(D) Given energy $E = 2 \ eV = 2 \times 1.602 \times 10^{-19} \ J = 3.204 \times 10^{-19} \ J$.For wavelength $(\lambda)$: $E = \frac{hc}{\lambda} \im

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$6.204 \times 10^{-7} \ m, 4.8 \times 10^{14} \ s^{-1}$

(D) Given energy $E = 2 \ eV = 2 \times 1.602 \times 10^{-19} \ J = 3.204 \times 10^{-19} \ J$.For wavelength $(\lambda)$: $E = \frac{hc}{\lambda} \implies \lambda = \frac{hc}{E}$.$\lambda = \frac{6.626 \times 10^{-34} \ J \cdot s \times 3 \times 10^8 \ m \cdot s^{-1}}{3.204 \times 10^{-19} \ J} = 6.204 \times 10^{-7} \ m$.For frequency $(\nu)$: $\nu = \frac{c}{\lambda} = \frac{3 \times 10^8 \ m \cdot s^{-1}}{6.204 \times 10^{-7} \ m} = 0.4835 \times 10^{15} \ s^{-1} \approx 4.8 \times 10^{14} \ s^{-1}$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

Difficult

The wavelength and frequency of a photon with energy $2 \ eV$ are respectively:

A
$6.204 \times 10^{-5} \ m, 3.65 \times 10^{14} \ s^{-1}$
B
$5.204 \times 10^{-7} \ m, 8.22 \times 10^{-10} \ s^{-1}$
C
$4.504 \times 10^{-6} \ m, 3.38 \times 10^{-10} \ s^{-1}$
D
$6.204 \times 10^{-7} \ m, 4.8 \times 10^{14} \ s^{-1}$

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Structure of Atom

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Atomic models and Planck's quantum theory

An electron initially present in an excited state of $H$ atom is further excited to another energy level by an incident photon. It releases $10$ photons while coming back to the ground state,out of which $7$ have higher energy than the incident photon. The electron was initially present in:

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Supposing the energy (in arbitrary units) of the energy levels in the hydrogen atom is given as under:

Energy level $K$ $(n=1)$ $L$ $(n=2)$ $M$ $(n=3)$ $N$ $(n=4...n=\infty)$

Energy $-864 \ a.u.$ $-216 \ a.u.$ $-96 \ a.u.$ $0 \ a.u.$

The excitation energy needed to raise the electron from $M$ level to $n = \infty$ would be:

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In the hydrogen spectrum,a line corresponds to a transition from the $3^{rd}$ to the $5^{th}$ orbit. Identify the series to which this transition belongs.

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The wavelength of $H_{\alpha}$ line of Balmer series is $X \ \mathring{A}$. What is the wavelength of $H_{\beta}$ line of Balmer series?

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What is the wavenumber of the photon emitted during transition from the orbit $n=5$ to that of $n=2$ in hydrogen atom (in $cm^{-1}$)?
$\left[R_{H}=109677 \ cm^{-1}\right]$

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Energy level	$K$ $(n=1)$	$L$ $(n=2)$	$M$ $(n=3)$	$N$ $(n=4...n=\infty)$
Energy	$-864 \ a.u.$	$-216 \ a.u.$	$-96 \ a.u.$	$0 \ a.u.$

The wavelength and frequency of a photon with energy $2 \ eV$ are respectively:

Similar Questions

An electron initially present in an excited state of $H$ atom is further excited to another energy level by an incident photon. It releases $10$ photons while coming back to the ground state,out of which $7$ have higher energy than the incident photon. The electron was initially present in:

In the hydrogen spectrum,a line corresponds to a transition from the $3^{rd}$ to the $5^{th}$ orbit. Identify the series to which this transition belongs.

The wavelength of $H_{\alpha}$ line of Balmer series is $X \ \mathring{A}$. What is the wavelength of $H_{\beta}$ line of Balmer series?

What is the wavenumber of the photon emitted during transition from the orbit $n=5$ to that of $n=2$ in hydrogen atom (in $cm^{-1}$)?$\left[R_{H}=109677 \ cm^{-1}\right]$

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What is the wavenumber of the photon emitted during transition from the orbit $n=5$ to that of $n=2$ in hydrogen atom (in $cm^{-1}$)?
$\left[R_{H}=109677 \ cm^{-1}\right]$