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Principal azimuthal , and magnetic qua...

Principal azimuthal , and magnetic quantum numbers are respetively related to

A

Size, shape and orientation

B

Shape, size and orientation

C

Size, orientation and shape

D

None of the above

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The correct Answer is:
A
n, l and m are related to size, shape and orientation respectively.
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An electron in an atom can be completely designated with the help of four quantum numbers. Out of these, the first three i.e., principal (n), azimuthal (l) and magnetic (m) quantum number are obtained from the solution of Shrodinger wave equation while the spin(s) quantum number arises from the spin of the electron around its axis clockwise or antiaclockwise. Ot of these principal quantum number tells about the size, azimuthal quantum number about the shape and magnetic quantum signifies the orientation of the electron orbital. The maximum number of electrons in a subshell having the same value of spin quantum number is given by

An electron in an atom can be completely designated with the help of four quantum numbers. Out of these, the first three i.e., principal (n), azimuthal (l) and magnetic (m) quantum number are obtained from the solution of Shrodinger wave equation while the spin(s) quantum number arises from the spin of the electron around its axis clockwise or antiaclockwise. Ot of these principal quantum number tells about the size, azimuthal quantum number about the shape and magnetic quantum signifies the orientation of the electron orbital. How many electrons in a given atom have the following set of quantium numbers? n = 3, l =2, m = +2, s = -1//2

An electron in an atom can be completely designated with the help of four quantum numbers. Out of these, the first three i.e., principal (n), azimuthal (l) and magnetic (m) quantum number are obtained from the solution of Shrodinger wave equation while the spin(s) quantum number arises from the spin of the electron around its axis clockwise or antiaclockwise. Ot of these principal quantum number tells about the size, azimuthal quantum number about the shape and magnetic quantum signifies the orientation of the electron orbital. The electronic configuration of P in H_(3)PO_(4) is

For the principal quantum number n = 2, the possible values of azimuthal quantum number and magnetic quantum number respectively are

The set of principal (n), azimuthal (l) and magnetic (m_(l)) quantum number that is not allowed for the electron in H-atom is

n+l +m for the valence electrons of rb will be (where n,l,m, are prinicipal quantum number azimuthal qunatum number magnetic quantum number respectivley ):

For n=2 the correct set of azimuthal and magnetic quantum numbers are

ERRORLESS-STRUCTURE OF ATOM-PAST YEARS QUESTIONS
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  2. Which one is the wrong statement ?

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  3. Principal azimuthal , and magnetic quantum numbers are respetively r...

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  4. The total number of orbitals possible for the quantum number n is

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  5. For azimuthal quantum number l=3, the maximum number of electrons wi...

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  6. Maximum number of electrons in a sub-shell with l = 3 and n = 4 is.

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  7. For which of the following sets of four quantum numbers, an electron w...

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  8. Which of the following set of quantum number is possible ?

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  9. Which of the following set of quantum numbers is not valid.

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  10. Azimuthal quantum number defines.

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  11. The quantum numbers 'm' of a free gaseous atom is associated with :

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  12. For principle quantum number n = 4 the total number of orbitals having...

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  13. What is the maximum number of electrons that can be associated with a ...

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  14. What is the maximum number of orbitals that can be identified with the...

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  15. Two electrons occupying the same orbital are distinguished by:

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  16. Five valence electrons of ""(15)P are labelled as If the spin qua...

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  17. The statements. (i) In filling a group of orbitals of equal energy, ...

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  18. Which of the following explains the sequence of filling the electrons ...

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  19. Which one is the correct outer configuration of chromium.

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  20. Elements up to atomic number 103 have been synthesized and studied. If...

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