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What are the possible values of ml if the l quantum number is 5?
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Which quantum number specifies the direction of an electron's angular momentum?
"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.
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.
The numeric values of the magnetic quantum number is zero for pz?
Yes, it would be pz: ml= 0, px: ml=-1 and py: +1
What would the fourth quantum number of a 1 S 2 electron be?
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 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 ml for an electron in a d orbital?
2,1,0,-1,-2 are the possible values of ml for an electron in d orbital.
What is the set of quantum number for 4d orbital?
n (principle quantum number) = 4 l (angular momentum quantum number) = 2 ml (magnetic quantum number) = -2, -1, 0, 1, or 2 ms (spin quantum number) = +1/2 or -1/2
What does a quantum number describe?
n is the first quantum number. It is the principle quantum number. It refers to what energy level it is and will be one greater than the number of nodes in the orbital. l is the second quantum number. It is the angular momentum quantum number and refers to the shape of the orbital. ml is the third quantum number. It is the magnetic quantum number and it refers to the orientation of the orbital. ms is the fourth quantum number. It is the spin quantum number and refers to the magnetic character of the orbital.
Is Magnetic quantum number ever larger than the principle quantum number?
No, for any given electron, the principle quantum number will be larger. For example, a second shell, p-subshell electron will have the quantum numbers {2, 1, ml, ms} where mlcan be -1, 0, or 1 and, as always, ms can be ½ or -½. The largest ml can be is +1, which is smaller than the principle quantum number, 2.
What is the second quantum number of a 2s2 electron in phosphorus 1s22s22p63s23p3?
ml=0
What does the third quantum number (ml) describe?
The specific orbital within a sublevel
What could be a third quantum number of a 2p3 electron in phosphorus?
ml = -1
