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The Bohring World of Niels Bohr
In 1913WBohr proposed that electrons are arranged in concentric circular paths or orbits around the
nucleus. Bohr answered in a novel way why electrons which are attracted to protons, never crash into
the nucleus. He proposed that electrons in a particular path have a fixed energy. Thus they do not lose
energy and crash into the nucleus. 7カje energy /eve/ of g/) e/ecro7 5 太e 7eg/O7 g7Ounの のe 70C7eus
Were た5がeルfo pe. These energy levels are like rungs on a ladder, lower levels have less energy and
work. The opposite is also true if an electron loses energy it falls to a lower level. Also an electron can
only be found
rungs of a ladder. The amount of energy gained or lost by every electron is not always the same. Unlike
the rungs of a ladder, the energy levels are not evenly spaced. 4 gug/fg77 O7 ene79y 75 妨e 977Ou7た Oげ
ener9y ee0eg ro 77oVe 7 e/ecfron廊O77 745 prese7t
_ene/rgy 7eve/ 7O je exf jgカer oe or to make a quantum
leap-
The Quantum Mechanical Model
Like the Bohr model, the ggg74777 776c7g77Co/ 777Oe/
leads to gugn67ze9 energy levels for an electron.
However the Quantum Mechanical model does not define
the exact path an electron takes around the nucleus. It is
concerned with the likelihood of finding an electron in a
certain position. This probability can be portrayed as a
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Figure 3A
Classical Alomic
Schematic of Carbon
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Figure 3B
New Atomic Schematic of Carbon
1 nucleus while
Gtrostatc equivalents keep
Envelopes separale
Figure 3C
New Atomic Schematic of Oxygen
(Electron Envelope above page not shown)
blurry cloud of negative charge (electron cloud). The cloud is most dense where the electron is likely to 人M
be.
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