NEET Physics Atoms MCQs

An electron in a hydrogen atom transitions from an unknown energy level $n_i$ to $n_f = 2$. If the emitted photon has a wavelength of 486 nm, what is the value of $n_i$? (Rydberg constant, R = $1.097 imes 10^7 m^{-1}$)

The ratio of the wavelengths of the first line of the Lyman series and the first line of the Balmer series in the hydrogen spectrum is:

The limiting line in the Balmer series of hydrogen corresponds to a transition from $n = \infty$ to $n = 2$. What is the wavelength of this line? (Rydberg constant, $R = 1.097 imes 10^7 m^{-1}$)

In the spectrum of a hydrogen-like species, the wavelength of the first line of the Lyman series is $\lambda$. What is the wavelength of the first line of the Balmer series for this species?

The Balmer series in the hydrogen spectrum corresponds to electron transitions ending at which energy level (n)?

When an electron in a hydrogen atom jumps from n=3 to n=1, what type of electromagnetic radiation is emitted?

When an electron in a hydrogen atom jumps from n=4 to n=2, the radiation emitted belongs to which series?

When an electron in a hydrogen atom transitions from n=3 to n=2, the emitted radiation falls in which region of the electromagnetic spectrum?

The Balmer series in the hydrogen spectrum lies in which region of the electromagnetic spectrum?

Given the Rydberg constant is $10^7 m^{-1}$, the wave number of the last line of the Balmer series in hydrogen spectrum will be: