Ionisation energy of a hydrogen like species is 54.4eV .Calculate radius of second Bohr orbit of this species.
(A) 0.529A
(B) 1.058A
(C) 2.116A
(D) 1.116A

The ratio of kinetic energy and potential energy of an electron in a Bohr orbit of a hydrogen - like species is :

The kinetic energy of an electron in the second Bohr orbit of a hydrogen atom is [ a_(0) is Bohr radius] :

In a hydrogen like species electrons is in 2^(nd) excited state the binding energy of the fourth state of this species is 13.6 eV then

Calculate the radius of 1^(st), 2^(nd),3^(rd),4^(th) Bohr's Orbit of hydrogen.

The ionisation potential of hydrogen is 13.60 eV . Calculate the energy required to produce one mole of H^(o+) ion (1 eV = 96.3 kJ mol^(-1)) .

The kinetic energy of the electron in the second Bohr's orbit of a hydrogen atom [ a_(0) is Bohr's radius] is

A mu-meson ("charge -e , mass = 207 m, where m is mass of electron") can be captured by a proton to form a hydrogen - like ''mesic'' atom. Calculate the radius of the first Bohr orbit , the binding energy and the wavelength of the line in the Lyman series for such an atom. The mass of the proton is 1836 times the mass of the electron. The radius of the first Bohr orbit and the binding energy of hydrogen are 0.529 Å and 13.6 e V , repectively. Take R = 1.67 xx 109678 cm^(-1)

If I exciation energy for the H-like (hypothetical) sample is 24 eV, then binding energy in III excited state is : (a)2eV (b)3eV (c)4eV (d)5eV

Assertion The radius of second orbit of hydrogen atom is 2.1Å Reason Radius of nth orbit of hydrogen atom r_(n)propn^(2)

The ionization energy of a hydrogen like Bohr atom is 4 Rydberg. If the wavelength of radiation emitted when the electron jumps from the first excited state to the ground state is N-m and if the radius of the first orbit of this atom is r-m then the value of (N)/(r )=Pxx10^(2) then, value of P . (Bohr radius of hydrogen =5xx10^(-11)m,1 Rydberg =2.2xx10^(-18)J )