12.1 Electrons in Atoms

The successive ionisation energies of vanadium are shown.

State the sub-levels from which each of the first four electrons are lost

Outline why there is an increase in ionisation energy from electron 3 to electron 5.

Explain why there is a large increase in the ionisation energy between electrons 5 and 6.

IE1	IE2	IE3	IE4	IE5	IE6
578	1816	2744	11576	14829	18375

 

Explain the large increase in ionisation energy from IE₃ to IE₄

Determine the energy, in J, of a photon of red light, correct to two significant figures, given that the wavelength is 650.0 nm using Sections 1 and 2 of the Data Booklet.

The first ionisation energies of the elements in period 3 are shown below.

Explain the general trend seen in ionisation energy across period 3.

On the diagram below, sketch the line for the first ionisation energies of period 2 elements

Sketch a graph of ionisation energy versus the number of electrons removed for five ionisations of silicon. Explain the shape of the trend you have drawn.

The wavelength of a line in the Balmer series of hydrogen is 726.2 m. Calculate the energy of photons emitted, in kJ, using Sections 1 and 2 of the Data Booklet.

Draw a graph on the diagram to to show the second ionisation energies of the period 3 elements

Explain the differences seen in first and second ionisation energies of the elements in period 3.

Hydrogen spectral data give the frequency of 3.28 x 10¹⁵  s^-1 for its convergence limit.

On the diagram below, draw a line that corresponds to the first ionisation energy of hydrogen and explain your reasoning.