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An in-depth exploration of atomic structure, focusing on the periodic table, electronic configuration, and the relationship between electrons and electromagnetic radiation. Topics include atomic number, electronic structure, protons, neutrons, electrons, energy levels, and the electromagnetic radiation spectrum. The document also covers the fundamental equation of quantum theory and the dual behavior of subatomic particles.
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H
C
z =
6
C =
carbon
PA =
12,011g/mol
nucleous
Energy levels
THE ATOM: BRIEF REMINDER
THE ELECTROMAGNETIC RADIATION
•To understand the internal structure of the atoms that form thematter and how this organization relates with their chemicalproperties, it is necessary understand their electronic structure,that is how the electrons are arranged around a core.•The electronic structure of atoms can be indirectly addressed byobserving the properties of the electromagnetic radiation they emit.•The visible light, infrared radiation, microwaves, radio waves, x-rays and other forms of radiant energy are all electromagneticradiations, that only differ on the quantity of energy they carry. Thecomplete set of all of the different types is known as the electromagnetic spectrum
(
See next slides
).
Electric field
Magnetic field
THE ELECTROMAGNETIC RADIATION
10
10
)
nt
environtme
(any
v
c
)
( 10
(^7)
nm
THE ELECTROMAGNETIC RADIATION
Fundamental equation of quantum theory
h
= Planck’constant = 6,63. 10
J·s.
THE ELECTROMAGNETIC RADIATION:
ITS ENERGETICS
c
h
h
E
THE ATOM:
BORH MODEL
Increasing energetic magnitude of the orbits
One photon is released with an
energy proportional to the orbit leap
=E/h
THE ATOM:
BORH MODEL
THE ATOM:
THE WAVE FUCTION
l
THE ATOM: THE WAVE FUCTION.
BASIC CONCEPTS
Symbol
Orbital meaning
Range of values
Value examples
n
Shell
1
≤
n
n
= 1, 2, 3,
…
l
subshell
(s orbital is listed as 0, p
orbital as 1 etc.)
0
≤
l
≤
n
for
n
= 3:
l
= 0, 1, 2 (s, p, d)
m
l
e
nergy shift
(orientation of the subshell's
shape)
−
l
≤
m
l^
≤
l
for
l
= 2:
m
l
=
−
2,
−
1, 0, 1, 2
m
s
spin of the electron
(
−
½
= "spin down",
½
= "spin
up")
−
s
≤
ms
≤
s
for an electron
s
=
½
,so
ms
=
−
½
,
½
ℓ
s
THE ATOM:
THE QUANTUM NUMBERS
n
l
m
l
R(r)
Y(j,q)
1
0
0
2
Z a
0
3 2
e
Zr a
0
1 4
1 2
1s
2
0
0
Z 2
a
0
3 2
2
Zr a
0
e
Zr
2
a
0
1 4
1 2
2s
2
1
0
1
3
Z
2
a
0
3 2
Zr a
0
e
Zr
2
a
0
3 4
1 2
cos
2p
z
2
1
1
3
Z
2
a
0
3 2
Zr a
0
e
Zr
2
a
0
3 4
1 2
sen
cos
2p
x
2
1
1
3
Z
2
a
0
3 2
Zr a
0
e
Zr
2
a
0
3 4
1 2
sen
sen
2p
y
•The functions shape for the wave function of all the potentialelectronic states of the hydrogen electron are:
•Each solution gives a region of the space were the electron can bewhen its energy correspond to the quantity marked by
n
number.
THE ATOM:
THE QUANTUM NUMBERS
