7. An electron is accelerated through a potential difference of 12.1 V. n = 5 -0.54 eV 0.8 eV n = 3 -1.5 eV n = 2 -3.4 eV n = 1 -13.6 eV (a) How much kinetic energy has it gained in (i) electronvolts (ii) joules? (b) This electron hits a hydrogen atom and excites it. (i) Explain what is meant by excitation (ii) Using the energy values given in the diagram above, work out the two energy levels between which this accelerated electron will likely produce a transition. (iii) Calculate the energies of the three photons that might be emitted as the electron return to the ground state.

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Question 7 b(ii) , b(iii) and 7 a(ii) , 7a(i) 

7. An electron is accelerated through a potential difference of 12.1 V.
n =
n
0.54 eV
0.8 eV
n = 3
-1.5 eV
n = 2
-3.4 eV
n = 1
-13.6 eV
(a) How much kinetic energy has it gained in (i) electronvolts (ii) joules?
(b) This electron hits a hydrogen atom and excites it.
(i) Explain what is meant by excitation
(ii) Using the energy values given in the diagram above, work out the two energy levels between which this
accelerated electron will likely produce a transition.
(iii) Calculate the energies of the three photons that might be emitted as the electron return to the ground state.
8. The three lowest energy levels of an atom are shown below.
-1.6 eV
-6.2 eV
n =
n = 2
n = 1
-18.6 eV
(i) Determine the minimum energy in joule required to eject an electron initially in the lowest energy level from
the atom.
k
(ii) Assuming that the energy level, n, is associated with energy
determine the energy of the level n = 4 in
electronvolts.
(iii) Determine the wavelength of the electromagnetic radiation emitted when an electron makes a quantum
jump from the level n
3 to the level n =
2. Name the region of the electromagnetic spectrum in which this
radiation is found.
|||||
Transcribed Image Text:7. An electron is accelerated through a potential difference of 12.1 V. n = n 0.54 eV 0.8 eV n = 3 -1.5 eV n = 2 -3.4 eV n = 1 -13.6 eV (a) How much kinetic energy has it gained in (i) electronvolts (ii) joules? (b) This electron hits a hydrogen atom and excites it. (i) Explain what is meant by excitation (ii) Using the energy values given in the diagram above, work out the two energy levels between which this accelerated electron will likely produce a transition. (iii) Calculate the energies of the three photons that might be emitted as the electron return to the ground state. 8. The three lowest energy levels of an atom are shown below. -1.6 eV -6.2 eV n = n = 2 n = 1 -18.6 eV (i) Determine the minimum energy in joule required to eject an electron initially in the lowest energy level from the atom. k (ii) Assuming that the energy level, n, is associated with energy determine the energy of the level n = 4 in electronvolts. (iii) Determine the wavelength of the electromagnetic radiation emitted when an electron makes a quantum jump from the level n 3 to the level n = 2. Name the region of the electromagnetic spectrum in which this radiation is found. |||||
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