Light from Electron Configurations
Source/Author: Daniel Burkett, US Science Teacher
September 25, 2020
Shorecrest Upper School Chemistry students have been learning about the arrangement of electrons in atoms and ions. These differences can be observed when students introduce ions to a flame, forcing electrons into higher energy orbitals. As the electrons "relax" back to their ground state, a characteristic color of light is emitted based on the element's electron configuration. In the top photo you can see the characteristic yellow-green flame from the barium ion.
The Chargers also learned about hydrates - crystalline compounds that incorporate molecules of water into their structure. By heating a hydrate of copper (II) sulfate, a blue crystalline compound, students were able to drive off the water from the crystalline compound, observing the brilliant blue color of the hydrate fade to a dull, ashy blue (bottom photo). Measuring the mass of the compound before and after heating allowed the students to determine the empirical formula of the hydrate, making use of several calculations that were discussed in class over the past couple of weeks.
The Chargers also learned about hydrates - crystalline compounds that incorporate molecules of water into their structure. By heating a hydrate of copper (II) sulfate, a blue crystalline compound, students were able to drive off the water from the crystalline compound, observing the brilliant blue color of the hydrate fade to a dull, ashy blue (bottom photo). Measuring the mass of the compound before and after heating allowed the students to determine the empirical formula of the hydrate, making use of several calculations that were discussed in class over the past couple of weeks.
