Solutions for Lecture 9: Periodic Table; Ionic and Covalent Bonds | Massachusetts Institute of Technology - Edubirdie

University:
Massachusetts Institute of Technology
Course:
5.111SC | Principles of Chemical Science
Academic year:

2021
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10

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1
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destricar154

LECTURE 9 1. (a) Which atom or ion in each of the following pairs has the larger radius? (i) V or Mo (ii) V or Zn (iii) Ca or Ca2+ (b) Briefly explain the relationship between effective nuclear charge and atomic radius. (a) (i) Mo (ii) V (iii) Ca (b) As effective nuclear charge increases, atomic radius decreases. 2. Consider the KF molecule, which has an ionic bond. The bond length is 2.17 x 10-10 m. (a) Calculate the energy required to dissociate the KF molecule into the ions K+ and F-. (b) The energy required to dissociate KF into neutral atoms is 498 kJ/mol. Given that the first ionization energy for K is 418 kJ/mol, calculate the electron affinity (in kJ/mol) for F. Show your work for all calculations. (a) +6.40 x 102 kJ mol-1 or +1.06 x 10-18 J (b) +276 kJ mol-1 3. Draw an energy diagram (with energy on the y-axis and internuclear distance, r, on the xaxis) plotting a C–F and a C–I bond. You should include numbers on the y-axis. No numbers are needed on the x-axis, but relative distances should be correct. Bond dissociation energies are 238 kJ/mol and 484 kJ/mol for C-I and C-F respectively.

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