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]

State the full electron configuration of a calcium atom (Z = 20), and explain why 4s is written before 3d in the filling order.

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]

Explain why the successive ionization energies of an element always increase, and why a single large jump appears between the 1st and 2nd ionization energies of a Group 1 element.

The first six successive ionization energies of an element Q (kJ mol⁻¹) are: 590, 1 145, 4 912, 6 491, 8 153, 10 496.

Deduce the group of Q, and explain how the data lead to your answer.

Deduce the full electron configuration of the chromium(III) ion, Cr³⁺.

(Chromium has atomic number 24.)