Explain why the Bohr model was insufficient and how the quantum model explained this deficiency. How is the electron viewed differently in each model

Answer and Explanation:

Bohr's model of the atom defined the electron as a particle that orbits around the nucleus in only certain orbital levels. As a result, it couldn't readily give account of the energy levels of larger elements with high atomic number.

The quantum model of the atom however, approaches the electron in an atom as not just a particle but a wave, with its distinct quantum number per energy level. It can therefore give the position and speed of an electron simultaneously at any energy level.

I hope this explanation is sufficient.

iron and sleel

make siroeel

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."