Atomic Structure
The energy of a photon is $$3 \times 10^{-12}$$ ergs. Its wavelength (in nm) will be:
The de Broglie wavelength of a particle of mass 1 gram and velocity $$100\ { ms }^{ -1 }$$ is:
Mass of particle, $$m= 1\ gram = 10^{-3}\ Kg$$ Velocity, $$v=100 \, ms^{-1}$$ De broglie wavelength $$\lambda =\dfrac{h}{mv}$$ $$=\dfrac{6.626\times 10^{-34}}{1\times 10^{-3}\times 100}$$ $$=6.626\times 10^{-33}\ m$$ Hence, option C is correct.
The energy of a photon is $$3 \times 10^{-12}$$ ergs. Its wavelength (in nm) will be:
Calculate the de Broglie wavelength for a beam of electron whose energy is 100 eV:
If the de-Broglie wavelength of a particle of mass $$m$$ is $$100$$ times its velocity then its value in terms of its mass $$(m)$$ and Planck's constant $$(h)$$ is:
Threshold wavelength of a metal is $${\lambda}_{0}$$. The de Broglie wavelength of photoelectron when the metal is irradiated with the radiation of wavelength $$\lambda$$ is:
The de Broglie wavelength associated with a ball of mass 200 g and moving at a speed of 5 meters / hour, is of the order of ($$h= 6.625\times 10^{-34}J s $$) is:
The de Broglie wavelength of an electron in the 4th Bohr orbit is:
The de Broglie wavelength (λ) associated with a photoelectron varies with the frequency (v) of the incident radiation as, [v0 is thrshold frequency]:
The de-Broglie's wavelength of electron present in first Bohr orbit of $$'H'$$ atom is?
Photoelectrons are liberated by ultraviolet light of wavelength $$3000\mathring{A}$$ from a metallic surface for which the photoelectric threshold is $$4000\mathring{A}$$. The de-Broglie wavelength of electrons emitted with maximum kinetic energy is:
The energy of an electron having de-Broglie wavelength $$'\lambda'$$ is: [h = Planck's constant, m = mass of electron]