Atomic Spectrum (Hydrogen Spectrum)

The frequency of oscillation of the electric field vector of a certain electromagnetic.wave is  $5\times {10}^{14}$ Hz. What is the frequency of oscillation of the corresponding magnetic field vector and to which part of the electromagnetic spectrum does it belong?

According to Bohr theory, the electronic energy of a hydrogen atom in the ${\mathrm{n}}^{\mathrm{th}}$ Bohr atom is given by ${\mathrm{E}}_{\mathrm{n}}=\frac{21.76\times {10}^{-19}}{{\mathrm{n}}^2}\mathrm{J}$. Calculate the longest wavelength of light that will be needed to remove and electron from the third Bohr orbit of the ${\mathrm{He}}^{+}$ ion (If the wavelength is $x\times {10}^{-7}$(in meter) and $x$ is an integer. Report '$x$')

In the Balmer series of atomic spectra of hydrogen, there is spectral line having wavelength $434.4 \mathrm{nm}$. Calculate the number of higher orbit from which the electron drops to generate this line. $\left(\mathrm{R}=10.97\times {10}^6 {\mathrm{m}}^{-1}\right)$

If the series limit to the wavelength of the Lyman series of the hydrogen atom is $912 \mathrm{\AA }$, then the series limit to the wavelength for the Balmer series of the hydrogen atom is

Assertion : The spectrum of ${\mathrm{He}}^{+}$ is expected to be similar to that of hydrogen.

Reason : ${\mathrm{He}}^{+}$ is also one electron system.

Which of the following is the value of the Rydberg constant for hydrogen?

Among the following, which transition in the Hydrogen spectrum would have the same wavelength as Balmer transition, $\mathrm{n}=4$ to $\mathrm{n}=2$ in ${\mathrm{He}}^{+}$ spectrum?

If the wavelength of the first line in Balmer series is $656 \mathrm{nm}$, then the wavelengths of its second line and limiting line respectively are

Which energy level transition among the following will have the least wavelength?

The electron in a hydrogen atom jump on absorbing $12.75 \mathrm{eV}$ of energy would jump to orbit

The shortest wavelength in hydrogen spectrum is approximately ______

Which of the following series of transitions in the spectrum of hydrogen atom falls in visible region?

Calculate the shell number of excite state of $\mathrm{H}$-atom in terms of wavelength $\lambda$, when the electron $\mathrm{d}$ excites to the ground level.

In the Balmer series of atomic spectra of hydrogen, there is spectral line having wavelength $434.4 \mathrm{nm}$. Calculate the number of higher orbit from which the electron drops to generate this line. $\left(\mathrm{R}=10.97\times {10}^6 {\mathrm{m}}^{-1}\right)$

What transition in the ${\mathrm{He}}^{+}$ spectrum would have the same wavelength as the first Lyman transition of hydrogen $({\mathrm{n}}_2=2 \mathrm{to} {\mathrm{n}}_1=1)$?

The frequency of the spectral line when an electron from the fifth orbit jumps to the second orbit in a hydrogen atom is $6.91\times {10}^{\mathrm{x}} \mathrm{Hz}$ . Calculate the value of x?

${\mathrm{R}}_{\mathrm{H}} = 109737 {\mathrm{cm}}^{-1}$

The frequency of radiation having wavelength $5800 \stackrel{\circ }{\mathrm{A}}$ is $\mathrm{y}\times {10}^{14}$. The value of $\mathrm{y}$ is

Roundoff the answer up to one significant figures.

Suppose that an excited hydrogen atom returns to the ground state, the wavelength of the emitted photon is $\mathrm{\lambda }$. What will be the principal quantum number of the excited state?