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

(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

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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(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

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

The truth value "if 3 + 2 = 5 then 1 xx 0 = 0 " is

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

If sin^(2) x - 2 sin x - 1 = 0 has exactly four different solutions in x in [0, n pi] , then value/ values of n is / are (n in Z)

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

AAKASH SERIES-ATOMIC STRUCTURE-Objective Exericse - 2A
  1. For a particular value of azimuthal quantum number (I), the total numb...

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

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

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

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  5. The radial probability distribution curve obtained for an orbital wave...

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  6. The configuration 1s^(2)2s^(2)2p^(5)3s^(1) shows

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  7. The incorrect electronic arrangment is

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  8. Given this set of quantum numbers for a multi electron atom 2, 0, 0, a...

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  9. Which one of the following pairs of atoms/ions have identical ground s...

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  10. How many 'd' electrons are present in Cr^(2+) ion?

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  11. The atomic nụmber of the element with the maximum number of unpaired 2...

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  12. The total number of electrons present in all the 's' orbitals, all the...

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  13. Which atom has as many 's' electrons as P-electrons

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  14. An element has 2 electrons in its K-shell. 8 electrons in L-shell, 13 ...

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  15. The electronic configuration 1s^(2)2s^(2)2p^(6)3s^(1)3p^(3)3d^(2) repr...

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  16. The atomic number of an element M is 20. How many electrons are presen...

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  17. Consider the ground state of Cr atom (Z = 24). The numbers of electron...

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  18. Which is the first element to have 4d-electron in its electronic confi...

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  19. In the ground state, an element has 13 electrons in its "M - shell". T...

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  20. (A) : The electronic configuration of Cr is [Ar]3d^(5)4s^(1) but not [...

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