The radial wave function for 1 s electron in H-atom is `R=(2)/a_(0)^(3//2)e^(-r//a_(0))` where `a_(0)`=radius of `1^(st)` orbit of H-atom . The ratio of probablitiy of `1^(st)` electron in hyrogen atom at distance `a_(0)` from nucleus to that at distance `a_(0)/2` from nucleus.

The first orbital of H is represented by: psi=(1)/(sqrtr)((1)/(a_(0)))^(3//2)e^(-r//a_(0)) , where a_(0) is Bohr's radius. The probability of finding the electron at a distance r, from the nucleus in the region dV is :

The first orbital of H is represented by: psi=(1)/(sqrtpi)((1)/(a_(0)))^(3//2)e^(-r//a_(0)) , where a_(0) is Bohr's radius. The probability of finding the electron at a distance r, from the nucleus in the region dV is :

For an electron in a hydrogen atom, the wave function psi is proportional to exp -r//a_(0) , where a_(0) is the Bohr radius. Find the ratio of probability of finding the electron at the nucleus to the probability of finding it at a_(0) .

For an electron in a hydrogen atom, the wave function y is proportional to exp- r//a_(0) , where a_(0) is the Bohr radius. Find the ratio of probability of finding the electron at the nucleus to the probability of finding it at a_(0) .

For an electron in a hydrogen atom , the wave function Phi is proportional to e^(-r/a(0)) where a_(0) is the Bohr's radius What is the radio of the probability of finding the electron at the nucleus to the probability of finding at a_(0) ?

The Schrodinger wave equation for hydrogen atom is psi_(2s) =1/(4sqrt(2pi)) (1/(a_(0)))^(3//2)(2-r/(a_(0)))e^(-t//a_(0)) where a_0 is Bohr's radius. If the radial node in 2 s be at r_0 , then r_0 would be equal to

The wave function for 1s orbital of hydrogen atom is given by: Psi_(1s)=(pi)/sqrt2e^(-r//a_(0)) Where, a_(0) = Radius of first Bohar orbit r= Distance from the nucleus (Probability of finding the ekectron varies with respect to it) What will be the ratio of probability of finding rhe electron at the nucleus to first Bohr's orbit a_(0) ?