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The maximum number of photons emitted wh...

The maximum number of photons emitted when an electron jumps from an energy level n=5 to n=1 is s

A

3

B

10

C

8

D

6

Text Solution

Verified by Experts

The correct Answer is:
B
The number of photons emitted (emission lines) when the electron jumps from n = 5 to n = 1 is given by
`N=(n(n-1))/(2) = (5xx4)/(2) =10`
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What happens when an electron jumps from a lower energy level to a higher energy level?

Calculate the energy and frequency of the radiation emitted when an electron jumps from n = 3 to n = 2 in a hydrogen atom

Knowledge Check

  • The maximum number of photons emitted when an electron jumps from an energy level n=4 to n=1 is

    A
    1
    B
    2
    C
    3
    D
    4

  • The total number of spectral lines obtained when an electron jumps, from n = 5 to n =1 in a sample of hydrogen atoms.

    A
    4
    B
    6
    C
    12
    D
    10

  • The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to (n(n-1))/(2). For exampe, in the case of n=4, number of lines produced is 6 (4 to 3,4 t 2,4 to 1,3to 2,3 to 1,2 to 1). When an electron returns from n_(2) and n_(1) state, the number of lines in the spectrum will be equal to (n _(2)-n_(1))(n_(2)-n_(1) +(1)/(2) If the electron comes back from energy level having energy E _(2) to energy level having energy E _(1), then the difference may be expressed in terms of energy of photon as : E_(2) -E_(1) =Delta E, lamda= (hc) /(Delta E) Since h and c are constants, Delta E corresponds to definite energy, thus each transition from one energy level to another will produce a light of definitewavelength. This is actually observed as a line in the spectrum of hydrogen atom. Wave number of line is given by the formula vecv=R((1)/(n _(1)^(2))-(1)/(n _(2) ^(2))), where R is a Rydberg's constant (R=1.1 xx 10 ^(7)m^(-1)) In a collection of H–atom, electrons make transition from 5th excited state to 2nd excited state then maximum number of different types of photons observed are :

    A
    3
    B
    4
    C
    6
    D
    15

    • Similar Questions

    Explore conceptually related problems

    Calculate the energy and frequency of the radiation emitted when an electron jumps from n=3 to n=2 ina hydrogen atom.

    How many spectrual lines are emitted by atomic Hydrogen, when an electron jumps from 5th energy level to ground state ?

    The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to (n(n-1))/(2). For exampe, in the case of n=4, number of lines produced is 6 (4 to 3,4 t 2,4 to 1,3to 2,3 to 1,2 to 1). When an electron returns from n_(2) and n_(1) state, the number of lines in the spectrum will be equal to (n _(2)-n_(1))(n_(2)-n_(1) +1))/(2) If the electron comes back from energy level having energy E _(2) to energy level having energy E _(1), then the difference may be expressed in terms of energy of photon as : E_(2) -E_(1) =Delta E, lamda= (hc) /(Delta E) Since h and c are constants, Delta E corresponds to definite energy, thus each transition from one energy level to another will produce a light of definitewavelength. This is actually observed as a line in the spectrum of hydrogen atom. Wave number of line is given by the formula vecv=R((1)/(n _(1)^(2))-(1)/(n _(2) ^(2))), where R is a Rydberg's constant (R=1.1 xx 10 ^(7)m^(-1)) The energy photon emitted corresponding to transition n =3 to n =1 is [h=6 xx 10 ^(-34)J-sec]

    The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to (n(n-1))/(2). For exampe, in the case of n=4, number of lines produced is 6 (4 to 3,4 t 2,4 to 1,3to 2,3 to 1,2 to 1). When an electron returns from n_(2) and n_(1) state, the number of lines in the spectrum will be equal to (n _(2)-n_(1))(n_(2)-n_(1) +(1)/(2) If the electron comes back from energy level having energy E _(2) to energy level having energy E _(1), then the difference may be expressed in terms of energy of photon as : E_(2) -E_(1) =Delta E, lamda= (hc) /(Delta E) Since h and c are constants, Delta E corresponds to definite energy, thus each transition from one energy level to another will produce a light of definitewavelength. This is actually observed as a line in the spectrum of hydrogen atom. Wave number of line is given by the formula vecv=R((1)/(n _(1)^(2))-(1)/(n _(2) ^(2))), where R is a Rydberg's constant (R=1.1 xx 10 ^(7)m^(-1)) The wave number of electromagnetic radiation emitted during the transition of electron in between two levels of Li ^(2+) ion whose principal quantum numbers sum is 4 and difference is 2 is:

    If the electron jumps from 7.00 eV energy level to 5.0 eV energy level it

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