Concept explainers
(a)
Interpretation:
The structure of
Concept Introduction:
Valence Shell Electron Pair Repulsion model predicts shape by inclusion of bond angles and most distant arrangement of atoms that leads to minimum repulsion.
For molecules that have lone pairs around central atom, lone pairs influence shape, because there are no atoms at the positions occupied by these lone pairs. The key rule that governs the molecular shape, in this case, is the extent of lone –lone pair repulsions are far greater than lone bond pair or bond pair-bond pair repulsions. The table that summarizes the molecular shapes possible for various combinations of bonded and lone pairs is given as follows:
(b)
Interpretation:
The structure of
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemical Principles: The Quest for Insight
- 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.arrow_forwardWhich of these molecules have an odd number of valence electrons: NO2, SCl2, NH3, NO3?arrow_forwardFollowing are the structures of three isomers of difluorobenzene, C6H4F2. Are any of them nonpolar?arrow_forward
- It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardA compound of chlorine and fluorine, CIFx, reacts at about 75C with uranium to produce uranium hexafluoride and chlorine fluoride, CIF. A certain amount of uranium produced 5.63 g of uranium hexafluoride and 457 mL of chlorine fluoride at 75C and 3.00 atm. What is x? Describe the geometry, polarity, and bond angles of the compound and the hybridization of chlorine. How many sigma and pi bonds are there?arrow_forwardIf you have three electron regions around a central atom, how can you have a triangular planar molecule? An angular molecule? What bond angles are predicted in each case?arrow_forward
- • identify sigma and pi bonds in a molecule and explain the difference between them.arrow_forwardConstruct the bond-line structure of C5H7ClO.arrow_forwardConsider cyclooctatetraene,C8H8, which has the octagonal structure shown belowWhat experiments or calculations could you perform to determinewhether cyclooctatetraene exhibits resonance?arrow_forward
- Draw the molecular shapes and predict the bond angles (relative to the ideal angles) of (a) SbF5 and (b) BrF5.arrow_forwardDescribe the bonding in pyridine, C5H5N, using hybrid orbitals.arrow_forwardDescribe the electron-pair geomtery and molecular geomtery around the central atom in GeBr3-arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning