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(A) : For n = 3, 1 may be 0,1,2 and .m. ...

(A) : For n = 3, 1 may be 0,1,2 and .m. may be 0, (`+-2, +-1` and 0)
(R) : For each value of n there are 0 to (n-1) possible values of 1 and for each value of l values of .m. are -1….0….+1

A

Both (A) and (R) are true and (R) is the correct explanation of (A)

B

Both (A) and (R) are true and (R) is not the correct explanation of (A)

C

(A) is true but (R) is false

D

(A) is false but (R) is true

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The correct Answer is:
A
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(A) : For n = 3,l may be 0,1,2 and 'm' may be 0, (+-1 and 0), ( +- 2, +-1 and 0) (R) : For each value of n there are 0 to (n-1) possible values of 1. For each value of 1 'm' values are -1…..0,…..+1

How many orbitals is/are possible with n=3 l-1 and m_(1) = -1 value ?

The equation of Schroedinger for the hydrogen atom in the time-independet, non-relativistic form is a partial differential equation involving the position coordinates (x, y and z). The potential energy term for the proton-electron system is spherically symmetric of the form -1//4pi in_(0) xx (e^(2)//r) . THus it is advantages to change over from the cartesian coordinates (x,y and z) to the spherical polar coordinates, (r, theta and phi ). In this form the equation become separable in the radial part involving r and the angular part involving theta and phi . The probability of locating the electron within a volume element d tau = 4pi r^(2)dr is then given |Psi|^(2)(4pir^(2)dr) , where Psi is a function of r, theta and phi . With proper conditions imposed on Psi , the treatment yields certain functions, Psi , known as atomic orbitals which are solutions of the equations. Each function Psi correspods to quantum number n, l and m, the principal, the azimuthal and the magnetic quantum number respectively, n has values 1, 2, 3,...., l has values 0, 1, 2, ....(n-1) for each value of n and m (n-1) for each value of n and m (m_(l)) has values =1, +(l+1),...1,0,-1,-2...-l i.e., (2l+1) values for each value of l. In addition a further quantum number called pin had to be introduced with values +-1//2 . Any set of four values for n, l , m and s characterizes a spin orbital. Pauli.s exclusion principle states that a given spin orbital can accomodate not more than electron. Further the values l = 0, l=1, l=2, l=3 are designated s,p,d and f orbitals respectively. It is a basic fact that any two electrons are indistinguishable. 3 electrons are to be accomodated in the spin orbitals included under the designated 2p, conforming to the Pauli principle. Calculate the number of ways in which this may be done.

The equation of Schroedinger for the hydrogen atom in the time-independet, non-relativistic form is a partial differential equation involving the position coordinates (x, y and z). The potential energy term for the proton-electron system is spherically symmetric of the form -1//4pi in_(0) xx (e^(2)//r) . THus it is advantages to change over from the cartesian coordinates (x,y and z) to the spherical polar coordinates, ( r, theta and phi ). In this form the equation become separable in the radial part involving r and the angular part involving theta and phi . The probability of locating the electron within a volume element d tau = 4pi r^(2)dr is then given |Psi|^(2)(4pir^(2)dr) , where Psi is a function of r, theta and phi . With proper conditions imposed on Psi , the treatment yields certain functions, Psi , known as atomic orbitals which are solutions of the equations. Each function Psi correspods to quantum number n, l and m, the principal, the azimuthal and the magnetic quantum number respectively, n has values 1, 2, 3,...., l has values 0, 1, 2, ....(n-1) for each value of n and m (n-1) for each value of n and m (m_(l)) has values =1, +(l+1),...1,0,-1,-2...-l i.e., (2l+1) values for each value of l. In addition a further quantum number called pin had to be introduced with values +-1//2 . Any set of four values for n, l , m and s characterizes a spin orbital. Pauli.s exclusion principle states that a given spin orbital can accomodate not more than electron. Further the values l = 0, l=1, l=2, l=3 are designated s,p,d and f orbitals respectively. How many spin orbitals are there corresponding to n = 3?

The equation of Schroedinger for the hydrogen atom in the time-independet, non-relativistic form is a partial differential equation involving the position coordinates (x, y and z). The potential energy term for the proton-electron system is spherically symmetric of the form -1//4pi in_(0) xx (e^(2)//r) . THus it is advantages to change over from the cartesian coordinates (x,y and z) to the spherical polar coordinates, (r, theta and phi ). In this form the equation become separable in the radial part involving r and the angular part involving theta and phi . The probability of locating the electron within a volume element d tau = 4pi r^(2)dr is then given |Psi|^(2)(4pir^(2)dr) , where Psi is a function of r, theta and phi . With proper conditions imposed on Psi , the treatment yields certain functions, Psi , known as atomic orbitals which are solutions of the equations. Each function Psi correspods to quantum number n, l and m, the principal, the azimuthal and the magnetic quantum number respectively, n has values 1, 2, 3,...., l has values 0, 1, 2, ....(n-1) for each value of n and m (n-1) for each value of n and m (m_(l)) has values =1, +(l+1),...1,0,-1,-2...-l i.e., (2l+1) values for each value of l. In addition a further quantum number called pin had to be introduced with values +-1//2 . Any set of four values for n, l , m and s characterizes a spin orbital. Pauli.s exclusion principle states that a given spin orbital can accomodate not more than electron. Further the values l = 0, l=1, l=2, l=3 are designated s,p,d and f orbitals respectively. Which of the following diagrams corresponds to the 2s orbital ?

The value of the integral I=int_(0)^(1)x(1-x)^(n) is

If 2tan^(2)x-5secx=1 for exactly 7 distinct values of x in [0,(npi)/2], n in N then greatest value of n is

The value of 2^(n)n!(1.3.5.....(2n-1)) is

AAKASH SERIES-ATOMIC STRUCTURE-Level - I (EAMCET) (Exercise -IV (Quantum numbers))
  1. The number of orbitals in the quantum level n = 4 is

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  2. The quantum number which is equal for all the d-electrons in an atom i...

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  3. Correct set of four quantum numbers for the valence electron of Rubidi...

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  4. n, l and m values of the 2p(z) orbital are

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  5. Which of the following is not a possible value of azimuthal quantum nu...

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  6. The azimuthal quantum number for the last electron in sodium atom is

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  7. Maximum number of electrons that can be present in M and N - shells re...

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  8. What is the maximum number of electrons that can be theoretically pres...

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  9. The correct set of quantum numbers for a 4d electrons is

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  10. Which of the following sets of quantum numbers is correct for an elect...

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  11. The number of different spatial arrangements for the orbital with 1 = ...

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  12. An electron in an atom has m = -2 value. Then (I) its 'n' value shou...

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  13. The maximum number of electrons that can be present in an orbit with s...

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  14. The maximum number of eletrons with s = +1/2 in an orbital for which l...

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  15. (A) : The energy of electron is largely determined by its principal qu...

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  16. If the value of principal quantum number is 3, the total possible valu...

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  17. For a particular value of azimuthal quantum number (l), the total numb...

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  18. How many electrons maximum can have n + 1 = 4 in an atom.

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  19. (A) : For n = 3, 1 may be 0,1,2 and .m. may be 0, (+-2, +-1 and 0) (...

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  20. If magnetic quantum number of a given electron is represented -3, then...

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