This is actually pretty simple, so I\'ll help explain. Take a given hydrogen atom, but we\'ll use an ionic form that has 5 electrons (as you\'ve stated). Now, for the quantum numbers. The first one, N, is the electron shell in question. Shells work as providing spaces for electron density. The first shell, in which N=1, holds two electrons because it only contains one orbital. N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number of electrons before entering the third shell. Because the ion in question has 5 electrons, its N value is 2. A simple way to calculate the maximum number of electrons in a given atom that occupies a specific shell is to take that shell number, N, square it and multiply the result by two. That is why the maximum quantum number N for an atom whose electrons occupy the third shell is 18 (which is (3^2)2). Onto the next quantum number, which is l. If you understand the order of atomic shells and their orbitals, this is a simple one. The first shell is l=0, which is the \"s\" shell of an atom. s shells can only hold one atomic orbital, which is two electrons. We denote this as \"1s2\". The next shell is 2s, and because we can fill it, it become 2s2.Because we have 5 electrons, we need to keep going up. The next shell is l=1, which is the \"p\" shell. That fits our last electron, so your value for the l quantum number is \"1.\" Now we\'re at the ml quantum number. These are the numbers we assign to the specific orbitals in which electrons reside in, within a given shell. We\'re currently in the p shell, which holds 3 orbitals whose names are -1, 0, and +1. Unless you have a picture of the electron shells, we can only guess that the 5th electron is in any one of these, so the safe bet is to put it into the -1 orbital (though it can really be in any of them). Lastly, the ms quantum number. This denotes the spin on the electron. Up spin is +1/2, whilst down spin is -1/2. Unless you have a picture, I can\'t tell you which way it is spinning, but it\'s a safe guess to say that it\'s up. In sum, your quantum numbers as: 2, 1, 0, (1/2) I hope that helps. (: Feel free to ask any questions. Solution This is actually pretty simple, so I\'ll help explain. Take a given hydrogen atom, but we\'ll use an ionic form that has 5 electrons (as you\'ve stated). Now, for the quantum numbers. The first one, N, is the electron shell in question. Shells work as providing spaces for electron density. The first shell, in which N=1, holds two electrons because it only contains one orbital. N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number of electrons before entering the third shell. Because the ion in question has 5 electrons, its N value is 2. A simple way to calculate the maximum number of electrons.

1. This is actually pretty simple, so I'll help explain.
Take a given hydrogen atom, but we'll use an ionic form that has 5 electrons (as you've stated).
Now, for the quantum numbers.
The first one, N, is the electron shell in question. Shells work as providing spaces for electron
density. The first shell, in which N=1, holds two electrons because it only contains one orbital.
N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has
anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number
of electrons before entering the third shell. Because the ion in question has 5 electrons, its N
value is 2.
A simple way to calculate the maximum number of electrons in a given atom that occupies a
specific shell is to take that shell number, N, square it and multiply the result by two. That is why
the maximum quantum number N for an atom whose electrons occupy the third shell is 18
(which is (3^2)2).
Onto the next quantum number, which is l. If you understand the order of atomic shells and their
orbitals, this is a simple one.
The first shell is l=0, which is the "s" shell of an atom. s shells can only hold one atomic
orbital, which is two electrons. We denote this as "1s2". The next shell is 2s, and because we
can fill it, it become 2s2.Because we have 5 electrons, we need to keep going up. The next shell
is l=1, which is the "p" shell. That fits our last electron, so your value for the l quantum number
is "1."
Now we're at the ml quantum number. These are the numbers we assign to the specific orbitals
in which electrons reside in, within a given shell. We're currently in the p shell, which holds 3
orbitals whose names are -1, 0, and +1. Unless you have a picture of the electron shells, we can
only guess that the 5th electron is in any one of these, so the safe bet is to put it into the -1 orbital
(though it can really be in any of them).
Lastly, the ms quantum number. This denotes the spin on the electron. Up spin is +1/2, whilst
down spin is -1/2. Unless you have a picture, I can't tell you which way it is spinning, but it's a
safe guess to say that it's up.

2. In sum, your quantum numbers as: 2, 1, 0, (1/2)
I hope that helps. (: Feel free to ask any questions.
Solution
This is actually pretty simple, so I'll help explain.
Take a given hydrogen atom, but we'll use an ionic form that has 5 electrons (as you've stated).
Now, for the quantum numbers.
The first one, N, is the electron shell in question. Shells work as providing spaces for electron
density. The first shell, in which N=1, holds two electrons because it only contains one orbital.
N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has
anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number
of electrons before entering the third shell. Because the ion in question has 5 electrons, its N
value is 2.
A simple way to calculate the maximum number of electrons in a given atom that occupies a
specific shell is to take that shell number, N, square it and multiply the result by two. That is why
the maximum quantum number N for an atom whose electrons occupy the third shell is 18
(which is (3^2)2).
Onto the next quantum number, which is l. If you understand the order of atomic shells and their
orbitals, this is a simple one.
The first shell is l=0, which is the "s" shell of an atom. s shells can only hold one atomic
orbital, which is two electrons. We denote this as "1s2". The next shell is 2s, and because we
can fill it, it become 2s2.Because we have 5 electrons, we need to keep going up. The next shell
is l=1, which is the "p" shell. That fits our last electron, so your value for the l quantum number
is "1."
Now we're at the ml quantum number. These are the numbers we assign to the specific orbitals
in which electrons reside in, within a given shell. We're currently in the p shell, which holds 3
orbitals whose names are -1, 0, and +1. Unless you have a picture of the electron shells, we can

3. only guess that the 5th electron is in any one of these, so the safe bet is to put it into the -1 orbital
(though it can really be in any of them).
Lastly, the ms quantum number. This denotes the spin on the electron. Up spin is +1/2, whilst
down spin is -1/2. Unless you have a picture, I can't tell you which way it is spinning, but it's a
safe guess to say that it's up.
In sum, your quantum numbers as: 2, 1, 0, (1/2)
I hope that helps. (: Feel free to ask any questions.