The approximate radius of a $H - a t o m$ is $0.05 n m$ , and that of a proton is $1.5 \times 10^{- 15} m$ . Assuming both the hydrogen atom and the proton to be spherical, calculate a fraction of the space in an atom of hydrogen that is occupied by the nucleus.

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Solution

Radius of $H -$ atom = 0.05nm = $0.05 \times 10^{- 9}$
Radius of a proton = $1.5 \times 10^{- 15} m$
The volume behave like the third power of the raddi
$\frac{v o l u m e o f H a t o m}{v o l u m e o f a p r o t o n}$ = $[\frac{0.05 \times 10^{-} 9}{1.5 \times 10^{-} 15 m}]^{3}$
$= \frac{1}{0.000 000000000027}$
$= \frac{1}{2.7 \times 10^{- 14}}$

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The approximate radius of a H−atom is 0.05 nm, and that of a proton is 1.5×10−15m. Assuming both the hydrogen atom and the proton to be spherical, calculate a fraction of the space in an atom of hydrogen that is occupied by the nucleus.

Radius of H−atom = 0.05nm = 0.05×10−9Radius of a proton = 1.5×10−15mThe volume behave like the third power of the raddivolume of Hatomvolume of a proton = [0.05×10−91.5×10−15m]3 =10.000000000000027 =12.7×10−14

The approximate radius of a $H - a t o m$ is $0.05 n m$ , and that of a proton is $1.5 \times 10^{- 15} m$ . Assuming both the hydrogen atom and the proton to be spherical, calculate a fraction of the space in an atom of hydrogen that is occupied by the nucleus.