Fully worked solutions will be appreicated :) Part A The figure below shows the

Question

Fully worked solutions will be appreicated :)

Part A The figure below shows the first four energy levels of the fictitious atom X E (eV) -2.0 3.0 n=3 11 (a) In your own words, explain what the term "ionisation energy" means. What is the ionisation energy of (b) What wavelengths are observed in the absorption spectrum of element X? Give your answer(s) in nm, and (c) If an atom of element X was illuminated with X-ray photons of 90 nm, would you expect electrons to be (d) It is said that the photoelectric effect demonstrates the particle-like nature of light. Explain how this element X? explain which transitions will occur. ejected? If so, what would the stopping voltage of the ejected electrons be? conclusion is reached. That is, what experimental evidence is consistent with particle-like behavior for light but not with wave-like behaviour? Cite at least two pieces of evidence

Explanation / Answer

a)

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. The first or initial ionization energy or Ei of an atom or molecule is the energy required to remove one mole of electrons from one mole of isolated gaseous atoms or ions.

You may think of ionization energy as a measure of the difficulty of removing electron or the strength by which an electron is bound. The higher the ionization energy, the more difficult it is to remove an electron.

Therefore, ionization energy is in indicator of reactivity. Ionization energy is important because it can be used to help predict the strength of chemical bonds.

The first ionization energy is 6.5eV

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