0102口408032 7.If orbitals have such interesting shapes,why are atoms considered to be spherical? Orbitals do not really have these shapes. Therbitals are the argest and are spherical,making theentiremappear spherical The spherical shape of of all put together Electrons are spherical None of the above 8.Predict the electronic configuration of Vanadium(element #23): 1s 2s22p 3s 3p 4s2 3d C1s22s22p53s23p53d34s2 口1522s22p53s23p4s'3对 C[Kr]4s3d None of the above 9.In an atom of He,one electron has the quantum numbers n=1,1=0,m0, m,+1/2.What are the quantum numbers of the other electron? Cn2,0,m-0,m,=+1/2 C=l,0,m-0,m,-1n. C=L,1,m-0,m=+12. C n=1,1-0,mr-1,m-+1/2. None of the above 10.Why is the electronic configuration of Mo [Kr]5s'4dand not [Kr]5s4d as predicted by AUFBAU?1 2 4 8 32 7. If orbitals have such interesting shapes, why are atoms considered to be spherical? Orbitals do not really have these shapes. The s orbitals are the largest, and are spherical, making the entire atom appear spherical. The spherical shape of the atom is a time average of all its orbitals put together. Electrons are spherical None of the above 8. Predict the electronic configuration of Vanadium (element #23): 1s2 2s2 2p6 3s2 3p6 4s2 3d3 1s2 2s2 2p6 3s2 3p6 3d3 4s2 1s2 2s2 2p6 3s2 3p6 4s1 3d4 [Kr] 4s2 3d3 None of the above 9. In an atom of He, one electron has the quantum numbers n=1, l=0, ml=0, ms=+1/2. What are the quantum numbers of the other electron? n=2, l=0, ml=0, ms=+1/2 n=1, l=0, ml=0, ms=-1/2. n=1, l=1, ml=0, ms=+1/2. n=1, l=0, ml=1, ms=+1/2. None of the above 10. Why is the electronic configuration of Mo [Kr] 5s1 4d5 and not [Kr] 5s2 4d4 as predicted by AUFBAU?