The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) where l is the azimuthal, angular momentum quantum number.
The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n.
The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell.
The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1). ml "defines " the shape of the orbital and the number within the subshell.
As an example for a d orbital (l=2), the values are -2, -1, 0, +1, +2, , so 5 d orbitals in total.
They act as codes that provide information about each electron in an atom.
n - energy level (can be 1,2,3…)
l - orbital shape (s=0, p=1, d=2)
ml - orbital orientation (goes from -/to +/by integers)
ms - spin (arrow up or down, and can be either +½ or -½)
The names of the quantum numbers are:
Principal Quantum number (n)
Angular Momentum Quantum Number (l)
Magnetic Quantum Number (m)
Spin Quantum Number (+1/2 and -1/2)
The "n" gives the energy level of the electron then the "l" which is the sublevel then "m" which tells you which orbital it is in and last "s" which tells you if the electron is going to have a positive or negative 1/2 spin
There are 4 quantum numbers, n, l, ml, ms
They have long names respectively principal, azimuthal (angular momentum), magnetic and spin.
n can have values 0, 1, 2, 3, 4, 5......
l depends on n, and can have values, 0 to (n-1) (0 is an s orbital, 1 is a p subshell, 2 is a d subshell, 3 is a f subshell etc
ml can have -l to +l (sorry this font is rubbish the letter l looks like a 1) so for a d subshell, where l = 2, it can be -2, -1, 0, +1, +2. Five d orbitals in all.
ms can be -1/2 or +1/2 (These are the maximum of 2 electrons having opposite spin)
n = 2, l = 0, ml = 0
n = 1, l = 0, ml = 0
n = 3, l = 1, ml = -1
n = 2, l = 1, ml = -1
or
n = 3, l = 2, ml = 1
n = 3, l = 2, ml = -2
B.n = 2, l = 0, ml = 0
C.n = 1, l = 0, ml = 0
D.n = 3, l = 1, ml = -1
1. Principle Quantum Number (n)- Distance from the nucleus
For example, when you do the ground state configuration: 1s2 2s2 2p6
The first number (1,2,2) represents the distance from the nucleus
2. Orbital Quantum Number (l)- Shape of the orbital
s-0 p-1 d-2 f-3
3. Magnetic Quantum Number (m)- Indicates a particular suborbital; orientation of the orbital in space
For example, the p shells have 3 orbitals. The first is -1, the second is
0, and the third is 1
4. Spin Quantum Number (s)- Spin of the electron; clockwise or counterclockwise (1/2 or -1/2)
If it is the first electron in the suborbital, it is +1/2 if it is the second,
it is -1/2
Theoretically, n can be any integer greater than 0
n= 1, 2, 3, 4,....
However, in the ground staes of the elements it is between 1 and 7.
"n" is the principal quantum number, which indicates the shell an electron occupies. A higher shell number means that an electron is further away from the nucleus, and therefore has greater energy. Because atoms can only get so large before breaking apart, the "n" number is limited to about 7 for the largest known atoms.
To determine what n is for a particular electron in an atom, you need to understand the electron configuration of atoms. You may be familiar with something like this:
1s22s22p63s23p64s23d104p6....
This is one way to show the electron configuration of an atom. The large numbers are the shell numbers, the letters indicate the sub-shell, and the superscript numbers show how many electrons are in that particular sub-shell of that particular shell. The shell number is equal to the principal quantum number (n).
For instance, the outermost electron in a Lithium atom (with three total electrons) would be in Shell #2, because the first two electrons filled up Shell #1. Therefore, the principal quantum number for the outermost electron in a Lithium atom is n=2.
If you've never learned or have forgotten electron configuration, you need to review it before trying to find n for a particular electron.
Hope this helps!
all the non-negative integers: 0,1,2,..., n-1, where n is a principal quantum number
The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n. The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell. The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) so for an f orbital the values are -3. -2, -1, 0, +1, +2, +3, so 7 f orbitals in total. ml "defines " the shape of the orbital and the number within the subshell.
two --- + 1/2 or - 1/2
The spin quantum number was created in the early twentieth century to account for the magnetic properties of the electron. It has only two possible values, +1/2 and -1/2, which indicates the two possible spin states of the electron. A single orbital can hold up to 2 electrons, which must have opposite spin states.
In theory, the number of electrons with each quantum number is not limited. However, for any given "main quantum number" (n), the number of electrons having the other quantum numbers is limited - but it depends on the value of "n". For more information, the Wikipedia article on "quantum number" seems to give a good overview.
Possible values of quantum numbers in order of n,l,m,s in the second shell:2,0,0,-1/22,0,0,+1/22,1,-1,-1/22,1,-1,+1/22,1,0,-1/22,1,0,+1/22,1,1,-1/22,1,1,+1/2
The values of the magnetic quantum number depend on the value of the azimuthal quantum number (orbital angular momentum quantum number) and has values -l, .. 0 . ..+l l=1, p orbital, -1, 0, +1 - three p orbitals l=2 d orbital -2, -1, 0., +1,+2 five d orbitals etc.
"l" is known as the angular momentum quantum number. Principal Quantum Number = n Angular Momentum " " = l Magnetic " " = ml Spin " " = ms (Only possible values are 1/2 and -1/2) Search "Permissible Values of Quantum Numbers for Atomic Orbitals" for the values. You basically have to understand the concepts & be able to recreate the chart for tests, otherwise you can blindly memorize it. The chart should be in your book.
For a principle quantum number 3, there are three possible sub-shells. These are 3s, 3p, 3d. Azimuthal quantum no. is less than principle quantum number. There for 3s it is 0, for 3p it is 1, for 3d it is 2.
The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n. The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell. The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) so for an f orbital the values are -3. -2, -1, 0, +1, +2, +3, so 7 f orbitals in total. ml "defines " the shape of the orbital and the number within the subshell.
two --- + 1/2 or - 1/2
-l to l, so given l=2 (d orbital) the values for ml will be -2, -1, 0, +1, +2
Yes, it would be pz: ml= 0, px: ml=-1 and py: +1
the spin quantum number has only two possible values__(+ 1/2 & -1/2)
The spin quantum number was created in the early twentieth century to account for the magnetic properties of the electron. It has only two possible values, +1/2 and -1/2, which indicates the two possible spin states of the electron. A single orbital can hold up to 2 electrons, which must have opposite spin states.
Just two, +1/2, -1/2. These correspond to electrons of opposite spin.
Either +1/2 or -1/2; the fourth quantum number is ALWAYS either +1/2 or -1/2 and it's not generally possible to say which (other than that two electrons in the same atom which have the same first three quantum numbers will always have different values for the fourth).
What are all the possible whole number values for 7