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## SOLVED:Which set of quantum numbers cannot specif…

Problem 61 Medium Difficulty

Which set of quantum numbers cannot specify an orbital?$$\begin{array}{ll}{\text { a. } n=2, l=1, m_{l}=-1} & {\text { b. } n=3, l=2, m_{l}=0} \ {\text { c. } n=3, l=3, m_{l}=2} & {\text { d. } n=4, l=3, m_{l}=0}\end{array}$$

Solved: Which Set Of Quantum Numbers Cannot Occur Together – Answer to Which set of quantum numbers cannot occur together to specify an orbital? A. n=3,l=?3,ml=0 B n=2,l=1,ml=?1 C. n=3,l=1,m…The value of 3 is not possible. So this set of quantum numbers cannot occur in an orbital. (d) n = 4, 1 = 3, m 1 = 0 When n = 4, / can have values of 0, 1, 2 and 3 and m 1 can have values from − 3 to + 3.The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on. The principal quantum number (n) cannot be zero. The allowed values of nare therefore 1, 2, 3, 4, and so on.

SOLVED:Which set of quantum numbers cannot occur – Here's what I got. As you know, the four quantum numbers that we use to describe the location and the spin of an electron in an atom are related as follows: So all you have to do here is to look at which values are permitted for the four quantum numbers given to you for each set. n = 2, l = 1, m_l = 1, m_s = -1/2" " " "color(darkgreen)(sqrt()) This is a valid set because all four quantumWhich set of quantum numbers cannot occur together to specify an orbital? Which set of quantum numbers cannot occur together to specify an orbital? n=3,l=2,ml=3 n=2,l=1,ml=−1 n=3,l=1,ml=−1 n=4,l=3,ml=3 Can someone explain how this works? My textbook is being super confusingThe number before the orbital name (such as 2s, 3p, and so forth) stands for the principal quantum number, n. The letter in the orbital name defines the subshell with a specific angular momentum quantum number l = 0 for s orbitals, 1 for p orbitals, 2 for d orbitals.

Quantum Numbers and Electron Configurations – We're asked to determine which set of quantum numbers cannot occur together to specify an orbital. To solve this problem, let's first define the values of the first three quantum numbers: • principal quantum number (n) → energy level in orbitals and its value could be any positive integer starting from 1 to infinityWhich set of quantum numbers cannot occur together to specify an orbital?. You'll find the correct answer below. 18. Which set of quantum numbers cannot occur together to specify an orbital? A. n=3, l=âˆ'3, ml=0 B. n=4, l=3, ml=0 C. n=2, l=1, ml=1 D. n=3, l=2, ml=0. The Correct Answer is. n=3, l=âˆ'3, ml=0None of these represent the ground state, but If they are excited states then . n =3; l =3; ml =1. cannot specify an orbital – if n = 3 then l can be 0, 1, or 2, not 3