Examine the Lewis structure for the ammonia (NH3)molecule shown below.HN-HHWhich one of the options gives the electron andmolecular geometry (EG and MG) for this molecule?Select one:EG: Trigonal planar; MG: Trigonal planarEG: Trigonal planar; MG: BentEG: Tetrahedral; MG: TetrahedralO EG: Tetrahedral; MG: Trigonal pyramidal

Answer:Molecular formulaHybridizationElectronic geometry (EG)Molecular Geometry…

Examine the Lewis structure for the ammonia (NH3) molecule shown below. H N-H H Which one of the options gives the electron and molecular geometry (EG and MG) for this molecule? Select one: O EG: Trigonal planar; MG: Trigonal planar EG: Trigonal planar; MG: Bent EG: Tetrahedral; MG: Tetrahedral EG: Tetrahedral; MG: Trigonal pyramidal

Examine the Lewis structure for the ammonia (NH3) molecule shown below. H N-H H Which one of the options gives the electron and molecular geometry (EG and MG) for this molecule? Select one: O EG: Trigonal planar; MG: Trigonal planar EG: Trigonal planar; MG: Bent EG: Tetrahedral; MG: Tetrahedral EG: Tetrahedral; MG: Trigonal pyramidal

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 3RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6....

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Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.
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.
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How many central atoms does the molecule H2NCH3 have, and what is the shape about each?
7.50 Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with each of them, (a) CN , (b) NH4+ . (c) CO32
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Use the Molecule Shape simulator (http://openstaxcollege.org/I/6MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
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