Consider a hydrogen atom with its electron in the `n^(th)` orbital An electomagnetic radiation of wavelength `90 nm` is used to ionize the atom . If the kinetic energy of the ejected electron is `10.4 eV` , then the value of `n` is ( hc = 1242 eVnm)

Consider a hydrogen atom with its electron in the `n^(th)` orbital An

1.	Consider a hydrogen atom with its electron in the `n^(th)` orbital An electomagnetic radiation of wavelength `90 nm` is used to ionize the atom . If the kinetic energy of the ejected electron is `10.4 eV` , then the value of `n` is ( hc = 1242 eVnm)
Answer» Correct Answer - `2` `(hc)/(lambda)-{13.6eV.(1)/(2)}=10.4` `rArr(124eV)/(90)-(13.6)/(n^(2))=10.4` `rArr(41.4)/(3)-(13.6)/(n^(2))=10.4` `rArr13.8-10.4=(13.6)/(n^(2))` `rArr3.4=(13.6)/(n^(2))` `rArrn^(2)=4` `rArr n=2`

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Consider a hydrogen atom with its electron in the `n^(th)` orbital An electomagnetic radiation of wavelength `90 nm` is used to ionize the atom . If the kinetic energy of the ejected electron is `10.4 eV` , then the value of `n` is ( hc = 1242 eVnm)

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