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Just two, +1/2, -1/2. These correspond to electrons of opposite spin.
Gonzalo Abernathy
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What is need of Spin quantum number?
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.
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.
If the principle quantum number is 3 what possible values can azimuthal quantum number have?
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.
How many possible values are there for the spin quantum number?
two --- + 1/2 or - 1/2
How many possible values are there for spin numbers?
the spin quantum number has only two possible values__(+ 1/2 & -1/2)
How many orbitals in the fourth energy level?
The atomic states with principal quantum number 4 can have orbital angular momentum quantum numbers from -4 to 4. Hence there are 9 possible values of the orbital angular momentum quantum number. Each electron can have spin +1/2 or -1/2, so each of the states specified by a given orbital angular momentum quantum number can have at most two electrons in the state without violating Pauli's exclusion principle. So, in sum, there are 18 possible states for an electron with principal quantum number 4.
What are the possible values of ml for an electron in a d orbital?
The possible values of ml for an electron in a d orbital range from -2 to +2. This corresponds to the five orbitals in a d subshell: dz^2, dx^2-y^2, dxz, dyz, and dxy. Each orbital can hold up to two electrons with opposite spins.
How many electrons can have the quantum numbers n 5 ℓ 0 ml0?
There can be two electrons with those quantum numbers in an atom. Each electron is completely described by four quantum numbers. The one that's missing in the list provided is ms, which can have only two possible values (+1/2 and -1/2).
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.
A quantum of energy as defined in the Quantum Mechanical Model is a?
A quantum of energy in the Quantum Mechanical Model is the minimum amount of energy that can be gained or lost by an atom. It is quantized, meaning it can only exist in specific discrete amounts. This concept helps explain the discrete energy levels of electrons in atoms.
The numerical values of the magnetic quantum number m1 depends on the?
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.
What would the fourth quantum number of a 1 S 2 electron be?
The fourth quantum number is the electron spin quantum number, denoted by (m_s). For a 1S orbital with 2 electrons, the electron spin quantum numbers of the two electrons would be (m_s = +\frac{1}{2}) and (-\frac{1}{2}) according to the Pauli exclusion principle.
