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24——,, , =, ‘TEST ASSIGNMENT, , ted states of an atom, Rules for filling, Pauli’s exclusion principle,, ‘onfigurations of elements, , Relative energies of orbitals, Ground and e3, electrons in orbitals; Aufbau principle,, Hund’s rule, Electronic 6, , , , 1, What are degenerate orbitals? Give one example., Which of the following sets of quantum numbers for the same atom has a greater enerBy, 3,1 = 1 and m = 41 iin =3,l=2andm=-1 (Ans. iid, .d excited states., , for electrons? i. n, , , , Write the electronic configurations of a hydrogen atom in the ground ani, , State Aufbau principle. Which of the following orbitals are possible: 1p, 2s, 2p and 3f ?, Uns. 28, 2p], , ae, , In building up of the atoms, the filling of 4s orbital takes place before the 3d orbital., Explain., , *, , 6, State Pauli’s exclusion principle., 7, What is the most important outcome of the Pauli’s exclusion principle?, , g, If the quantum numbers needed to specify an electron in any orbital are n, 1, m and + 1/2,, , then what should be the quantum numbers of the second electron to be accommodated, , in the same orbital? [Ans. a, l, m and — V/2), , 9. Give the values of the quantum numbers n, / and m for the electron with highest energy, , in sodium atom. Uns. n = 3,1 =0, m= 0), , 10. Using the concept of quantum numbers, calculate the number of electrons that could be, , present in the L-shell of an atom. tans. 8], , 11, State Hund’s rule of maximum multiplicity. Can it be applied for the filling of electrons, into molecular orbitals?, , 12, ee ee configuration, 1s? 26? 2p? 2p 2p? not correct for the ground state, 18, Why is the electronic configuration of oxygen written as 1s? 2s? 2p? 2p! 2p! and, 1s? 2s? 2p? 2p}? Name the rule governing this type of distribution,, 4. Describe the extra-stability of half‘filled and completely-flled orbitals,