Explain, with reference to the electronic transitions involved, how characteristic flame colours of metal ions are formed and why the flame colours are different.


To answer this we need to talk about how electrons move in an atom. Electrons are in energy levels (orbitals) and an electron in the highest unoccupied orbital can be excited to a higher shell when given enough thermal energy (heat) from the flame (must make sure you refer back to the specifics of a question). This electron then drops back down to its ground state (the shell it was previously in), and this causes a photon to be emitted with energy equivalent to the difference in energies between the two states/orbitals. Different metal ions have different sized gaps between their orbitals (energy levels) and so the energy of the photon emitted will change, hence the wavelength of the photon ( E=hc/f although this is beyond the scope of the syllabus it might be useful to teach some students also studying physics as it would give them a better understanding of the atom and its implications).

Answered by Isabel K. Chemistry tutor

4153 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is a bond?


A sample of CaCO3 has been weighed in at 6.3 g. How many moles of calcium carbonate are present?


Draw an example using a diagram of Carbon, three "Y" substrates and an "L" indicating any leaving group the Sn1 nucleophilic substitution reaction. (3 marks) Which step is fastest (1 mark).


What is a buffer solution? How to make a buffer solution?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo
Cookie Preferences