What Are the Quantum Numbers for All Electrons in Boron and Nitrogen Atoms?

[alingy1]

Homework Statement

Give a possible set of values of the four quantum numbers for all the electrons in boron atom and a nitrogen atom if each is in the ground state.

I know the principles behind this. It comes from Zumdahl's Chemistry textbook (ninth edition, p. 345, number 95). The solutions manual however lists 5 examples for boron and 7 for nitrogen.

However, doesn't this question ask for only ONE possible set of values?

Shouldn't writing n=0 l=0 ml=0 ms=+1/2 for both boron and nitrogen enough to get the answer right?

I'm a second language speaker! Why do they say "all the electrons"? What are they asking for?

 

[Simon Bridge]

It asks for "a" possible set of values - since there is more than one possible set, there is more than one possible correct answer. Therefore the solutions manual has to list them all.

However ... this is not the case for this problem.
Reading carefully you see it wants the set of values for all the electrons ... how many electrons does Boron have? How many does Nitrogen have? Therefore - how many values must be in each set?

 

[alingy1]

Hmm. If I give a possible set of values for each electron in each atom, my answer would be :
BORON: 1s22s22p1
n 1 1 2 2 2
l 0 0 0 0 1
ml 0 0 0 0 -1
ms +1/2 -1/2 +1/2 -1/2 +1/2NITROGEN: 1s22s22p3
n 1 1 2 2 2 2 2
l 0 0 0 0 1 1 1
ml 0 0 0 0 -1 0 +1
ms +1/2 -1/2 +1/2 -1/2 +1/2 +1/2 +1/2

Would this answer be the most concise and thorough answer?

 

[alingy1]

Sorry, it seems the forum does not accept long spaces. My tables are therefore not aligned.

 

[DeeNos]

I can provide a response to the content of the given problem. The four quantum numbers, namely the principal quantum number (n), angular momentum quantum number (l), magnetic quantum number (ml), and spin quantum number (ms), describe the energy levels, shapes, orientations, and spin states of electrons in an atom.

For the ground state of an atom, the values of the quantum numbers for all the electrons are determined by the electron configuration, which follows the Aufbau principle and the Pauli exclusion principle. Based on this, a possible set of values for the four quantum numbers for all the electrons in a boron atom would be n=2, l=1, ml=-1, and ms=+1/2. This means that there are two electrons in the second energy level (n=2), in the p subshell (l=1) with a -1 orientation (ml=-1) and a spin state of +1/2 (ms=+1/2).

Similarly, for a nitrogen atom in the ground state, a possible set of values for the four quantum numbers could be n=2, l=1, ml=0, and ms=+1/2. This indicates that there are two electrons in the second energy level, in the p subshell with a 0 orientation, and a spin state of +1/2.

It is important to note that the question is asking for a possible set of values for all the electrons in each atom, not just one electron. This is because the quantum numbers of electrons in an atom are not independent of each other, and the set of quantum numbers for one electron can affect the values for the others.

In conclusion, writing n=2, l=1, ml=-1, and ms=+1/2 for both boron and nitrogen is not enough to get the answer right. The question is asking for a complete set of values for all the electrons in the ground state of each atom. I hope this explanation helps clarify the problem.