Question

In: Chemistry

The energy difference between n=11 and n=12 for an atom is 3.50x10-19 J and the energy...

The energy difference between n=11 and n=12 for an atom is 3.50x10^-19 J and the energy difference between n=12 and n=13 is 2.50x10^-19 J, if an electron makes a transition from n=11 to n=13 by absorbing a photon, calculate the wavelength of the absorbed photon (express in nm)?

1,987.8

331.3

993.9

662.6

165.6

When a photon was used to eject an electron from the metal, the kinetic energy of the ejected electron was found to be 3.626x10^-19 J. If the work function or binding energy of the metal is 3.00x10^-19 J, what is the wavelength of the photon used (in nm)?

900

500

400

600

300

For a particle with mass m in a one dimensional box of lenth L, the energy is given by: E_n=n²h²/(8mL²). If the same particle is now placed in another one dimensional box of length 2L, for the same energy level (i.e. the same quantum number n), the energy should be __x___ times the energy for the first box.

8

1/2

2

4

1/4

Expert Solution

queen_honey_blossom answered 2 years ago

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Consider the following energy levels of a hypothetical atom: E4 −1.31 × 10−19 J E3 −4.61...

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The absolute value of ∆E (J) for an atom is equal to Ephoton, the energy of...

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Calculate the energy (J) of the photon emitted when an electron in the hydrogen atom falls...

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Find the wavelength (in nm) of a photon whose energy is 9.00 × 10-19 J.