1. Consider the structure of aspartic acid, an essential amino acid. Using VSEPR theory, determine the molecular geometry around each interior atom (7 total). Remember that a dark wedge indicate the bond is coming out of the plain of the page (towards you) and that dashes means that the bond is going behind the plane of the page (away from you). 01 geometry: C2 geometry: C3 geometry: H. JIU, A NH H 4 :0:

1. Consider the structure of aspartic acid, an essential amino acid. Using VSEPR theory, determine the molecular geometry around each interior atom (7 total). Remember that a dark wedge indicate the bond is coming out of the plain of the page (towards you) and that dashes means that the bond is going behind the plane of the page (away from you). 01 geometry: C2 geometry: C3 geometry: H. JIU, A NH H 4 :0:

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 10.50QE

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A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment. (a) HCN (b) I2 (c) NO
Which of these molecules has a net dipole moment? For each of the polar molecules, indicate the direction of the dipole in the molecule. (a) nitrosyl fluoride, FNO (b) disulfur difluoride, S2F2
Use the VSEPR model to predict the bond angles around each central atom in the following Lewis structures (benzene rings are frequently pictured as hexagons, without the letter for the carbon atom at each vertex). Note that the drawings do not necessarily depict the bond angles correctly.
) Bean hexene is an odor compound used in cosmetics and cleaners. It is also known as leguminal. Its formula is: CH3CH2CHCHCH2CH2OCHCH2CH3 | OCH3 Please draw a Lewis structure for this compound with CORRECT GEOMETRY (use dashes and wedges!) Label all pi bonds in the molecule (if there are any) Indicate the bond angles for the red highlighted section of the molecule. (hint: you may want to keep the main carbon chain in-plane with the page for clarity) For this question, you don’t need to draw out the orbitals.
Why is it less clear to see the electrons on HBrO2 molecular electron geometry than it is on something like H2O? I know there should be 20 electrons on HBrO2, but this leads me to an incorrect drawing. And with the correct drawing, I don't see where all the electrons are. It seems like there's only 10 total. What am I missing here?
Name 5 common organic compounds that are found in your home. Draw their Lewis structures and give their molecular formula. Encircle and identify the functional group/s that is/ are present in each molecule. Write your answers in another sheet of paper. Ex. Acetic acid in vinegar Substance Molecular formula Lewis structure CH,COOH - more preferable H-C+C 0-H Acetic acid C2H4O2 in vinegar H Carboxylic acid エーO-エ

Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CH3CH20H) give the structure around the bold atom. Molecule ЕPG Hyb (circle if 2D Lewis Structure 3D Lewis Structure MG polar) ВА CH2S GeO2 CF4
Although models cannot show this simply, for molecules like NF3 (whose Lewis structure you drew on the previous page), the actual bond angles may not exactly equal the angles predicted by VSEPR theory. For example, the F-N-F bond angles in NF3 are less than the 109.5° tetrahedral angle. Why do you think this might be so? 2.
Answer the questions in the table below about the shape of the methanone (H₂CO) molecule. How many electron groups are around the central carbon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central carbon atom? (You may need to use the scrollbar to see all the choices.) (choose one) X S
Table 2: Complete this table with your partner. You may ask the instructor to check your work. Formula Lewis structure Molecular geometry around central atoms(s) and name Polar or nonpolar, Draw dipole arrow Hybridization of each atom Orbitals involved in each bond XeCl2 CIF CH;CN SEF3 SF,Cl2 of each atom y dipole arrow
1. Draw the Lewis dot structure for HCOOH. (Hint: make the atom atom connectivity H-C-O-H, put in extra O on C) Based on your structure answer the following questions around the C. what is the electronic geometry? what is the molecular geometry? 2. Draw the Lewis dot structure for CH3NH2. (Hint: make the atom atom connectivity C-N-H) Based on your structure answer the following questions around the N. what is the electronic geometry? what is the molecular geometry?