+ Draw the Lewis structure of glycine (NHCH2COO) and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure. A sp³/sp³/sp² B 0 sp/sp²/sp² sp²/sp/sp³ D sp/sp/sp² E sp³/sp³/sp Click to draw a new structure

+ Draw the Lewis structure of glycine (NHCH2COO) and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure. A sp³/sp³/sp² B 0 sp/sp²/sp² sp²/sp/sp³ D sp/sp/sp² E sp³/sp³/sp Click to draw a new structure

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 18P: When one electron is added to an oxygen molecule, a superoxide ion (O2) is formed. The addition of...

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When one electron is added to an oxygen molecule, a superoxide ion (O2) is formed. The addition of two electrons gives a peroxide ion (O22) . Removal of an electron from O2 leads to O2+ . (a) Construct the correlation diagram for O2 . (b) Give the valence electron configuration for each of the following species: O2+,O2,O2,O22 . (c) Give the bond order of each species. (d) Predict which species are paramagnetic. (e) Predict the order of increasing bond dissociation energy among the species.
Identify the orbitals on each of the atoms that form the bonds in H3CCN. How many bonds and bonds form?
Draw an example of a bent molecule with a bond angle of near 109.5°; then draw a different bentmolecule with a bond angle of about 120°.
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
Following is a structural formula of benzene, C6H6, which we study in Chapter 21. (a) Using VSEPR, predict each HCC and CCC bond angle in benzene. (b) State the hybridization of each carbon in benzene. (c) Predict the shape of a benzene molecule. (d) Draw important resonance contributing structures.
In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?
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.
Molecule or Polyatomic C₂H₂ NO3 2- SO3²- CH₂O OF 2 Lewis structure H-C=C-H O :0 10: H-C-H : F-0—F : 2- Hybrid- ization AXE sp AX₂ sp AX3 3 sp AX3E 2 sp AX3 sp 3 AX₂E2 Electron pair geometry Molecular shape linear linear trigonal planar trigonal planar tetrahedral trigonal pyramidal trigonal planar trigonal planar tetrahedral bent Bond angles all 180° all 120° all ~109.5° all 120° ~109.5° Bond Polarity Molecular Polarity if the molecule is polar, add a dipole arrow if not polar, state so and why H-C=C-H . L H F |||S. o H F
Molecule or Polyatomic CHzCl 2- Co₂² CH4 CS₂ H₂O Lewis structure H-C-CI: H H H-C-H H s=c=s H–O–H 2- Hybrid- ization AXE 3 sp³ AX4 2 sp² AX3 3 sp³ AX4 sp AX2 3 sp³ AX₂E2 Electron pair geometry Molecular shape tetrahedral tetrahedral trigonal planar trigonal planar tetrahedral tetrahedral linear linear tetrahedral bent Bond angles all ~109.5° all 120° all ~109.5° 180° ~109.5° Bond Polarity H C 2.5 2.1 Cl 2.5 3.0 CO 2.5 3.5 C-H 2.5 2.1 Molecular Polarity if the molecule is polar, add a dipole arrow if not polar, state so and why H H H i no molecular polarity because of shape CI H H HC H no polar bonds, so no molecular polarity H S=C=S H
Just need the last two, Bond angle and 3D structure and polarity
Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.
Draw the Lewis structure of AsO³- showing all lone pairs. Select Draw Rings More ||||||||| As G Erase Q2 Q 3- Identify the molecular geometry of AsO³. 4 see-saw O T-shaped tetrahedral octahedral linear square pyramidal trigonal planar trigonal pyramidal bent square planar O trigonal bipyramidal