Tutorial 2 1 The bond dissociation enthalpies for

Tutorial – 2 1) The bond dissociation enthalpies for the nitrogen–nitrogen bond in N 2 and [N 2] are 945 and 765 k. J/mol respectively. Account for this difference in terms of MO theory, and state diamagnetic or paramagnetic nature of N 2 and [N 2]. 2) Using MO theory, explain why the N N bond distance in [N 2]+ is longer (112 pm) than in N 2 (109 pm). 3) Using VSEPR model predict the shape of SO 32 - and SO 42 - 4) Draw the Lewis structure of SO 42 - and calculate charge on each atom. 5) Explain why the first ionization energy of phosphorus, P (I 1=1011 k. J/mol) is more than sulfur, S (I 1=1000 k. J/mol). 6) Predict the ground-state electron configurations of (a) Ti and (b) Ti 3+.

Tutorial - 3 7) (a) Write down the wavefunction (derived from Schrödinger equation) of electron in polar coordinates. (b) Plot the radial part of wavefunction of s orbitals (1 s and 2 s) of hydrogen atom against distance, r, from the nucleus. (c) Plot the radial part of wavefunction of p orbitals (2 p and 3 p) against distance, r, from the nucleus. 8) How many radial nodes are possible for 1 s, 2 p, 3 p and 3 d orbitals. 9) Plot the radial distribution function [4πr 2 R(r)2 ] of s orbitals (1 s, 2 s, 3 s) against distance, r, from the nucleus. Explain the signification of radial distribution function from each plot.