Chemistry Reference
In-Depth Information
1 1
1
UU U
x
%%%
1
2
Δ
U
where
Δ
U
and
= potential energies of material points,
Δ
U
= resultant potential
2
1
energy of the system.
The electron with mass m, moving near the proton with mass Ɇ, is equivalent to
the particle with mass
mM
.
m
r
mM
Therefore, assuming that the energy of atom valence orbitals (responsible for in-
teratomic interactions) can be calculated by following the principle of adding the re-
ciprocals of some initial energy components. The introduction of Ɋ-parameter as an
averaged energy characteristic of valence orbitals is assigned [1] based on the follow-
ing equations:
1
1
1
1
1
1
(1), (2), (3)
or
:
PPr
2
Wn
PP
2
Wrn
q
q
E
0
r
i
i
E
0
i
i
where
W
i
= orbital energy of electrons [2],
r
i
= orbital radius of
i
-orbital [3],
q = Z*/n*
,
n
i
= number of electrons of the given orbital,
Z*
and
n*
= nucleus effective charge and
effective main quantum number [4, 5], r = bond magnitude.
In Equations (1, 2) the parameters
q
2
and
Wr
can be considered as initial (primary)
values of Ɋ
0
-parameter that are tabulated constants for the electrons of the given atom
orbital. For its dimensionality it can be written down as follows:
3
kg m
¸
¯
2
<> <><><><>
P
q
¸ ¸
E
r
h
V
Jm
¡
¢ ±
0
2
s
where [E], [h], and [ȣ] = dimensionality of energy, plank constant, and velocity.
At the same time, for like-charged systems (for example--orbitals in the given
atom) and homogeneous systems, the principle of algebraic addition of such param-
eters are preserved:
P
0
,
(4), (4ɚ)
P
P
r
P
E
0
i
E
r
Applying the Equation (4, 4ɚ) to hydrogen atom for initial values of P-parameters we
can obtain the following:
2
2
¬
¬
-
e
e
-
2
K
-
K
-
mc
M
(5)
-
-
® ®
n
n
1
2
where:
ɟ
= elementary charge,
n
1
and
n
2
= main quantum numbers,
m
= electron mass,
ɫ
= electromagnetic wave velocity,
λ
= wave length,
Ʉ
= constant.
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