Structure of the Atom (SL IB Physics)

The energy levels of a hydrogen atom are shown below.                                                                                  

Calculate the wavelength of radiation emitted when an electron falls from level n = 5 to the ground state in the hydrogen atom.

When an electron of energy 1.88 × 10⁻¹⁷ J collides with a hydrogen atom, photons of ten different energies are emitted.  

Sketch arrows on the diagram from part (a) to show the transitions responsible for these photons. 

Calculate the wavelength of the photon with the largest energy. Give your answer to an appropriate number of significant figures. 

One way to excite a hydrogen atom is by the absorption of a photon. 

Explain why, for a particular transition, the photon must have an exact amount of energy. 

The lowest energy levels of an argon atom are shown below. 

Calculate the wavelength of an emitted photon due to the transition level n = 5 to level n = 3.

Draw arrows on the diagram above to show the electron transitions which emit a photon with a longer wavelength than that emitted in the transition from n = 5 to n = 3.

A fluorescent tube is filled with argon gas at low pressure. When the argon atoms are excited, they emit photons.

Explain how the excited argon atoms emit photons.

Explain how the coating on the inside surface of the glass in a fluorescent tube helps to emit photons in the visible spectrum.

In a HeNe laser, electrons collide with helium atoms. The ground state of a helium is labelled as 1s and the next energy level is labelled 2s.

When an electrons de-excite from 2s to 1s in helium, photons are emitted with a wavelength of 58.4 nm.

Calculate the energy difference of this transition, giving your answer in eV.

An electron collides with a helium in its ground state, causing an electron to transition from 1s to 2s. The electron initially has 45.0 eV of kinetic energy.

Calculate the electron’s kinetic energy after the collision.

Explain why it is not possible for the same electron from (b) to collide with the ground state helium atom and be left with 40.0 eV of kinetic energy. 

Helium and neon coincidentally have very similar energy gaps for certain transitions, allowing one atom to cause an excitation in the other.

The excited helium atom from part (b) then collides with a ground state neon atom. The neon atom becomes excited and subsequently emits two photons in order to return to its ground state.

Rutherford used the scattering of α particles to provide evidence for the structure of the atom. The apparatus includes a narrow beam of α particles fired at a very thin sheet of gold foil inside a vacuum chamber.

Explain why it is essential to use:

[1]

[1]

[1]

The diagram shows α particles incident on a layer of atoms in a gold foil.

Outline the results of the scattering experiment by explaining:

[2]

[3]

The Thomson model of the atom preceded Rutherford’s model. In the Thomson model, the atom was imagined as a sphere of positive charge of diameter 10^–10 m containing electrons moving within the sphere.

Thomson’s model could explain some of the results of the Rutherford experiment, but not all.

Explain

[3]

[3]

Transitions between three energy levels in a particular atom give rise to three spectral lines.

In increasing magnitudes, these are related to the wavelengths, λ_a, λ_b, and λ_c,  

Use a diagram to show that the equation that relates λ_a, λ_b, and λ_c is:

An atom has a ground state energy of −6.60 eV. 

 

Sketch a diagram of the possible energy levels for the atomic line spectra to show that the wavelengths λ_a, λ_b, and λ_c satisfy the equation. 

Describe the nature of the atomic line spectra shown in part (b). 

Sir William Herschel discovered infrared radiation in 1800. The equipment he used is listed below:

• Glass prism
• Blackout curtains with an envelope slit to allow natural light through
• Thermometers

Explain how he discovered infrared radiation using this equipment. 

Two students debate which electron energy transition causes a photon of infrared radiation to be emitted from excited hydrogen atoms. 

Student 1 thinks it’s the transition to  .

Student 2 thinks it’s the transition  to .

State and explain which student is correct.

In a new type of special effects tube covered in a special infrared absorbent coating, the hydrogen atoms inside are excited. This leads to a series of events which result in the emission of photons in the visible region of the electromagnetic spectrum from the coating of the tube. 

Describe the series of events, following the excitation of the atoms, which results in the emission of visible photons.

Discuss the meaning of the first molar ionisation energy.

An electron is accelerated through an electric field between two parallel plates. The plates are separated by 2.2 cm and the electric field has a strength of 6.37 × 10² V m⁻¹.

Determine the kinetic energy of the electron in eV. 

The electron then hits a hydrogen atom in its ground state and excites it. 

Determine the range of wavelengths of all the photons that could be emitted as this electron returns to its ground state. 

Transitions between three energy levels in a particular atom give rise to three spectral lines. In decreasing magnitudes, these are , and .

The equation which relates , and  is:

Explain, including through the use of a sketch, how this equation relates ,  and .

A different atom has a complete line emission spectra with a ground state energy of  –10.0 eV. is:

Sketch and label a diagram of the possible energy levels for the atomic line spectra shown.

Explain the significance of an electron at an energy level of 0 eV.