What are the values of NLM and S if the electron is present in the 3s orbital?

n = 3 , 1 = 0 , m = 0 , s = -1⁄2 for second electron.

What are the values of NLM for 4f orbital?

For a 4f orbital, the principal quantum number is n = 4, the azimuthal quantum number is 3. The values of magnetic quantum numbers will be -3, -2, -1, 0, +1, +2, +3. Total 7 orbitals are present in 4f subshell. Each orbital can contain two electrons which are present in opposite directions.

What are the possible m values for an electron in 4th shell?

– So, the value of ℓ will range from 0 to 3. So, the total number of orbitals is 16. Hence, the total value of m for the electrons (n=4) is option (C) 16. – The Aufbau Principle states that the electrons are filled in the increasing order of the energy of the orbitals.

What are the possible values of quantum numbers for an electron in a 4 d orbital?

For a 4d orbital, the value of n (principal quantum number) will always be 4 and the value of l (azimuthal quantum number) will always be equal to 2. The values of the magnetic quantum number range from -l to l, so the possible values of ml for the 4d orbital are -2, -1, 0, 1, and 2.

What are the values of NLM for 3p orbitals?

for 3p-orbitals,, n=3, l=1 and m=+1,0,-1.

What is the only possible value of MLML for an electron in an s orbital express your answer numerically?

apply the quantum number rules for an electron in an atom. For an s orbital, the only possible value for ml is 0. For a d orbital, the values of ml are: -2, -1, 0, +1, and +2. Finally, the sets that apply for an electron in an atom are a., c., and d.

What are N and L value for an electron present in 4f?

The values of all the quantum numbers for 4f subshell is, n = 4, l = 3, Explanation : Principle Quantum Numbers : It describes the size of the orbital.

What are the value of N and L for 4f orbital?

n=4,l=0,1, m1=−1,0,+1.

What are the values of NLM?

Here n = represent the principal quantum number,

What is the possible values of S?

(b) The quantum numbers associated with the total spin angular momentum will range from a maximum value found by adding the individual quantum numbers together to a minimum value found by taking the absolute value of the difference of the two numbers in integer steps. The possible values for S are 0 and 1.

What is are the possible value S of the L quantum number if the n quantum number is 3?

0
What is the name of the oribital(s) with quantum number n=3? 3s, 3p, and 3d. Because n=3, the possible values of l = 0, 1, 2, which indicates the shapes of each subshell.