Determine if the structural formula below is an acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. :0: CH3 CH-C-Ö-ČH-CH3 A. This is not the correct Lewis structure. B. No, All atoms do not have a zero formal charge, therefore this is not the correct Lewis structure. C. All atoms have a zero formal charge, therefore this is the correct Lewis

Determine if the structural formula below is an acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. :0: CH3 CH-C-Ö-ČH-CH3 A. This is not the correct Lewis structure. B. No, All atoms do not have a zero formal charge, therefore this is not the correct Lewis structure. C. All atoms have a zero formal charge, therefore this is the correct Lewis

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter1: Bond Angles And Shape

Section: Chapter Questions

Problem 12CTQ: Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this...

See similar textbooks

Similar questions

There is persuasive evidence for the brief existence of theunstable molecule OPCl.(a) Draw a Lewis diagram for this molecule in which theoctet rule is satisfied on all atoms and the formalcharges on all atoms are zero .(b) The compound OPCl reacts with oxygen to giveO2PCl. Draw a Lewis diagram of O2PCl for which allformal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
This bond is made of an sp3 orbital from a carbon atom to a 1s orbital from the H atom. The correct orbital overlap is sp3-s. What type(s) of orbital overlap is(are) indicated on the following structure: -sp3-sp -sp2-s -sp3-s -p-p -sp3-sp2
1. Please explain how an FTIR works 2. Why it's so important and useful for organic chemistry
(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).
1. Draw Lewis Structures for the following compounds. (Be sure to minimize formal charges and draw resonance structures where appropriate.): XeF2O, ClO4-, HNO2, CH3CH(NH2)COOH (amino acid alanine). 2. ID the molecules with the following labels (1 is more than one label): Oxyacid, has a resonance structure, expanded octet, has a carbon backbone 3. For the molecule with resonance structures—what is the bond order for the atoms that share e-?
In most amines, the nitrogen atom is sp3 hybridized, with a pyramidal structure and bond angles close to 109°. In urea, both nitrogen atoms are found to be planar, with bond angles close to 120°. Explain this surprising finding. (Hint: Consider resonance forms and the overlap needed in them.)
Select one: True or False 1- Besides providing the largest suitable number of valance orbitals for covalent bond formation it can determine the final shape of the molecule for example Sp hybridization leads to a diagonal planner molecule, SP2 hybridization while Sp3 hybridization leads a pyramidal (tetrahydral shape) 2- About the underlying compound ( in the images ) , it it’s a calcium complex of EDTA used to treat metal toxicities like pulmbism in order to avoid hypocalcaemia.
Which member of the following would you expect to be more energetically stable? Justify each choice. a. NaBr or NaBr2 b. C1O4 or C1O4- c. SO4 or XeO4 d. OF4 or SeF4
Devise a 3-D model that demonstrates the bonding between atoms of ClF3 molecule as well as any lone pairs. You can use any material you want/have to demonstrate the model. Please attach clear pictures of the model.
There are three different dichloroethylenes (molecular for-mula C₂H₂Cl₂), which we can designate X, Y, and Z. CompoundX has no dipole moment, but compound Z does. Compounds Xand Z each combine with hydrogen to give the same product:C₂H₂Cl₂ (X or Z) +H₂→ClCH2-CH2Cl What are the structures of X, Y, and Z? Would you expect com-pound Y to have a dipole momen
Sketch propylene (C3H6) showing the orbitals and any overlapping orbitals to indicate covalent bonds. Also, label all bonds using sigma or pi notation followed by the type of overlapping orbitals.