### Determining Possible and Impossible Subshell Designations**Question:**Which of the subshell designations are possible and which are impossible?### Explanation:To answer this question, it's important to understand the rules governing the possible subshell designations in an atom's electron configuration. These rules involve the quantum numbers, specifically the principal quantum number (\(n\)) and the azimuthal quantum number (\(l\)). The possible values for \(l\) (azimuthal quantum number) are integers ranging from 0 to \(n-1\). Each value of \(l\) corresponds to a specific subshell:- \(l = 0\) corresponds to s subshell- \(l = 1\) corresponds to p subshell- \(l = 2\) corresponds to d subshell- \(l = 3\) corresponds to f subshellThe possible combinations of \(n\) and \(l\) must conform to these rules.#### Possible Subshells:- **4d**: Here, \(n = 4\) and \(l = 2\). Since \(l\) (2) is less than \(n\) (4), this subshell is possible.- **2f**: Here, \(n = 2\) and \(l = 3\). Since \(l\) (3) is not less than \(n\) (2), this subshell would normally be considered impossible according to the standard rules. There might be an error in the provided answer.#### Impossible Subshells:- **5f**: While the image classifies this as impossible, based on quantum mechanics and allowed quantum numbers, \(n = 5\) and \(l = 3\) are compatible. Thus, this should be possible, indicating another potential misclassification.- **0p**: Here, \(n = 0\) and \(l = 1\). Since \(n\) is less than 1, it is an impossible subshell.- **1d**: Here, \(n = 1\) and \(l = 2\). \(l\) cannot be larger than or equal to \(n\), making this subshell impossible.### Summary:- The answer bank should reassess the designation of the 2f and 5f subshells.- According to standard quantum mechanical rules

Number of possible azimuthal quantum number (l) = 0 to (n-1) Relation between (l) and subshell: l…

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Which of the subshell designations possible and which are impossible? are Possible Impossible 5f 4d Op 2f ld

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Electronic Transitions and Spectroscopy

The term “electronic” connotes electron, and the term “transition” implies transformation. In a molecule, the electrons move from a lower to a higher energy state due to excitation. The two energy states, the ground state and the excited state are the lowest and the highest energy states, respectively. An energy change is observed with this transition, which depicts the various data related to the molecule.

Photoelectron Spectroscopy

Photoelectron spectroscopy (PES) is a part of experimental chemistry. It is a technique used in laboratories that involves projecting intense beams of radiation on a sample element. In response, the element ejects electrons for which the relative energies are measured.

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