For the 1s orbital of the Hydrogen atom, the radial wave function is g

1.	For the 1s orbital of the Hydrogen atom, the radial wave function is given as: R(r)=1√π(1a0)32e−ra0 (Where a0=0.529 ∘A) The ratio of radial probability density of finding an electron at r=a0 to the radial probability density of finding an electron at the nucleus is given as (x.e−y). Calculate the value of (x+y).
Answer» For the $1 s$ orbital of the Hydrogen atom, the radial wave function is given as: $R (r) = \frac{1}{\sqrt{π}} {(\frac{1}{a_{0}})}^{\frac{3}{2}} e^{\frac{- r}{a_{0}}}$ (Where $a_{0} = 0.529 \circ A$ ) The ratio of radial probability density of finding an electron at $r = a_{0}$ to the radial probability density of finding an electron at the nucleus is given as $(x . e^{- y})$ . Calculate the value of $(x + y)$ .

For the 1s orbital of the Hydrogen atom, the radial wave function is given as: R(r)=1√π(1a0)32e−ra0 (Where a0=0.529 ∘A) The ratio of radial probability density of finding an electron at r=a0 to the radial probability density of finding an electron at the nucleus is given as (x.e−y). Calculate the value of (x+y).

Answer»

For the $1 s$ orbital of the Hydrogen atom, the radial wave function is given as:
$R (r) = \frac{1}{\sqrt{π}} {(\frac{1}{a_{0}})}^{\frac{3}{2}} e^{\frac{- r}{a_{0}}}$ (Where $a_{0} = 0.529 \circ A$ )

The ratio of radial probability density of finding an electron at $r = a_{0}$ to the radial probability density of finding an electron at the nucleus is given as $(x . e^{- y})$ .
Calculate the value of $(x + y)$ .

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