When electron jumps from nth orbit to 1st orbit in an imaginary atom obeying Bohr’s model, itemits two radiations of wavelengths 400 nm and 300 nm. The frequency of radiation emitted out inthe transition n = n to n = 1 will be

The problem is based on the Bohr's model of the atom and the concept of electron transitions between energy levels.

Step 1: According to Bohr's model, the energy difference between two orbits is given by the formula:

ΔE = E1 - En = h*(c/λ)

where E1 and En are the energies of the 1st and nth orbits respectively, h is Planck's constant, c is the speed of light, and λ is the wavelength of the emitted radiation.

Step 2: Given that the electron emits two radiations of wavelengths 400 nm and 300 nm when it jumps from the nth orbit to the 1st orbit, we can write two equations based on the above formula:

E1 - En = h*(c/400 nm) ----(1)

E1 - En = h*(c/300 nm) ----(2)

Step 3: Subtract equation (2) from equation (1), we get:

0 = hc(1/400 nm - 1/300 nm)

This implies that the two given wavelengths cannot be emitted in a single transition from the nth orbit to the 1st orbit in the Bohr's model.

Step 4: Therefore, the frequency of radiation emitted in the transition n = n to n = 1 cannot be determined based on the given information.