Bohr's Model for the Hydrogen Atom

In a hydrogen atom, if the energy of an electron in the ground state is  $\text{–13.6 eV}$, then that in the $\text{2nd}$ excited state is

Which of the following is the correct value of most probable radius for locating the electron in ${\mathrm{He}}^{+}$?

Assertion : The spectrum of ${\mathrm{He}}^{+}$ is expected to be similar to that of hydrogen.

Reason : ${\mathrm{He}}^{+}$ is also one electron system.

When an electron in an atom absorbs a definite amount of energy, the electron jump from its most stable state to some high energy level called the _____ state.

Define excited state for an atom.

The first orbit is called the ground state in hydrogen like atoms.

Discuss the ground state of hydrogen like atoms.

The excited state is the most stable state for an electron in an atom.

What do you mean by excited state in an atom?

Suppose that an excited hydrogen atom returns to the ground state, the wavelength of the emitted photon is $\mathrm{\lambda }$. What will be the principal quantum number of the excited state?

If Bohr radius is represented by ${\mathrm{a}}_0,$ the radius of the second orbit of helium ion $\left(\mathrm{H}{\mathrm{e}}^{+}\right)$ will be _____ $\stackrel{°}{\mathrm{A}}$. (Correct upto 3 decimal places)

If the velocity of the revolving electron of ${\mathrm{He}}^{+}$ in the first orbit $(\mathrm{n}=1)$ is $\mathrm{v},$ the velocity of the electron in the second orbit is:

Suppose that a hypothetical atom gives a red, green, blue and violet line in the spectrum. Which jump according to figure would give off the red spectral line?

In a certain electronic transition in the hydrogen atoms from an initial state $\left(1\right)$ to the final state $\left(2\right)$, the difference in the orbital radius $({\mathrm{r}}_1-{\mathrm{r}}_2)$ is $24$ times the first Bohr radius. Identify the transition.

The radii of two of the first four Bohr orbits of the hydrogen atom are in the ratio $1:4.$ The energy difference between them may be

The correct statements among the following.

i. ${\mathrm{E}}_{2\mathrm{s}}\left(\mathrm{H}\right)>{\mathrm{E}}_{2\mathrm{s}}\left(\mathrm{Li}\right)<{\mathrm{E}}_{2\mathrm{s}}\left(\mathrm{Na}\right)>{\mathrm{E}}_{2\mathrm{s}}\left(\mathrm{K}\right)$
ii. The maximum number of electrons in the shell with principal quantum number $n$ is equal to $2n^2$
iii. Extra stability of half-filled subshell is due to smaller exchange energy.
iv. Only two electrons, irrespective of their spin, may exist in the same orbital are.

The energy of electrons in atom is _____. (quantised/ not quantised)

If the radius of electron orbit in the excited state of hydrogen atom is $476.1 \mathrm{pm}$, the energy of electron in that excited state in $\mathrm{J}$ is (Radius and energy of electron in the first orbit of hydrogen atom are $52.9 \mathrm{pm}$ and $-2.18\times {10}^{-18} \mathrm{J}$ respectively)

According to the Bohr theory, which of the following transitions in the hydrogen atom will given rise to the least energetic photon?

Ionization energy of ${\mathrm{He}}^{+}$ is $19.6\times {10}^{-18}{\mathrm{Jatom}}^{–1}$. The energy of the first stationary state $(\mathrm{n} = 1)$ of ${\mathrm{Li}}^{2+}$ is