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Find the radius of a hydrogen atom in the n = 2 state according to Bohr’s theory.

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04:16

An excited hydrogen atom could, in principle, have a radius of 1.00 cm. What would be the value of $n$ for a Bohr orbit of this size? What would its energy be?

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Determine the most probable distance from the nucleus of an electron in the $n=2, \ell=0$ state of hydrogen.

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Calculate the radial probability density $P(r)$ for the hydrogen atom in its ground state at (a) $r=0,$ (b) $r=a$ , and(c) $r=2 a,$ where $a$ is the Bohr radius.

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For the hydrogen atom in its ground state, calculate (a) the probability density $\psi^{2}(r)$ and (b) the radial probability density $P(r)$for $r=a$ , where $a$ is the Bohr radius.

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Calculate the probability that the electron in the hydrogen atom, in its ground state, will be found between spherical shells whose radii are $a$ and $2 a,$ where $a$ is the Bohr radius.

Transcript

Thanks student. Thanks a lot for costing the problem. Welcome to the solution. Basically, we have to find the Bohr radius for N is equal to two. So the equation of the board radius, let us denote it as we are, is equal to 0.5 to nine, multiplied by n Squire, divided by zero and as the state of the atom. And that is the atomic number that is here since its hydrogen, it is one and is given to me too. And this and so would…

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