What will be the amount of energy absorbed when an electron jumps from first orbit to second orbits, if the value of energy in nth orbit of H-atom is expressed as (E_n=-13.6/n² eV)

An electron changes its position from orbit n=2 to the orbit n=4 of an atom. The wavelength of the emitted radiations is (R = Rydberg’s constant)

Imagine an atom made of a proton and a hypothetical particle of double the mass of the electron but having same charge as the electron. Apply Bohr atom model and consider all possible transitions of the hypothetical particle to the first excited level. The longest wavelength photon that will be emitted has wavelength λ equal to

Ionisation potential of hydrogen atom is 13.6 eV. Hydrogen atoms in ground state are excited by monochromatic radiation of photon energy 12.1 eV. According to Bohr’s theory, the spectral lines emitted by hydrogen will be

In Bohr’s model the atomic radius of the first orbit is r₀, the radius of the third orbit will be

Taking Rydberg’s constant =1.097 x10⁷ m first and second wavelength of Balmer series in hydrogen spectrum, is

Which of the following lines of the H-atom spectrum belengs to Balmer series?

The density of uranium is of the Order of

Two radioactive materials A and B have decay constants 10λ and λ, respectively. If initially they have the same number of nuclei, then the ratio of the number of nuclei of A to that of B will be 1/e after a time.

If R is the radius and A is the mass number, then log R versus log A graph will be