Home
Class 11
CHEMISTRY
Applyig bohr's model when H-atom comes f...

Applyig bohr's model when H-atom comes from n=4 to n=2, calcualte its wavelength. In this process, write whether energy is released or aborbed? Also write the range of radiation `R_(H)=2.18xx10^(-18)J,h=6.63xx10^(-34)J-s`

Text Solution

Verified by Experts

Energy is released in this process, and the radiation will belong to visible region (Balmer series).
`E=(hc)/(lamda)=R_(H)Z^(2)[(1)/(n_(1)^(2))-(1)/(n_(2)^(2))]`
`(1)/(lamda)=(R_(H)Z^(2))/(hc)[(1)/(n_(1)^(2))-(1)/(n_(2)^(2))]`
`=(2.18xx10^(-18)xx1^(2))/(6.63xx10^(-34)xx3xx10^(8))[(1)/(4)-(1)/(16)]`
`=(2.18xx10^(-18)xx1^(2))/(6.63xx10^(-34)xx3xx10^(8))[(3)/(16)]`
`lamda=(6.63xx10^(-34)xx3xx10^(8)xx16)/(3xx2.18xx10^(-18))`
`=4866xx10^(-10)m`
`=4866` Ã…
Promotional Banner

Topper's Solved these Questions

  • ATOMIC STRUCTURE

    OP TANDON|Exercise Practice Problems|88 Videos

  • ATOMIC STRUCTURE

    OP TANDON|Exercise Questions with single correct Answer|203 Videos

  • ATOMIC STRUCTURE

    OP TANDON|Exercise Some Solved Examples|12 Videos

  • AROMATIC HYDROCARBONS (ARENES)

    OP TANDON|Exercise EXAMPLES|24 Videos

  • CHARACTERISATION OF ORGANIC COMPOUNDS

    OP TANDON|Exercise Passage-2|5 Videos

Similar Questions

Explore conceptually related problems

Determine the energy of 1 mole photons of radiations whose frequency is 5xx10^(10)s^(-1)" "(h=6.62xx10^(-34)J-s) .

The speed of electron having de Broglie wavelength of 10 ^(10) m is ( me = 9.1 xx 10 ^(-31) kg, h = 6.63xx 10^(-34) J-s)

The wavelength of the radiation emitted when an electron falls from Bohr 's orbit 4 to 2 in H atom is

What is the wavelength of light . Given energy =3.03xx10^(-19)J, h=6.6xx10^(-34)JS, c=3.0xx10^(8)m//s ?

Calculate the de Broglie wavelength associated with an alpha -particle having an energy of 7.7xx10^(-13)J and a mass of 6.6xx10^(-24)g.(h=6.6xx10^(-34)J-s) .

The frequency of radiation emiited when the electron falls n =4 to n=1 in a hydrogen atom will be ( given ionization energy of H= 2.18 xx 10 ^(-18)J "atom "^(-1) and h= 6.625 xx 10 ^(-34)Js)

If the electron in a hydrogen atom were in the energy level with n 3, how much energy in joule would be required to ionise the atom ? ( Ionisation energy of H - atoms is 2.18 xx 10^(-18) J ) :