Electrons in stable orbits do not radiate Electrons can change orbits by radiating (larger to smaller), absorbing radiation (smaller to larger), or by collisions (either larger to smaller or smaller to larger) Solve problems and use available evidence to discuss the merits and limitations of the Bohr model of the atom See above for an explanation of the Bohr model of the atom MERITS The Bohr model introduced the newly developed quantum theory to the model of the atom, which established many important features of the atom, such as quantised energy differences between orbitals This explained the observation that excited atoms release generate line emission spectra His model successfully accounted for the observed emission spectrum , atomic radius, and ionisation energy of hydrogen with reasonable precision LIMITATIONS Attempts to extend the Bohr model of hydrogen to other elements and ions disagreed with the experimental line spectrum frequencies observed Bohr could not explain why only a restricted number of energy levels existed, or why the accelerating electrons did not lose energy Bohr also couldn’t explain the further analysis of the emission spectrum of hydrogen, such as the splitting of spectral lines when a magnetic field was applied His model couldn’t explain the relative intensities of the observed line spectra His model describes electrons in defined orbits around the nucleus, but this violates Heisenberg’s uncertainty principal as an electron’s there is a limit to the certainty of an electron’s position and momentum around the nucleus ASSESSMENT Whilst the Bohr model could not explain observations beyond the line spectra, his application of quantum theory to the model of the atom allowed the further for further development, thus it was an important development in the study of atoms Explain what is meant by n, the principal quantum number As discussed above, the Bohr model of the atom introduced the quantisation of angular momentum, which implied that electrons orbited around the nucleus in certain allowable radii that was associated with a specific energy level Each orbital radii or energy level can be represented by the principal quantum number, or n, which indicates the energy level of an electron The quantum number can only take an integer (i.e. 1, 2, 3, 4…) Energy levels with greater energy are assigned larger principal quantum number, so n=1 denotes the orbit closest to the radius, n=2 denotes the next energy level up, and so on Identify that, as electrons return to lower energy levels, they emit quanta of energy which humans may detect as a specific colour
Electrons in stable orbits do not radiate Electrons can change orbits by radiating (larger to smaller), absorbing radiation (smaller to larger), or by collisions (either larger to smaller or smaller to larger) Solve problems and use available evidence to discuss the merits and limitations of the Bohr model of the atom See above for an explanation of the Bohr model of the atom MERITS The Bohr model introduced the newly developed quantum theory to the model of the atom, which established many important features of the atom, such as quantised energy differences between orbitals This explained the observation that excited atoms release generate line emission spectra His model successfully accounted for the observed emission spectrum , atomic radius, and ionisation energy of hydrogen with reasonable precision LIMITATIONS Attempts to extend the Bohr model of hydrogen to other elements and ions disagreed with the experimental line spectrum frequencies observed Bohr could not explain why only a restricted number of energy levels existed, or why the accelerating electrons did not lose energy Bohr also couldn’t explain the further analysis of the emission spectrum of hydrogen, such as the splitting of spectral lines when a magnetic field was applied His model couldn’t explain the relative intensities of the observed line spectra His model describes electrons in defined orbits around the nucleus, but this violates Heisenberg’s uncertainty principal as an electron’s there is a limit to the certainty of an electron’s position and momentum around the nucleus ASSESSMENT Whilst the Bohr model could not explain observations beyond the line spectra, his application of quantum theory to the model of the atom allowed the further for further development, thus it was an important development in the study of atoms Explain what is meant by n, the principal quantum number As discussed above, the Bohr model of the atom introduced the quantisation of angular momentum, which implied that electrons orbited around the nucleus in certain allowable radii that was associated with a specific energy level Each orbital radii or energy level can be represented by the principal quantum number, or n, which indicates the energy level of an electron The quantum number can only take an integer (i.e. 1, 2, 3, 4…) Energy levels with greater energy are assigned larger principal quantum number, so n=1 denotes the orbit closest to the radius, n=2 denotes the next energy level up, and so on Identify that, as electrons return to lower energy levels, they emit quanta of energy which humans may detect as a specific colour
Chemistry_Notes_-_Chemistry_of_Art_by_Ian_Wilkinson.docx