14. Explanation:Explanation:
Bohr’s atomic theory isn't a lawBohr’s atomic theory isn't a law
yet. If anyone comes andyet. If anyone comes and
researches more about it, thenresearches more about it, then
this theory can have changes too.this theory can have changes too.
It will continue to have changesIt will continue to have changes
until it becomes a law.until it becomes a law.
Bohr introduced the radius=rBohr introduced the radius=r
relating to the nucleusrelating to the nucleus
Electrons are arranged it aElectrons are arranged it a
quantized orbit which is alsoquantized orbit which is also
called fixed energy.called fixed energy.
-
17. The Bohr model of the atom, like many ideas in
the history of science, was at first prompted by
and later partially disproved by experimentation.
http://en.wikipedia.org/wiki/Category:Chemistry
Increasing energy
of orbits
n = 1
n = 2
n = 3
A photon is emitted
with energy E = hf
e-
e-
e-
e-
e-
e-
e-
e-
e-
e-
e-
18. According to classical
physics, light
should be emitted as the
electron
circles the nucleus. A loss of
energy
would cause the electron to
be drawn
closer to the nucleus and
eventually
spiral into it.
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 294
19. Q1.What are sub shells?
Q2.What is the meaning of energy level?
Q3.Atomic models are related to which model?
Q4.How will the electrons fall into the nucleus?
Q5.Explian emission of energy which electron takes
or gives?
Q6.What are electrons?
Q7.How can we find the number of protons ?
Q8. What is the another name for energy level?
Q9.Which type of foil did Rutherford use? And what
was its thickness?
Q10.What do you mean by arrangement of electrons?
Objectives:
To describe the Bohr model of the atom.
To explain the relationship between energy levels in an atom and lines in an emission spectrum.
In 1913, Niels Bohr proposed a theoretical model for the hydrogen atom that explained its emission spectrum.
– His model required only one assumption: The electron moves around the nucleus in circular orbits that can have only certain allowed radii.
– Bohr proposed that the electron could occupy only certain regions of space
– Bohr showed that the energy of an electron in a particular orbit is
En = – hc
n2
where is the Rydberg constant, h is the Planck’s constant, c is the speed of light, and n is a positive integer corresponding to the number assigned to the orbit.
n = 1 corresponds to the orbit closest to the nucleus and is the lowest in energy.
A hydrogen atom in this orbit is called the ground state, the most stable arrangement for a hydrogen atom.
As n increases, the radii of the orbit increases and the energy of that orbit becomes less negative.
A hydrogen atom with an electron in an orbit with n >1 is in an excited state — energy is higher than the energy of the ground state.
Decay is when an atom in an excited state undergoes a transition to the ground state — loses energy by emitting a photon whose energy corresponds to the difference in energy between the two states.