How come Niels Bohr's electron planetary model could not be applied Universely?

Answer 1

Because it was not an accurate representation of an atom. Electrons circling a nucleaus can really be anywhere is space around a nucleus. Based on the energy level of the electron, there are probablity fields that say where it will most likely be, but there is not determining that for sure, it is all probability.

Also, Bohr's model was only 2-dimensional. The real word is 3 dimensional.

Answer 2

Pretty much everything in quantum mechanics deals with probability. You can't say where exacly an electron will be, but you can figure out the probability of it being n a certain place. Bohr's planetary model didn't deal with that, it was giving the exact locations of electrons, but again we dont know exactly where the electrons are located.

Answer 3

Because it did not fit with observation and experimental results. Physicists found that they could either detect an electron's position around the nucleus of the atom or they could detect its velocity, but never both.

It all depends on which kind of test you're applying. If you are looking for location, you cannot measure speed and vice versa.

Also, atoms can exist in multiple states of energy, with only a "probability" of encountering any particular energy level. Bohr's model did not predict these situations.