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What are the possible values of ml for an electron in a d orbital?
Wiki User
∙ 9y ago
2,1,0,-1,-2 are the possible values of ml for an electron in d orbital.
Wiki User
∙ 9y ago
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What electron could have quantum numbers n 3 l 0 ml 0 ms?
A 3s electron
How many outer electrons does Rb have?
It outermost electron in Krypton is 4s1 so the quantum number set is: n l ml ms 4 0 0 1/2 n= principal quantum number l- angular shapes of the lob ml- orientation of the lobe ms- magnetic spin of the lobe , which always alternates between the values 1/2 and -1/2 Note that the quantum number l is always zero for the s orbital because there are only one subshell.
What will be the value of magnetic quantum number if the value of azimuthal quantum number is given to you?
-l to l, so given l=2 (d orbital) the values for ml will be -2, -1, 0, +1, +2
What does the third quantum number (ml) describe?
The specific orbital within a sublevel
What does the second quantum number?
It's the azimuthal quantum number. It specifies the angular momentum of the orbital, which can broadly speaking be thought of as its "shape." (The reason I'm putting that in quotation marks is that it's possible for two orbitals with the same azimuthal quantum number to appear rather different in overall shape.)
Values of n l and ml of 2p orbital?
n : 2 l : 1 ml : -1, 0, or 1
What is the maximum value that m can have for a 3d orbital?
For the d orbital, the value of l is 2 and the value of ml is - l to + l, so the values of ml would be -2, -1, 0, +1, +2. So, the maximum value would be +2.
What electron could have quantum numbers n 3 l 0 ml 0 ms?
A 3s electron
What are the possible values of the magnetic quantum number ml?
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.
How many qantum numbers are used to describe each electron?
Four: Principal (n) - shell Azimuthal (l) - subshell Magnetic (ml or just m) - orbital orientation Spin (ms or just s) - electron's angular momentum
What is the quantum number set of the ground-state electron that is found in helium but not in hydrogen?
The quantum number set of the ground-state electron in helium, but not in hydrogen, is (1s^2) or (n=1, l=0, ml=0, ms=0). It indicates that the electron occupies the 1s orbital, which has a principal quantum number (n) of 1, an orbital angular momentum quantum number (l) of 0, a magnetic quantum number (ml) of 0, and a spin quantum number (ms) of 0.
What is the difference between two isotopes of an electron?
There is no difference. Electrons are subatomic particles and therefore identical.Added:In the same orbital, defined by one 'tri' set of quantum numbers (n, l, and ml ) the spin quantum number differs, the two values being ms = +1/2 and ms = -1/2, are each taken by one electron.
What quantum number tell us the spin of an electron?
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)
How many outer electrons does Rb have?
It outermost electron in Krypton is 4s1 so the quantum number set is: n l ml ms 4 0 0 1/2 n= principal quantum number l- angular shapes of the lob ml- orientation of the lobe ms- magnetic spin of the lobe , which always alternates between the values 1/2 and -1/2 Note that the quantum number l is always zero for the s orbital because there are only one subshell.
What will be the value of magnetic quantum number if the value of azimuthal quantum number is given to you?
-l to l, so given l=2 (d orbital) the values for ml will be -2, -1, 0, +1, +2
What are the possible values of the magnetic quantum number?
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.
What does the third quantum number (ml) describe?
The specific orbital within a sublevel
