f) The unusual molecule [2.2.2] propellane is pictured.1) Given the bond length and bond angles in the image, what hybridization schemebest describes the carbons marked by the askerisks?2) What types of orbitals are used in the bond between the two carbons marked bythe askerisks?3) How does this bond compare to an ordinary carbon-carbon bond (which is usually1.54 Å long)?H₂CH₂CCH2 1.60ÅハC.*CH₂H₂C*CH₂120°

Answered: Image /qna-images/answer/08e9dcc6-e936-432b-8043-c5e25365ff7f.jpg

Answered: f) The unusual molecule [2.2.2]…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 76QAP: In each of the following molecules, a central atom is surrounded by a total of three atoms or...

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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?
Which of the following statements is/are true? Correct the false statements. a. The molecules SeS3. SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle which is approximately 120. b. The bond angle in SO2 should be similar to the bond angle in CS2 or SCI2. c. Of the compounds CF4, KrF4, and SeF4, only SeF4 exhibits an overall dipole moment (is polar). d. Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.
Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in HF place greater electron density near the H or the F atom? Why? b. Would the bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both? Why? c. Answer the previous two questions for the antibonding molecular orbital in HF.
Aspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is (a) Complete the Lewis structure and give the number of and bonds in aspartame. (b) What is the hybridization about each carbon atom that forms a double bond with an oxygen atom? (c) What is the hybridization about each nitrogen atom?
7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?
Benzene is one of the compounds used as an octane enhancer in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2H2C6H6 Draw Lewis structures for these compounds, with resonance structures as appropriate, and determine the hybridization of the carbon atoms in each.
How can we drsw the Lewis structures for the 4 boxes? And how many charges are in Oxime?
Consider a molecule AB, where element A has 6 valence electrons and B has 7 valence electrons. If the AEn 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.
Carbon dioxide, dinitrogen monoxide, the azide ion N3-, and cynate ion OCN- have the same arrangement of atoms and the ame number of valence shell electrons. Howeer, there are significant differences in the electronic structures. What hybridization should be assigned to the central atom in each species? Are there any resonance structures associated with these molecules and/or ions? If so, descrie them. Estimate the bond lengths and bond orders of each atom in these molecules and ions.
A compound composed of 2.1% H, 29.8% N, and 68.1% Ohas a molar mass of approximately 50 g/mol. (a) Whatis the molecular formula of the compound? (b) What isits Lewis structure if H is bonded to O? (c) What is the geometryof the molecule? (d) What is the hybridization ofthe orbitals around the N atom? (e) How many s and howmany π bonds are there in the molecule?
The following “bubble” diagram is for the compound H2C=C=CH2 . Using the system we discussed in class label all of the bonds on the bubble diagram using valence bond theory the format is : type of bond : atoms (type of orbital) - atom ( type of orbital) . Be specific as you can in your label Look In the diagram
Complete the following table: Lewis structure atoms: bonds between orbitals making each total bond order hybridization atoms: type E valence bond: between two atoms |Н: 1s C and H: o sp?(C) + 1s(H) C and H: 1 C: sp? Cl: sp3 0: sp? :0: || C and Cl: o sp?(C) + sp°(CI) C and Cl: 1 = sp?(C) + sp²(0) = p(C) + p(0) C and O: o C and O: 2 CI C and O: t C: C and C: C and C: C and C: C: H-C=C-H H: C and H: C and C: H: C and H: N: N and I: N and I: N= I: N and I: C: C and Cl: C and Cl: :Cl Cl: C and Cl: C and Cl: Cl: C and Cl: -c=cl: C and Cl: :Z: :U:

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