If the potential energy between electron and proton at a distance r is given by U = -`((ke^2)/(3r^3))`, the law of force is

Suppose the potential energy between an electron and a proton at a distance r is given by Ke^(2)// 3 r^(3) . Application of Bohr's theory tohydrogen atom in this case showns that

Supose the potential energy between electron and porton a distance r is given by U=-(Ke^(2))/(3r^(3)) Assuming Bohar's Model to be valid for this atom if the speed of elctron in n^(th) orbit depends on the prinicpal quantum number n as v oon^(x) then find the vlaue of x.

In a hypothetical atom, potential energy between electron and proton at distance r is given by ((-ke^(2))/(4r^(2))) where k is a constant Suppose Bohr theory of atomic structrures is valid and n is principle quantum number, then total energy E is proportional to 1) n^5 2) n^2 3) n^6 4) n^4

Assume a hypothetical hydrogen atom in which the potential energy between electron and proton at separation r is given by U = [k ln r - (k/2)], where k is a constant. For such a hypothetical hydrogen atom, calculate the radius of nth Bohr orbit and energy levels.

Soppose potential energy between electronand proton at seperation r is given by U = klog r, where k is a constant. For such a hypothetical hydrogen atom , calculate the radins of nth Bohr and its energy level

If potential energy between a proton and an electron is given by | U | = k e^(2)//2 R^(3) , where e is the charge of electron and R is the radius of atom , that radius of Bohr's orbit is given by (h = Plank's constant, k = constant)

The force between two electrons separated by a distance r varies as

The electrostatic potential energy between proton and electron separated by a distance 1 Å is

The force between two electrons separated by a distance r is proportional to

If the potential energy between two molecules is given by U= -(A)/(r^6) + B/(r^(12)) , then at equilibrium , separation between molecules , and the potential energy are :