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- The diagram that follows shows the highest-energy occupiedMOs of a neutral molecule CX, where element X is in thesame row of the periodic table as C. (a) Based on the numberof electrons, can you determine the identity of X? (b) Wouldthe molecule be diamagnetic or paramagnetic? (c) Considerthe p2p MOs of the molecule. Would you expect them to havea greater atomic orbital contribution from C, have a greateratomic orbital contribution from X, or be an equal mixtureof atomic orbitals from the two atoms?Use the References to access important values if needed for this question. Consider the fluorine molecule and the F," molecular ion: (a) Give the bond order of each species. If a fraction is needed, use a decimal number. Bond order F2 Bond order F2= (b) Predict which species should be paramagnetic. Is F2 paramagnetic? | Is F2 paramagnetic? (c) Predict which species has the greater bond dissociation energy. The species with the largest bond dissociation energy is: a. F2 b. F2I wonder (d) below. Carbon monoxide is produced by incomplete combustion offossil fuels.(a) Give the electron configuration for the valence molecular orbitals of CO. The orbitals have the same energyorder as those of the N2 molecule.(b) Do you expect CO to be paramagnetic or diamagnetic?(c) What is the bond order of CO? Does this match thebond order predicted by the electron-dot structure?(d) CO can react with OH- to form the formate ion,HCO2-. Draw an electron-dot structure for the formateion, and give any resonance structures if appropriate. Thanks:)
- с ☐ng.cengage.com/static/nb/ui/evo/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707785992&snapshoti... CWhat is the bond order of the C-O bonds in the carbonate ion ? ChemDoodle dIn which species (CO32- or CH3CHO) are the C-O bond(s) longer? Submit e In which species (CO32- or CH3CHO) are the C-O bond(s) weaker? Submit Answer PRO MacBook Air U (enter a decimal number) *Consider the molecule C4H5N, which has the connectivityshown below. (a) After the Lewis structure for the moleculeis completed, how many s and how many p bonds arethere in this molecule? (b) How many atoms in the moleculeexhibit (i) sp hybridization, (ii) sp2 hybridization, and(iii) sp3 hybridization?. Both the simple VB model and the LCAO method predictthat the bond order of Be2 is 0. Explain how each arrivesat that conclusion.
- 2. For each of the following homonuclear/heteronuclear diatomic molecules of the second row of the periodic table: (i) N₂ (ii) O₂ (iii) NO (iv) BO (v) HCI (a) sketch and label the molecular orbital energy level diagram (note: Remember to use sp mixing where appropriate). (b) determine the bond order, (c) state its magnetic properties, (d) give its molecular orbital electron configuration.c) What change to valenca bond theory had to be made to account for the molecular goometry of water and CO2? Explain what change was made and then specifically apply the change to these two molecules. d) When it was found that Og is paramagnetic, still another change in bonding theory had to be made, particularly for diatomic molecules. State what is meant by paramagnetism in the O2 molecule and the new approach to bonding that explained why it oocurred.a.) Sketch for yourself the MO diagram for the following three heteronuclear diatomic species. Give the bond order of: CO, NO, CN^- b.) Sketch for yourself the molecular orbital energy level diagram for KrF and deduce its ground state electron configurations. Is KrF likely to have a shorter or longer or same bond length as KrF+?
- 60. Column- (Molecular species) (A) SO, (8) PO (C) CO₂² (D) CIO CHEMISTR Column-II (Characteristics of molecular species) (P) All bond angles are same (Q) Bond order is fractional (R) Non axial d-orbital participate in bond formation (S) Three oxygen atoms lie in a plane (T) 2p-2p, bond is presentAntibonding molecular orbitals can be used to make bondsto other atoms in a molecule. For example, metal atomscan use appropriate d orbitals to overlap with the p*2p orbitalsof the carbon monoxide molecule. This is calledd@p backbonding. (a) Draw a coordinate axis system inwhich the y-axis is vertical in the plane of the paper andthe x-axis horizontal. Write “M” at the origin to denote ametal atom. (b) Now, on the x-axis to the right of M, drawthe Lewis structure of a CO molecule, with the carbonnearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO p*2p orbital, with phases (see the “CloserLook” box on phases) in the plane of the paper. Two lobesshould be pointing toward M. (d) Now draw the dxy orbitalof M, with phases. Can you see how they will overlap withthe p*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, s or p ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.1- Use the molecular orbital model to predict the bond order and magnetism of each of the following molecules.a- COb- CO+c- CO2+ 2- Compare and contrast bonding molecular orbitals with antibonding molecularorbitals. 3- Consider the following electron configuration:(σ3s)2(σ3s*)2(σ3p)2(π3p)4(π3p*)4Give four species that, in theory, would have this electron configuration. 4- Predict which substance in each of the following pairs would have the greaterintermolecular forces.I. CO2 or OCSII. SeO2 or SO2III. CH3CH2CH2NH2 or H2NCH2CH2NH2IV. CH3CH3 or H2COV. CH3OH or H2CO 5- Explain why water forms into beads on a waxed car finish. 6- At which temperature does water have its greatest density? 7- At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is solid. This is because of what?