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When an electron drops from a higher ene...

When an electron drops from a higher energy level to a low energy level, then

A

energy is absorbed

B

energy is emitted

C

atomic number increases

D

atomic number decreases

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Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" The energy required to promote the ground state electron of H-atom to the first excited state is: When an electron returns from a higher energy level to a lower energy level, energy is given out in the form of UV//Visible radiation.

When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the form of electromagnetic radiation. Why cannot it be emitted as other forms of energy?

Knowledge Check

  • when an electron falls from a higher energy to a lower energy level the difference in the energies appears in the form of

    A
    electromagnetic radiation only
    B
    thermal radiation only
    C
    both electromagnetic and thermal radiations
    D
    none of these

  • If Delta E is the energy emitted in electron vots when an electronic transition occurs from higher energy level to a lower energy level in H-atom, the wavelength of the line produced is approximately equal to

    A
    `(19800)/(DeltaE) Å`
    B
    `(12375)/(DeltaE) Å`
    C
    `(13600)/(Delta E) Å`
    D
    `(21800)/(Delta E) Å`

  • An electron in a hydrogen atom undergoes a transition from higher energy level to a lower energy level. The incorrect statement of the following is

    A
    kinetic energy of the electron increases.
    B
    velocity of the electron increases
    C
    angular momentum of the electron remains constant.
    D
    wavelengths of de-Broglie wave associated with the motion of electron decreases.

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    When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the forms of electromagnetic radiation. Why cannot it be emitted as other forms of energy?

    What happens when an electron jumps from a lower energy level to a higher energy level?

    When an electron of hydrogen like atom jumps from a higher energy level to a lower energy level.

    (1) As long as an electron revolves in a particular orbit , the electron does not lose its energy Therefore, these orbits are called stationary orbits and the electrons are said to be in station-ary energy state (2) Each orbit or shell is associated with a definite amount of energy . Hence , these are also called energy levels An electron jumps from a lower energy level to a higher energy level , by absorting energy . It jumps from a higher energy to a lower level by emmitting energy in the form of electromagnetic radiation Electrons move around the nucels in specified circular paths called orbits or shells or energy levels and are designated as K,L,M and N shells respectively Arrange the above postulates of Bohr's theory in a correct sequence

    When an electron falls form a height energy to a lower level, the difference in the energies appears in the form of electromegnetic radiation. Why can not it be emitted as other forms of energy ?

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