Home
Class 12
CHEMISTRY
The quantum number of four electrons are...

The quantum number of four electrons are given below:
`n=4,l=2,m_(l)=-2,m_(s)=-1//2`
`n=3,l=2,m_(l),m_(s)=+1//2`
`n=4,l=1,m_(l)=0,m_(s)=+1//2`
`n=3,l=1,m_(l)=1,m_(s)=-1//2`
The correct order of their increasing energies will be:

A

`IVltIIltIIltI`

B

`IltIIltIIIltIV`

C

`IVltIIltIIIltI`

D

`IltIIIltIIltIV`

Text Solution

AI Generated Solution

The correct Answer is:
To determine the increasing order of energy for the given electrons based on their quantum numbers, we will follow these steps: ### Step 1: Identify the Quantum Numbers We have the following quantum numbers for the four electrons: 1. Electron 1: \( n = 4, l = 2, m_l = -2, m_s = -\frac{1}{2} \) 2. Electron 2: \( n = 3, l = 2, m_l = ?, m_s = +\frac{1}{2} \) 3. Electron 3: \( n = 4, l = 1, m_l = 0, m_s = +\frac{1}{2} \) 4. Electron 4: \( n = 3, l = 1, m_l = 1, m_s = -\frac{1}{2} \) ### Step 2: Calculate \( n + l \) for Each Electron Using the \( n + l \) rule, we can calculate the energy levels: - For Electron 1: \( n + l = 4 + 2 = 6 \) - For Electron 2: \( n + l = 3 + 2 = 5 \) - For Electron 3: \( n + l = 4 + 1 = 5 \) - For Electron 4: \( n + l = 3 + 1 = 4 \) ### Step 3: Compare \( n + l \) Values Now, we compare the \( n + l \) values to determine the order of increasing energy: - Electron 4: \( n + l = 4 \) (Lowest energy) - Electron 2: \( n + l = 5 \) - Electron 3: \( n + l = 5 \) - Electron 1: \( n + l = 6 \) (Highest energy) ### Step 4: Determine the Order of Increasing Energy Since Electrons 2 and 3 have the same \( n + l \) value, we need to consider the principal quantum number \( n \) to determine their relative energies: - Between Electron 2 (\( n = 3 \)) and Electron 3 (\( n = 4 \)), Electron 2 will have lower energy because it has a lower \( n \). Thus, the order of increasing energy is: 1. Electron 4 (\( n = 3, l = 1 \)) 2. Electron 2 (\( n = 3, l = 2 \)) 3. Electron 3 (\( n = 4, l = 1 \)) 4. Electron 1 (\( n = 4, l = 2 \)) ### Final Answer The correct order of increasing energies is: **Electron 4 < Electron 2 < Electron 3 < Electron 1**
Promotional Banner

Topper's Solved these Questions

  • JEE MAINS

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise QUESTION|1 Videos

  • JEE MAIN

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise CHEMISTRY|146 Videos

  • JEE MAINS 2020

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise CHEMSITRY|23 Videos

Similar Questions

Explore conceptually related problems

The quantum number of four electrons are given below: I. n=4,l=2,m_l=-2,m_s=-1/2 II. n=3,l=2,m_l=1,m_s=+1/2 III. n = 4 , l =1 ,m _l=0 ,m_s=+1/2 IV. n=3,l=1,m_l=1,m_s=-1/2 The correct order of their increasing energies will be

The quantum numbers for the outer electrons of an atom are given by n = 2, l = 0, m = 0, s = +1//2

From the following sets of quantum numbers , state which are possible ? (i) n=0,l=0,m_(l)=1,m_(s)= +1//2 (ii) n=2,l=1,m_(l)=0,m_(s) = -1//2 (iii) n=2, l=0,m_(1)=3,m_(s) = +1//2 (iv) n=3,l=1,m_(l)=0,m_(s) = +1//2

The quantum number of electrons are given below: Arrange then in order of increasing energies a. n= 4,l= 2,m_(1)= -2, m_(s)= -(1)/(2) b. n= 3,l= 2,m_(1) = 1, m_(s)= +(1)/(2) c. n= 4,l= 1,m_(1) = 0, m_(s)= +(1)/(2) e.n= 3,l= 2,m_(1)= -2, m_(s)= +(1)/(2) f. n= 4,l= 1,m_(1) = +1, m_(s)= +(1)/(2)

Explain giving reasons, which of the following sets of quantum numbers are not possible? (a) n=0, l=0, m_(l)=0, m_(s)=+1/2 (b) n=1, l=0, m_(l)=0, m_(s)=-1/2 (c) n=1, l=1, m_(l)=0, m_(s)=+1/2 (d) n=2, l=1, m_(l)=0, m_(s)=-1/2 (e) n=3, l=3, m_(l)=-3, m_(s)=+1/2 (f) n=3, l=1, m_(l)=0, m_(s)=+1/2

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists: 1. n=4 , l=2 , m_(i) =-2, m_(s) =-1//2 2. n=3 , l=2 , m_(l) =1 , m_(s) =+1//2 3. n=4 , l=2 ,m_(l)=-2, m_(s) =-1//2 4. n=3 , l= 2, m_(i) =-1 , m_(s) = +1//2 5. n=3 , l=1 , m_(l) =-1 , m_(s) = +1//2 6. n=4 , l= 1 , m_(l) =0 , m_(s) =+1//2

The maximum number of electron inm n = 1,l = 0, m = 0,s= +- 1//2 is ……….

Explain , giving reason , which of the following sets of quantum number are not possible {:(a,n= 0 ,l = 0, m_(1) = 0, m_(s) = +1//2),(b,n= 1 ,l = 0, m_(1) = 0, m_(s) = -1//2),(c,n= 1 ,l = 1, m_(1) = 0, m_(s) = +1//2),(d,n= 2 ,l = 1, m_(1) = 0, m_(s) = -1//2),(e,n= 3 ,l = 3, m_(1) = -3, m_(s) = +1//2),(f,n= 3 ,l = 1, m_(1) = 0, m_(s) = +1//2):}

State which of the following sets of quantum number would be possible and which would not be permisible for an electron in an atom. (i) n=3,I=3,m_(l)=+3, m_(s)=+(1)/(2) (ii) n=3,I=3,m_(l)=+1, m_(s)=-(1)/(2) (iii) n=5,I=4,m_(l)=+3, m_(s)=(1) (iv) n=0,I=0,m_(l)=0, m_(s)=+(1)/(2) (v) n=4,I=3,m_(l)=-2, m_(s)=-(1)/(2)

In an atom, the total number of electrons having quantum number n = 4, |m_(l)| = 1 and m_(s) = - (1)/(2) is