecular geometry (shape).
10. Each ball-and-stick model below shows the electron-pair and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry based on the number of lone and bonding pairs around the central atom. (a) (b) (c) 11. Draw the Lewis structure for acetamide (CH3CONH2) and determine the geometry about each interior atom. Experiments show that the geometry about the N atom in acetamide is nearly planar. Draw a resonance structure that can account for the planar geometry about the N atom.
The cyanate ion is an anion consisting of one oxygen atom, one carbon atom, and onenitrogen atom, [OCN], in that order. a) Write three (3) resonance contributing structures for the cyanate ion. Show formalcharges.b) Based on your contributing structures, predict the O-C-N bond angle.
The N - N - H bond angles in hydrazine N2H4 are 112°. What is the hybridization of the nitrogen orbitals predicted by valence bond theory? How many non- bonding pairs of electrons are found on each of the N centers? How many bonding pairs of electrons are there for each N-center? Use the karet symbol (^) to indicate the superscript and answer in numeric.
SO < SO2< SO32-( a) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.)SO32- : is it 1.00, 1.33, 1.50, 2.00, 3.00 (b) Match each species with the correct formal charge on the central S atom. SO32- : is it -1.00 , -0.67 , -0.50, 0.00, +1.00, or +2.00 ? (c) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. SO32- : is it -1.00 , -0.67 , -0.50, 0.00, +1.00, or +2.00 ?
Arrange the highlighted bonds in the table below in decreasing order of polarity. That is, pick 1 for the most polar bond, pick 2 for the next most polar bond, and so on. bond polarity :F: (Choose one) (Choose one) |(Choose one)