Home
Class 12
CHEMISTRY
Find the value of n+l of the orbital 2S....

Find the value of `n+l` of the orbital 2S.

A

`1`

B

`2`

C

`3`

D

None of these

Text Solution

AI Generated Solution

The correct Answer is:
To find the value of \( n + l \) for the orbital 2s, we will follow these steps: ### Step-by-Step Solution: 1. **Identify the Principal Quantum Number (n)**: - The principal quantum number \( n \) indicates the energy level of an electron in an atom. For the orbital 2s, the principal quantum number is 2. - Therefore, \( n = 2 \). 2. **Identify the Azimuthal Quantum Number (l)**: - The azimuthal quantum number \( l \) defines the shape of the orbital. The value of \( l \) can take on integer values from 0 to \( n-1 \). - For s orbitals, \( l \) is always 0. Thus, for the 2s orbital, \( l = 0 \). 3. **Calculate \( n + l \)**: - Now that we have both \( n \) and \( l \), we can calculate \( n + l \): \[ n + l = 2 + 0 = 2 \] 4. **Conclusion**: - The value of \( n + l \) for the orbital 2s is 2. ### Final Answer: The value of \( n + l \) for the orbital 2s is **2**. ---
To find the value of \( n + l \) for the orbital 2s, we will follow these steps: ### Step-by-Step Solution: 1. **Identify the Principal Quantum Number (n)**: - The principal quantum number \( n \) indicates the energy level of an electron in an atom. For the orbital 2s, the principal quantum number is 2. - Therefore, \( n = 2 \). ...
Promotional Banner

Similar Questions

Explore conceptually related problems

An orbital has only positive values of wave function at all distances from the nucleus. Find the value of (n+l) for this orbital.

Find the value of the following. 2lm + 61 - 5m-n for l = 5, m = 2, n = -2

The arrangement of orbitals on the basis of energy is based upon their (n+l) value. Lower the value of (n+l), lower is the energy . For orbitals having same values of (n+l). The orbital with lower value of n will have lower energy. I. Based upon the above information arrange the following orbitals in the increasing order of energy. (a) 1s,2s,3s,2p (b) 4s,3s,3p,4d (c) 2p,4d,5d,4f,6s (d) 5f,6d,7s,7p II. Based upon the above information Solve the question. give below. (a) which of the following orbitals has the lowest energy 4d,4f,5s,5p (b) which of the following orbitals has the highest energy? 5p,5d,5f,6s,6p

What are the values of the orbital angular momentum of an electron in the orbitals 1s,3s,3d and 2p :-

n, l and m values of the 2p_(z) orbital are

Menstion the values of n and l corresponding to the following orbitals. (a) 2s (b) 2p (c ) 3d (d) 4f ( e) 3s

If S_(n) = 1 + (1)/(2) + (1)/(2^(2))+….+(1)/(2^(n-1)) , find the least value of n for which 2- S_(n) lt (1)/(100) .

(a) An atomic orbital has n=3. What are the possible values of l? (b) An atomic orbital has l=3. What are the possible values of m? (c ) An atomic orbital has n=2. What are the possible values of l and m?

If the value of (n + l) is more than 3 and less than 6 , then what will be the possible number of orbitals ?

Azimuthal quantum number (l) : It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1) {:("Value of l",0,1,2,3),("subshell",s,p,d,r):} Number of orbitals in a subshell =2l+1 Orbital angular momentum L =h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)] Magnetic quantum number (m) : It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals (p_x ,p_y and p_z) , d-subshell five orbitals (d_"xy", d_"yz",d_(x^2-y^2), d_z^2) and f-subshell has seven orbitals. Spin quantum number (s) : It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis. Spin of the electron produces angular momentum equal to S=sqrt(s(s+1)) h/(2pi) where s=+1/2 Total spin of an atom =+n/2 or -n/2 (where n is the number of unpaired electron ) The magnetic moment of an atom mu_s=sqrt(n(n+2)) B.M. n=number of unpaired electrons B.M. (Bohr magneton) Orbital angular momentum of an electron is sqrt3h/pi then the number of orientations of this orbital in spaces are :