Home
Class 12
CHEMISTRY
Estimate the difference in energy betwee...

Estimate the difference in energy between the first and second Bohr's orbit for a hydrogen atom. At what minimum atomic number , a transition from `n = 2` to `n = 1` energy level would result in the emission of X -rays with `lambda = 3.0 xx 10^(-8) m`? Which hydogen -like species does this atomic number correspond to ?

Text Solution

Verified by Experts

The correct Answer is:
2
`13.6Z^(2)((1)/(1)-(1)/(4))eV=(hc)/(lambda)" "rArr" "13.6xx1.6xx10^(-19)Z^(2)xx(3)/(4)=(6.626xx10^(-34)xx3xx10^(8))/(3xx10^(-8))`
`rArr" "Z^(2)=4 rArr Z=2`
Promotional Banner

Similar Questions

Explore conceptually related problems

Estimate the difference in energy between the first and second Bohr's orbit for a hydrogen atom At what minimum atomic number , a transition from n = 2 to n = 1 energy level would result in the enmission of X -rays with lambda = 3.0 xx 10^(-8) m ? Which hydogen -like spectrium does this atomic bnumber corresponding to ?

At what atomic number would a transition from n=2 to n=1 energy level result in emission of photon of lambda= 3xx10^(-8)m ?

One energy difference between the states n = 2 and n= 3 is EeV , in hydrogen atom. The ionisation potential of H atom is -

The energy difference between the first two levels of hydrogen atom is 10.2eV . For another element of atomic number 10 and mass number 20, this will be

Calculate the energy of an electron in the second Bohr's orbit of an excited hydrogen atom the energy of electron in the first Bohr orbit is -2.18 xx 10^(-11) erg

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 ) :

Determine the wavelengh of light emitted when a hydrogen atom makes a transition from the n=6 to the n=2 energy level according to the Bohr model

Energy of the lowest level of hydrogen atom is -13.6 eV . The energy of the photon emitted in the transition from n=3 to n=1 is