1) Draw the best Lewis structures for the molecules below in bond line notation with the correct bond geometry. Make sure to include formal charges if needed. If you can draw more than one resonance structure of the compound provide the best structure. a. CH3CH2CCCOOH b. CH3CH2C(NH)CH(CH3)2 c. CH2CHCH2NCO Geometry at terminal Carbon highlighted in bold Bond angle of indicated Carbon Geometry at Carbon highlighted in bold attached to N Bond angle of indicated Geometry at terminal Carbon highlighted in bold Bond angle at C

1) Draw the best Lewis structures for the molecules below in bond line notation with the correct bond geometry. Make sure to include formal charges if needed. If you can draw more than one resonance structure of the compound provide the best structure. a. CH3CH2CCCOOH b. CH3CH2C(NH)CH(CH3)2 c. CH2CHCH2NCO Geometry at terminal Carbon highlighted in bold Bond angle of indicated Carbon Geometry at Carbon highlighted in bold attached to N Bond angle of indicated Geometry at terminal Carbon highlighted in bold Bond angle at C

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

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...

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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.
3. Draw the best complete Lewis structure for each of the following molecules or ions. Make sure to include all lone pairs and formal charges when necessary a. CO₂H2 b. CH3O- c. CNH6+
T'he incomplete Lewis structure below shows all the atoms and sigma bonds for a particular molecule, but nothing else. The molecule has a net charge of 0. Fill in any missing electrons to create the best Lewis structure for the molecule. Make sure to include any non-zero formal charges. H. H. H нн H
ll X b My Questions | bartleby Login | bartleby 101 Chem101 ぐ app.101edu.co Question 1 Draw a resonance structure that shifts a pi bond to a new position. Don't increase the number of atoms with formal charges. Include all hydrogen atoms in your structure. H. Atoms, Bonds an Drawing CHa :CHs: %3. 3D CH2 CH2 MacBook 0:0 3D 3D
(b) For each of the following molecules below (i) draw the Lewis dot structure and any important resonance structures and (ii) use VSEPR theory to predict and draw its geometry. 1. BeCl2 2. N2O 3. SF4 4. H2O 5. SO42- 6. PF6− 7. H3O+ 8. IF3 9. ICl4−
Consider the generic polyatomic ion XY3". Element X is the least electronegative. For neutral atoms, element X has 7 valence electrons and element Y has 6. The highest occupied principal energy level of the central atom is greater than 2. A. How many total valence electrons are in the molecule. B. Draw a BEST Lewis structure (i.e. a major resonance contributor) for this molecule. Show all valence electrons on your structure. C. If you haven't already, add the formal charge of each atom to the structure. Show at least one sample calculation for formal charge. D. Outline 4 short bullet points (~several words each) that explain why your structure from part B is the best one. Hint: think about what makes a valid structure and what makes a best structure. E. Perform a calculation to determine the average bond order between the X and Y atoms in your structure from part B. No credit will be given for just a number. F. Draw one more valid resonance structure other than the one from part B.…
Using BEST Lewis structures and the VSEPR model, match each molecular formula with the molecular geometry that describes it.
8. For each molecular fomula, detem ine the electron pair geom etry (EPG), make a 3-dimensional representation, and determ ine the molecular geometry. Determine whether the molecule is polar or non- polar. All of these have central atoms surounded by term inal atom s/one pairs only. Formula A. CHF3 Lewis structure EPG 3-D drawing Mol Geom. Polar molecule? B. SF2
Draw a valid Lewis structure for each molecule. a. HI b. CH 2F 2 c. H 2Se d. C 2Cl 6
Write a Lewis structure for each of the following simple molecules. Show all bonding valenceelectron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules thatexhibit resonance, draw the various possible resonance forms.a. NO2b. H2SO4c. N2O4
Your answer is incorrect. Decide whether the Lewis structure proposed for each molecule is reasonable or not. • Row 1: Your answer is incorrect. ● Row 2: Your answer is incorrect. molecule proposed Lewis structure CO₂ IBr, SF 3 +TE. .. :0 C 0: Br F — S — :F: Br :E: Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: F
8. Molecule: IF3 indicate the number of available electrons that are in the molecule. in the space to the right connect all of the atoms ae = Trial Structure: to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization: