What is the approximate angular momentum (in | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The angular momentum $(L)$ of an electron in a hydrogen atom is given by Bohr's postulate: $L = \frac{nh}{2\pi}$ For the ground state, the princip

Vedclass · Accepted Answer

$1055 	imes 10^{-37}$

Vedclass · Answer

(C) The angular momentum $(L)$ of an electron in a hydrogen atom is given by Bohr's postulate: $L = \frac{nh}{2\pi}$ For the ground state, the principal quantum number $n = 1$. Substituting the values: $L = \frac{1 	imes 6.625 	imes 10^{-34}}{2 	imes 3.14159} \ J \ s$ $L \approx \frac{6.625 	imes 10^{-34}}{6.283} \ J \ s$ $L \approx 1.0545 	imes 10^{-34} \ J \ s$ To match the options, we express this as: $1.0545 	imes 10^{-34} = 1055 	imes 10^{-37} \ J \ s$ Therefore, the correct option is $C$.

What is the approximate angular momentum (in $J \ s$) of an electron in a hydrogen atom in its ground state? $(h = 6.625 \times 10^{-34} \ J \ s)$

Similar Questions

Bohr’s model of atom explains :

Which of the following electronic transitions in a hydrogen atom will require the highest energy?

The energy of an electron in the first Bohr orbit of a hydrogen atom is $-13.12 \times 10^5 \ J \ mol^{-1}$. Calculate the energy required for the transition of an electron from the first orbit to the second orbit.

Write down the postulates of Bohr's model for the hydrogen atom.

If the shortest wavelength of the Lyman series of the $H$ atom is $x$,then calculate the total energy of the $H$ atom in the first excited state.

Vedclass Test Series

Exam Paper Generator

Online Exam Module