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- Consider the molecule BF3. (a) What is the electron configurationof an isolated B atom? (b) What is the electron configurationof an isolated F atom? (c) What hybrid orbitalsshould be constructed on the B atom to make the B–F bondsin BF3? (d) What valence orbitals, if any, remain unhybridizedon the B atom in BF3?(a) If you combine two atomic orbitals on two different atomsto make a new orbital, is this a hybrid orbital or a molecularorbital? (b) If you combine two atomic orbitals onone atom to make a new orbital, is this a hybrid orbital or amolecular orbital? (c) Does the Pauli exclusion principle apply to MOs? Explain.If an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.
- Ethyl acetate, C4H8O2, is a fragrant substance used both as asolvent and as an aroma enhancer. Its Lewis structure is given (a) What is the hybridization at each of the carbon atomsof the molecule? (b) What is the total number of valenceelectrons in ethyl acetate? (c) How many of the valence electronsare used to make s bonds in the molecule? (d) Howmany valence electrons are used to make p bonds? (e) Howmany valence electrons remain in nonbonding pairs in themolecule?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 π2p 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?The ground-state electron configuration of He; is (o,1s)'(0,1s)' . Calculate the bond order of Hez. (A) 3/2 (B) 1/2 (С) 1 (D) -1/2
- The molecule shown below is called furan. It is represented intypical shorthand way for organic molecules, with hydrogenatoms not shown, and each of the 4 vertices representing acarbon atom. (a) What is the molecular formula for furan? (b) How manyvalence electrons are there in the molecule? (c) What isthe hybridization at each of the carbon atoms? (d) Howmany electrons are in the π system of the molecule? (e) TheC¬C¬C bond angles in furan are much smaller than thosein benzene. The likely reason is which of the following: (i) Thehybridization of the carbon atoms in furan is different fromthat in benzene, (ii) Furan does not have another resonancestructure equivalent to the one above, or (iii) The atoms in afive-membered ring are forced to adopt smaller angles than ina six-membered ring.(b) (i) Draw a labelled molecular orbital energy level diagram for F₂. Calculate the bond order for F₂ and state if the molecule is expected to exist. (II) Calculate the bond order for [F₂]* and [F₂).Indicate whether each statement is true or false. (a) s orbitalscan only make σ or σ* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a π* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.