Topic 1.3: Electron Configurations Questions

Deduce the maximum number of electrons that can occupy the third main energy level (n = 3), and name the three sublevels it contains. [2]

State the shape of an s orbital and the shape of a p orbital, and state how many p orbitals make up a p sublevel. [2]

The successive ionization energies of an element, in kJ mol-1, are 738, 1451, 7733, 10540. Deduce the group of the periodic table to which it belongs.

Draw the shape of an s orbital and of a p orbital.

Explain how the emission spectrum of hydrogen provides evidence that electron energy levels are discrete.

State the order of the regions of the electromagnetic spectrum in increasing energy, from radio waves to gamma rays, and state the relationship between energy and wavelength.

Explain why the lines in the emission spectrum of hydrogen converge at higher frequency.

State what happens at the convergence limit of the hydrogen emission spectrum and what quantity it can be used to determine.

Write the full electron configuration of a sulfur atom (Z = 16) and of a sulfide ion, S²⁻.

Write the full electron configuration of a calcium atom (Z = 20) and explain why the 4s sublevel fills before 3d.

State the maximum number of electrons that can occupy an s, a p and a d sublevel, and explain the pattern in terms of orbitals.

Write the condensed electron configuration of iron (Z = 26) using the noble gas core, and state the configuration of the Fe²⁺ ion.

State how many sublevels the third principal energy level contains, name them, and give the maximum number of electrons it can hold.

Explain what is meant by an orbital and state how many electrons one orbital can hold.

State the shapes of an s orbital and a p orbital, and state how many p orbitals there are in a given sublevel.

State the rule that determines how electrons occupy the three orbitals of a p sublevel, and apply it to nitrogen (Z = 7).

What is the electron configuration of a neutral sulfur atom, atomic number 16?

Explain why there is a large increase between the fourth and fifth successive ionization energies of an element.

Explain how the line emission spectrum of hydrogen provides evidence that the electron occupies discrete energy levels. [2]

The lines in the hydrogen emission spectrum get closer together (converge) toward the high-frequency end.

(a) State what this convergence tells us about the energy levels.

(b) State, with a reason, which transition emits the highest-energy photon. [3]