Given the below compounds, draw the appropriate Lewis structure, calculate the formal charge oneach atom, indicate the VSEPR notation, determine the electron and molecular geometry usingVSEPR theory, identify the hybridization of all interior atom(s), and make a sketch of the moleculebased on the valence bond theory.a) OSBr2b) SCl4c) CH3OH

Step 1: Step 2: Step 3: Step 4:

Answered: Given the below compounds, draw the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1. Briefly explain in your own words why the bond angle increases as the number of electron groups decrease? 2. How does electron domain geometry differ from molecular geometry? Briefly explain in your own words. 3. Write a complete list of steps you will utilize to predict the electron-domain geometry for a given species using only the Lewis structure. The only information you are provided with is the molecular formula and the net charge.
Choose the answer which gives the electron-domain geometry and molecular geometry which are both correct for NH2Cl (central N) . a) The electron-domain geometry is tetrahedral. The molecular geometry is T-shaped.b) The electron-domain geometry is trigonal planar. The molecular geometry is T-shaped.c) The electron-domain geometry is tetrahedral. The molecular geometry is trigonal pyramidal.d) The electron-domain geometry is trigonal planar. The molecular geometry is trigonal planar.e) The electron-domain geometry is tetrahedral. The molecular geometry is trigonal planar.
What molecules have trigonal planar ELECTRON PAIR GEOMETRY A) O3 B) HCl C) ClO3- D)NaCl E)CH2O F) BF3 G) BrF3
which of the following is an advantage of valence bond theory over lewis structures? gives information about bond length gives information about bond strength uses electrons in orbitals or all the above
1. a) Draw the dominant Lewis structure for the allene molecule (1,2-propyl diene, CH2CCH2 ) and use VSEPR theory to determine the molecule's geometry. In specifying the geometry give all bond angles and specify which nuclei lie in the same plane. b) Propose a hybridization and bonding scheme for the atoms in allene. That is, specify how each of the atoms is hybridized, which atomic orbitals overlap to form bonding molecular orbitals, and the nature (i.e., sigma", pi, etc.) of these molecular orbitals. c) Draw a plausible valence molecular orbital level diagram for allene (include only bonding MOs) based on the results from (b). d) Based on the work from (c) deduce the valence electronic configuration of the ground state of allene. e) Is the molecule planar or nonplanar? Explain your answer Answer subparts c, d, and e
What are the angles a and b in the actual molecule of which this is a Lewis structure? H H H C H a a = C b = ⁰ C H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. H X
Examine the model structures for PCl5and BrF5. Both molecules have five atoms attached to the central atom but different bond angles. Explain this difference.
2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.
ASK YOUR TEACHER Choose the answer which gives the electron-domain geometry and molecular geometry which are both correct for NH2Cl (central N) . a) The electron-domain geometry is tetrahedral. The molecular geometry is T-shaped. b) The electron-domain geometry is trigonal planar. The molecular geometry is T-shaped. c) The electron-domain geometry is tetrahedral. The molecular geometry is trigonal pyramidal. d) The electron-domain geometry is trigonal planar. The molecular geometry is trigonal planar. e) The electron-domain geometry is tetrahedral. The molecular geometry is trigonal planar.
Examine the model and real structures for ClF3. Why are the lone pairs in this molecule located in equatorial positions rather than axial positions?
Indicate which orbitals overlap to form the sigma bonds in each molecule. a) BeBr₂ b) HgCl₂ c) ICN
Choose the correct word(s) in the dropdown menu to correctly complete the statements: In the VSEPR bonding theory, electrons are delocalized on or between the bonding atoms. Valence bonding theory (VBT) theorizes that electrons in a sigma bond are shared [Select ] the internuclear axis. In molecular orbital theory (MOT) electrons are [Select ] in molecular orbitals.

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