28 The hydrogen atom
Table 2.2 Radial hydrogenic wavefunctionsRn,lin terms of the variableρ =
Zr/(na 0 ), which gives a scaling that varies withn. The Bohr radiusa 0 is defined in
eqn 1.40.
R 1 , 0 =
(
Z
a 0
) 3 / 2
2e−ρ
R 2 , 0 =
(
Z
2 a 0
) 3 / 2
2(1−ρ)e−ρ
R 2 , 1 =
(
Z
2 a 0
) 3 / 2
2
√
3
ρe−ρ
R 3 , 0 =
(
Z
3 a 0
) 3 / 2
2
(
1 − 2 ρ+
2
3
ρ^2
)
e−ρ
R 3 , 1 =
(
Z
3 a 0
) 3 / 2
4
√
2
3
ρ
(
1 −
1
2
ρ
)
e−ρ
R 3 , 2 =
(
Z
3 a 0
) 3 / 2
2
√
2
3
√
5
ρ^2 e−ρ
Normalisation:
∫∞
0
R^2 n,lr^2 dr=1
These show a general a feature of hydrogenic wavefunctions, namely
that the radial functions forl= 0 have a finite value at the origin, i.e.
the power series inρstarts at the zeroth power. Thus electrons with
l= 0 (called s-electrons) have a finite probability of being found at the
position of the nucleus and this has important consequences in atomic
physics.
Inserting|E|from eqn 2.20 into eqn 2.17 gives the scaled coordinate
ρ=
Z
n
r
a 0
, (2.21)
where the atomic number has been incorporated by the replacement
e^2 / 4 π 0 →Ze^2 / 4 π 0 (as in Chapter 1). There are some important prop-
erties of the radial wavefunctions that require a general form of the
solution and for future reference we state these results. The probability
density of electrons withl= 0 at the origin is
|ψn,l=0(0)|^2 =
1
π
(
Z
na 0
) 3
. (2.22)
For electrons withl= 0 the expectation value of 1/r^3 is
〈
1
r^3
〉
=
∫∞
0
1
r^3
Rn,l^2 (r)r^2 dr=
1
l
(
l+^12
)
(l+1)
(
Z
na 0
) 3
. (2.23)
These results have been written in a form that is easy to remember;
they must both depend on 1/a^30 in order to have the correct dimensions
and the dependence onZfollows from the scaling of the Schr ̈odinger