Physics Test - ...

A hydrogen atom and $L{i}^{++}$ ion are both in the second excited state. If$l_H$and$l_{Li}$ are their respective electronic moments, and $E_H$ and $E_{Li}$ their respective energies, then:

Imagine an atom made up of a proton and a hypothetical particle of double the mass of the electron but having the same charge as the electron. Apply the Bohr atom model and consider all possible transitions of this hypothetical particle to the first excited level. The longest wavelength photon that will be emitted has wavelength $\lambda$ (given in terms of Rydberg constant $R$ for the hydrogen atom) equal to:

Hydrogen ${(}_1{H}^1)$, Deuterium ${(}_1{H}^2)$, singly ionized Helium${{(}_{2}H{e}^4)}^{+}$and doubly ionized Lithium${{(}_{3}L{i}^6)}^{++}$all have one electron around the nucleus. Consider an electron transition from $n=2$ to $n=1$. If the wavelengths of emitted radiation are${\lambda }_1,{\lambda }_2,{\lambda }_3$, and${\lambda }_4$ respectively, then approximately which of the following is correct?

The intensity of X-ray from a Coolidge tube is plotted against wavelength as shown in the figure. The minimum wavelength found is \({\lambda_{c}}\) and the wavelength of \(K_{\alpha}\) line is \(\lambda_{k}\). As the accelerating voltage is increased:

If \(\lambda_{1}\) and \(\lambda_{2}\) are the wavelengths of the first members of Lyman and Paschen series, respectively, then \(\lambda_{1}: \lambda_{2}\) is:

A diatomic molecule is made of two masses $m_1$ and $m_2$, which are separated by a distance $r$. If we calculate its rotational energy by applying Bohr rule of angular momentum quantization, then its energy will be given by:

Energy levels $A,B$, and $C$ of a certain atom correspond to increasing values of energy $E_A<E_B<E_C$. If${\lambda }_1$,${\lambda }_2$, and${\lambda }_3$ are the wavelengths of radiations corresponding to transitions $C$ to $B,B$ to $A$, and $C$ to $A$, then which of the following relations is correct?

The energy of an electron in the second orbit of a hydrogen atom in $E_2$. The energy of an electron in the third orbit of$H{e}^2$ will be:

The diagram shows the energy levels for an electron in a certain atom. Which transition shown represents the emission of a photon with the most energy?

The wavelength of radiations emitted is ${\lambda }_0$when an electron in a hydrogen atom jumps from the third orbit to the second orbit. If in the $H$-atom itself, the electron jumps from the fourth orbit to the second orbit, then the wavelength of emitted radiation will be: