Can you solve this question according to the criteria

1. Arrange the following atoms according to increasing electron affinity: aluminum, argon, fluorine. Clearly and fully motivate the chosen ranking (10 pts). Answer - Definition of electron affinity - Use Coulomb's law to calculate the force by which the added electron is attracted to the nucleus; this means that you have to calculate the charge with which the 'new' electron is attracted to the nucleus, thus the Zetitformed anion. Define effective nuclear charge and explain how it is calculated approximately with the formula proposed in the course (no shielding of nuclear charge by outer electrons, and for inner electron shielding of one proton charge) you have to estimate the distance between the 'new' electron and the nucleus, which is proportional to the main quantum number of the orbital to which the 'new' electron is assigned, but the distance also decreases within the same period of time - The larger the force the more energy will be released when adding the 'new' electron - Ranking: Ar+2 Coulomb's Law and explanation of why it is used: +1 Definition effective nuclear charge: +1 Calculation Zeff,anions (explain why from anions and not atoms) with description of approximation to calculation: +3 Correct order substantiated by previous : +3 If Zeff is not used: 5 If Zeff was not clearly defined: -3 If Coulomb's law not stated/used: 3 If Zeff calculated from the atoms (instead of anions):-3 If it is stated that noble gases (such as Ar) have the noble gas configuration and are therefore inert, or are an exception... (or all possible variations on this): 5 If only the sequence is correct but the reasoning is wrong (cfr above): 3/10