Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. (a) (b) (c) H- H H-C H H H H H 03 B -H

Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. (a) (b) (c) H- H H-C H H H H H 03 B -H

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.123QE

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Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. (a) (b) (c) (d) HH H
Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula. For each atom enter one of the following: tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear. (a)[ (b) (c) (d) H H C b a Si-C H XHH H Н H H
A compound composed of 2.1% H, 29.8% N, and 68.1% Ohas a molar mass of approximately 50 g>mol. (a) Whatis the molecular formula of the compound? (b) What isits Lewis structure if H is bonded to O? (c) What is the geometryof the molecule? (d) What is the hybridization ofthe orbitals around the N atom? (e) How many s and howmany p bonds are there in the molecule?
(a) Determine the molecular geometry of SeF4using the VSEPR model. The molecular geometry of SeF4 is (___________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or T-shaped or octahedral or square pyramidal or square planar . (b) Explain why the molecular geometry of SeF4 is different from that of IBr3, although they have similar electron-domain geometries. Although both SeF4 and IBr3 have the electron-domain geometry of (_________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or T-shaped or octahedral or square pyramidal or square planar, IBr3 has _____ lone pair(s) of electrons whereas SeF4 has only ________ lone electron pair(s) in the (______________) axial or equatorial positions. Accordingly, the molecular geometry of SeF4 is (________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or…
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(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?
The AF, species are shown as follows, BF;; CF4; NF3; OF2. (i) Draw the Lewis structure for each of the above AF, species. (ii) Determine the molecular geometry for each of the above AF, species. (iii) Arrange the AFn species in the order of increasing bond angle. Explain your answer. (iv) Determine the hybridisation of the central atom for BF3 and NF3 respectively.
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