Calculate the value of is for H+, He+ and Li+2 ions at r = 0, r = a, and r = 4a,, Rationalize the trends in the values that you calculate. 3/2 -Zr/ao 41s = e Υπ

A6

Without consulting tables of data, on the same graph sketch the effective potential energy curves for H2 and He+2.

Answer is A

H2 has equilibrium bond length of 0.751 Å and bond dissociation energy of 432 kJ mol21, whereas F2 has equilibrium bond length of 1.417 Å and bond dissociation energyof 155 kJ mol21. On the same graph show qualitativesketches of the effective potential energy curve Veff for anH2 and an F2 molecule. In your solution, show the conversion from kJ mol21to the energy of a single molecule.1

Three biological ly important diatomic species. eitherbecause they promote or inhibit life. are (a) CO. (b) NO. and(c) CN-. The first binds to haemoglobin. the second is a neurotransmitter. and the third interrupts the respiratory electrontransfer chain. Their biochemical action is a reflection of theirorbital structure. Deduce their ground-state electron configurations. For heteronuclear diatomic molecules. a good firstapproximation is that the energy level diagram is much thesame as for homonuclear diatomic molecules

In a gaseous KCl molecule, the equilibrium internucleardistance is 2.67 × 10=10 m. Using data from Appendix Fand assuming that a Coulomb potential is a good approximation of the potential from K+ + Cl= to 2.67 3 10=10 m,estimate the dissociation energy of gaseous KCl into K andCl atoms (in kJ mo=1). (Note: Table 3.7 shows that aCoulomb potential is only a good approximation to thepotential between two charged atoms at long inter-atomicdistances; the percent ionic character of KCl at equilibrium is only 82%.)

Based on data in Table 8.1, estimate (within 30 kJ>mol) thelattice energy for (a) LiBr, (b) CsBr, (c) CaCl2.

18 19 20 21 22 23 A student proposes the following Lewis structure for the nitronium (NO₂) i ion. [0=N=0:1 Assign a formal charge to each atom in the student's Lewis structure. atom formal charge left O 1 N 0 right O 7 Kindergarten O....docx Continue Two Column N....pages X ✓ C. Grey Black and B....pdf 24 25 ©2022 M Grey Black and B....p

A normal mode of vibration for H₂O is at 3650 cm Calculate the force constant, k, for H₂O. Assuming the force constant to be the same for H₂O and D₂O. Do you expect the corresponding D₂O wave number to be higher or lower? (Given: The atomic masses for H, D and O are 1.0, 2.0 and 16.0 respectively) (ii)