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The following quantum numbers are possib...

The following quantum numbers are possible for how many orbitals `(s) n = 3, l = 2, m = + 2` ?

A

1

B

3

C

2

D

4

Text Solution

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The correct Answer is:
To determine how many orbitals correspond to the given quantum numbers \( n = 3 \), \( l = 2 \), and \( m = +2 \), we can follow these steps: ### Step 1: Understand the Quantum Numbers - The principal quantum number \( n \) indicates the energy level of the electron. Here, \( n = 3 \) means we are in the third energy level. - The azimuthal quantum number \( l \) indicates the shape of the orbital. For \( l = 2 \), this corresponds to the d orbitals. - The magnetic quantum number \( m \) indicates the orientation of the orbital in space. The possible values of \( m \) range from \( -l \) to \( +l \). ### Step 2: Determine the Possible Values of \( m \) - For \( l = 2 \), the possible values of \( m \) are: \[ m = -2, -1, 0, +1, +2 \] - This gives us a total of 5 possible orientations for the d orbitals. ### Step 3: Identify the Validity of the Given \( m \) - The question specifies \( m = +2 \). This is one of the valid values of \( m \) for \( l = 2 \). - Since \( m = +2 \) corresponds to one specific orientation of the d orbital, it indicates that there is only one orbital that can have this orientation. ### Conclusion - Therefore, the number of orbitals corresponding to the quantum numbers \( n = 3 \), \( l = 2 \), and \( m = +2 \) is **1**. ### Final Answer The answer is **1 orbital**. ---
To determine how many orbitals correspond to the given quantum numbers \( n = 3 \), \( l = 2 \), and \( m = +2 \), we can follow these steps: ### Step 1: Understand the Quantum Numbers - The principal quantum number \( n \) indicates the energy level of the electron. Here, \( n = 3 \) means we are in the third energy level. - The azimuthal quantum number \( l \) indicates the shape of the orbital. For \( l = 2 \), this corresponds to the d orbitals. - The magnetic quantum number \( m \) indicates the orientation of the orbital in space. The possible values of \( m \) range from \( -l \) to \( +l \). ### Step 2: Determine the Possible Values of \( m \) ...
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The following quantum numbers are possible for how many orbitals? n = 3, I= 2, m = +2.

The electron are distributed around the nucleus in various energy levels shells, subshells and orbitals. A set of quantum numbers completely describe the position and total energy of electron in an atom. The various permitted values of quantum numbers are : principal, n = 1,2,3,4...... azimuthal , l = 0,1,2,....(n -1) magnetic, m_l = -l .....0 .....+ l spin, m_s = +1//2 and -1//2 . Is the following set of quantum numbers possible or not ? n = 3, l = 2, m = 0, s = -1//2 .

Knowledge Check

  • The following quantum numbers are possible for how many orbitals ? n = 3, l = 2, n + 2

    A
    1
    B
    2
    C
    3
    D
    4

  • Quantum number n = 3,l = 2, m= +2 shows how many orbitals

    A
    1
    B
    2
    C
    3
    D
    4

    • Similar Questions

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    What of the following sets of quantum numbers are not possible? (i) n = 3, l = 2, m = 0, s = -1//2 (ii) n = 3, l = 2, m = -2, s = -1//2 (iii) n = 3, l = 3, m = -3, s = +1//2 (iv) n = 3, l = 1, m = 0, s + 1//2

    How many electrons in a given atom can have the following quantum numbers ? (a) n = 3, l = 1 (b) n = 3, l = 2, m_l = 0 (c ) n = 3, l = 2, m_l = +2, m_s = + 1/2 (d) n = 3 .

    Explain given 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 = 2",", m_l=0",", m_s = + 1//2):}

    Using the s,p,d notations, describe the orbital with the following quantum numbers : (a) n = 1, l = 0 " " (b) n = 3, l = 2 (c ) n = 3, l = 1 " " (d) n = 2, l = 1 (e ) n = 4, l = 3 " " (f) n = 4, l = 2 .

    Explain, giving reasons, which of the following sets of quantum numbers are not possible. (a) n=0, l=0, m_(1)=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

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