The allene molecule H2C=C=CH, is linear (the 3 C atoms lie on a straight line). What is the hybridization state of the carbon atoms? (a) either H2C=group (b) the =C= atom sp sp sp? sp?
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- Which of the following is the correct bond-line structure for (CH3)2CHCH₂C(CH3)3? OI O II IV OV ty || ||| IVDinitrogen difluoride, N₂F₂, is the only stable, simple inor-ganic molecule with an N=N bond. The compound occurs incisand transforms.(a) Draw the molecular shapes of the two forms of N₂F₂.(b) Predict the polarity, if any, of each form.Ketene, CH2=C=O, is an unusual organic molecule that has a singlecarbon atom doubly bonded to two different atoms. Determine thehybridization of both C atoms and the O in ketene. Then, draw a diagramshowing what orbitals are used to form each bond.
- 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:Octocrylene is an ingredient found in topical sunscreens. It is a water-resistant molecule that helps protect skin against harmful UVA and UVB radiation. (a) What is the hybridization of each nonhydrogen atom? (b) Circle all atoms bonded to the acyclic C=C double bond that are required to be in the same plane. (c) Are there two unique configurations possible about the acyclic C=C double bond? Explain. (d) Which of the two C-C single bonds indicated by arrows would you expect to be shorter? Explain. OctocryleneThe ground-state electron configuration of the H; molec- ular ion is (og15)'. (a) A molecule of H absorbs a photon, promoting the electron to the os molecular orbital. Predict what happens to the molecule. (b) Another molecule of H absorbs even more energy promoting the electron to the o,2, molecular orbital. Predict what happens to this molecule.
- 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?Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?Ethyl acetate, C4H8O2, is a fragrant substance used both as asolvent and as an aroma enhancer. Its Lewis structure is (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?
- 6.For the molecules shown below: L=molecule on left, R=molecule on the right H. CH3 at C H' ******* C%3Cd H -CH3 N. PCL R. (a) Add the lone pair of electrons to all atoms in both structures that have lone pairs (b) What hybrid orbital is used by the C in the CN group of L? (c) How many o (d) What is the approximate bond angle shown as “c" in L? - (e) What is the approximate bond angle shown as "f' in R? --- (f) What hybrid orbital is used by the O in the OCH3 group in R and how many t - bonds are there in L? --- -- -4. (a) Use the simple one-electron molecular orbital method, including overlap, to calculate the energies of the molecular orbitals of the hydrogen molecule (H₂) in terms of a, ß and S? (b) Calculate & given that a = -13.6 eV, that S = 0.6, and that the lowest UV absorption energy is 12 eV. (c) Determine the ionisation energy of the bonding molecular orbital in H₂ ? [6 marks]Are these statements true or false? Correct any that are false.(a) Two bonds comprise a double bond.(b) A triple bond consists of one bond π and two bonds σ.(c) Bonds formed from atomic sorbitals are always bonds.(d) A π bond restricts rotation about the σ-bond axis.(e) A π bond consists of two pairs of electrons.(f) End-to-end overlap results in a bond with electron density above and below the bond axis.