Degeneracy in hydrogenic atoms

Degeneracy in hydrogenic atoms refers to the number of possible states corresponding to a given energy value of a hydrogenic wavefunction.

The total wavefunction of a hydrogenic atom is characterised by three quantum numbers: , and . This implies that the state of the atom is defined by the set of quantum numbers . However, in a hydrogenic atom, the nucleus acts effectively as a point charge, and the electrostatic potential energy is spherically symmetric. This spherical symmetry means that the energy of the electron depends only on its distance from the nucleus. In other words, the energy of the electron is the eigenvalue associated with the radial component of the total wavefunction. As shown in eq462b, this eigenvalue is governed solely by the principal quantum number . Consequently, all the possible energy states defined by for a given must have the same energy and are therefore degenerate.

Since (see this article for explanation) and (see eq462a), the possible values of the orbital angular momentum quantum number range from 0 to for a given . Furthermore, for each value of , the magnetic quantum number can take on values (see this article for explanation). Therefore, the degeneracy for a given  is the sum of all the possible values of for each from 0 to :

 

Question

Show that .

Answer

The proof is in the 3rd Q&A of this article.

 

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Node

A node is a region in space where a wavefunction is zero. This implies that the probability of finding an electron at a node is zero. Since a wavefunction can have two components—radial and angular—it can have both radial and angular nodes.

A radial node is a spherical surface where the radial wavefunction of an atomic orbital is zero. The number of radial nodes in a hydrogenic wavefunction is given by the formula:

where is the principal quantum number and is the angular momentum quantum number.

 

Question

How is eq471 derived?

Answer

When , the associated Laguerre polynomial . Since the upper summation index of the explicit form of is , the polynomial will have roots if . In other words, will be zero (a node) as many times as .

 

An angular node is a flat plane or a cone where the angular wavefunction (also known as spherical harmonics) is zero. Using the same logic, the number of angular nodes  in corresponds to the number of roots when , where  are the associated Legendre polynomials. Since , the polynomial is of degree . Therefore,

The total number of nodes in is

The number of radial nodes helps define the spatial distribution of the electron density in orbitals. In other words, they influence the shape and energy of these orbitals, and therefore play a role in chemical bonding between orbitals.

 

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s-orbital

An s-orbital is a spherical region of space around the nucleus where an electron with zero orbital angular momentum is most likely to be found. The letter ”s” is of spectroscopic origin, standing for ‘sharp’.

One-electron s-orbital wavefunctions can be expressed using the total wavefunction of a hydrogenic atom:

where

, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .

The principal quantum number, , is also called a shell. Since the first shell is characterised by , the one-electron s-orbital wavefunction in the first shell, known as the 1s orbital, is defined by the set of quantum numbers . Substituting these values into the explicit formula for  yields:

Similarly, the one-electron s-orbital wavefunction in the second shell, known as the 2s orbital, is defined by the set of quantum numbers and has the formula:

Since  for all s-orbitals, their wavefunctions are independent of and . This implies that the values of an s-orbital wavefunction are the same in all directions in 3D space for a given . In other words, s-orbital wavefunctions are spherically symmetrical.

Finally, the 1s orbital and 2s orbital have 0 radial nodes and 1 radial node, respectively (see above diagram).

 

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Total wavefunction of a hydrogenic atom

The total wavefunction of a hydrogenic atom characterises the probability of locating an electron around the nucleus by incorporating both radial and angular components.

This spatial wavefunction is mathematically defined as:

where

, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .
is the distance between an electron and the nucleus of a hydrogenic atom.
is the polar angle.
is the azimuthal angle.
is the Bohr radius.
is the reduced mass of the atom.
is the ratio of the Planck constant and .
is the atomic number of the atom.
is the vacuum permittivity.

 

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p-orbital

A p-orbital, defined by the quantum number , is a dumbbell-shaped region of space around the nucleus where an electron is most likely to be found. The letter ”p” is of spectroscopic origin, standing for ‘principal’.

One-electron p-orbital wavefunctions can be expressed using the total wavefunction of a hydrogenic atom:

where

, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .

The principal quantum number, , is also called a shell. Since when , there are three p-orbitals that are characterised by the set of quantum numbers  of , and in each shell for . Each of the three p-orbitals has an angular node. Consider the set . Substituting these values into the explicit formula for  yields:

where .

Converting from spherical coordinates to Cartesian coordinates, where , gives

Eq474 is known as the orbital. When , the wavefunction is zero everywhere in the -plane, which is known as the nodal plane.

For the sets and , we have  and , respectively. These two wavefunctions include the factor , which may complicate calculations when they undergo symmetry operations. Therefore, we take linear combinations of these wavefunctions to form simpler wavefunctions. The first linear combination is , which normalises to , or equivalently in Cartesian coordinates:

since .

The second normalised linear combination is , or equivalently,

since .

and , like , each have an angular node.

 

Question

If and are already normalised, why do we need to normalise a linear combination of them? How do we normalise a linear combination of and ?

Answer

When forming a linear combination of normalised wavefunctions, the result is not necessarily normalised. Consider a general linear combination , where and are coefficients. The normalisation condition for requires that , where  represents the volume element in spherical coordinates. Expanding and noting that and are orthonormal, we have . If , which is the case for the two linear combinations of and , will not be normalised.

To normalise , we have  or

Using (see this article for proof) and some basic trigonometry identities yields

Setting and gives .

 

 

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d-orbital

A d-orbital, defined by the quantum number , is a region of space around the nucleus where an electron is most likely to be found. The letter ”d” is of spectroscopic origin, standing for ‘diffuse’.

One-electron d-orbital wavefunctions can be expressed using the total wavefunction of a hydrogenic atom:

where

, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .

The principal quantum number, , is also called a shell. Since when , there are five d-orbitals that are characterised by the set of quantum numbers  of , , , and in each shell for . Four of the five d-orbitals have cloverleaf shapes, while the fifth has a lobular structure along the -axis with a doughnut-shaped region around the equatorial plane. Each of the five d-orbitals has two angular nodes. Consider the set . Substituting these values into the explicit formula for  yields:

where .

Converting from spherical coordinates to Cartesian coordinates, where , gives

Eq478 is known as the wavefunction for the orbital. When or , . Therefore, the wavefunction is zero at in spherical coordinates. This implies that the angular nodes occur at two conical surfaces with their apices at the origin, extending at along the -axis.

For the sets and , we have  and , respectively. These two wavefunctions include the factor , which may complicate calculations when they undergo symmetry operations. Therefore, we take linear combinations of these wavefunctions to form simpler wavefunctions. The first linear combination is , which normalises to , or equivalently in Cartesian coordinates:

where and .

when or . This implies that has two nodal planes:  and .

 

Question

If and are already normalised, why do we need to normalise a linear combination of them? How do we normalise a linear combination of and ?

Answer

When forming a linear combination of normalised wavefunctions, the result is not necessarily normalised. Consider a general linear combination , where and are coefficients. The normalisation condition for requires that , where  represents the volume element in spherical coordinates. Expanding and noting that and are orthonormal, we have . If , which is the case for the two linear combinations of and , will not be normalised.

To normalise , we have  or

Since and ,

Using (see this article for proof) and setting and gives .

 

The second normalised linear combination is , or equivalently,

where and .

when or . This implies that has two nodal planes:  and .

For the remaining sets and , we apply the same logic to give and , where . when or , which implies two diagonal nodal planes. when or , which implies two nodes described by the planes and .

 

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f-orbital

An f-orbital, defined by the quantum number , is a region of space around the nucleus where an electron is most likely to be found. The letter ”f” is of spectroscopic origin, standing for ‘fundamental’. f-block elements have either hexagonal close pack, cubic close pack or body centred cubic structures. For non-cubic symmetry systems, we describe them using a general set of orbitals, which are derived in the same way as the d-orbitals. For cubic symmetry systems, they are better described by another set of f-orbitals known as the cubic set, which are derived by taking a different set of linear combinations. Both sets are eigenfunctions of the Schrödinger equation.

One-electron f-orbital wavefunctions can be expressed using the total wavefunction of a hydrogenic atom:

where

, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .

 

General set

The principal quantum number, , is also called a shell. Since when , there are seven f-orbitals that are characterised by the set of quantum numbers  of , , , , , and in each shell for . Each of the seven f-orbitals has three angular nodes. Consider the set . Substituting these values into the explicit formula for  yields:

where .

Converting from spherical coordinates to Cartesian coordinates, where , gives

Eq482 is known as the orbital. When or or , . represents the nodal plane, while implies that the angular nodes occur at two conical surfaces with their apices at the origin, extending at along the -axis.

For the sets and , we have  and , respectively. These two wavefunctions include the factor , which may complicate calculations when they undergo symmetry operations. Therefore, we take linear combinations of these wavefunctions to form simpler wavefunctions. The first linear combination is , which normalises to , or equivalently in Cartesian coordinates:

where , and .

One angular node occurs at  or when , which represents the -nodal-plane. The second and third angular nodes correspond to . These nodes are described by two conical surfaces with their apices at the origin, extending at along the -axis.

The second normalised linear combination is , or equivalently,

where .

One angular node occurs at , which represents the -nodal plane. The second and third angular nodes correspond to . These nodes are described by two conical surfaces with their apices at the origin, extending at along the -axis.

 

Question

If and are already normalised, why do we need to normalise a linear combination of them? How do we normalise a linear combination of and ?

Answer

When forming a linear combination of normalised wavefunctions, the result is not necessarily normalised. Consider a general linear combination , where and are coefficients. The normalisation condition for requires that , where  represents the volume element in spherical coordinates. Expanding and noting that and are orthonormal, we have . If , which is the case for the two linear combinations of and , will not be normalised.

To normalise , we have  or

Using (see this article for proof),  and setting and gives .

 

For the remaining sets , , and , we apply the same logic to give:

Wavefunction Angular nodes

-plane

-planes

-plane

-plane

-plane

-plane

-planes

-plane

-planes

 

Cubic set

Out of the seven cubic f-orbitals, three of them, ,  and are the same as the general set of f-orbitals. The other four derived by taking different linear combinations of general set of f -orbitals. They are:

Linear combination Normalised wavefunction Angular nodes

-plane

Conical surfaces with apices at the origin, extending along the -axis

-plane

Conical surfaces with apices at the origin, extending along the -axis

-plane

-planes

-plane

-planes

 

Question
    1. How do we know which set of linear combinations result in the cubic set of wavefunctions?
    2. How do we determine the angular nodes of ?
Answer
    1. The linear combinations that give the cubic set of wavefunctions must transform according to the point group.
    2. The angular nodes occur when , which implies that or . Obviously, corresponds to the -nodal-plane. , which states that increases as increases in spherical coordinates, represents two conical surfaces with their apices at the origin. Substituting gives . When (along the -axis), the angles that the conical surfaces make with the -axis are .

 

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Binomial theorem and the binomial series

The binomial theorem (or binomial expansion) expresses how to expand the power of a sum of two variables into a series of terms involving the individual powers of each variable, with coefficients determined by their positions in the expansion.

In general, the binomial expansion of  is

where are variables, and are non-negative integers and are the binomial coefficients.

The binomial theorem can be proven by induction. For , we have

If the theorem holds for all when , then for ,

Substituting for the first summation yields . Changing the index from back to gives

 

Question

Show that .

Answer

 

Therefore,

and the theorem holds for all and .

The binomial theorem defines . This is evident from eq319, where

The binomial series, on the other hand, is a more general concept where  can be any real number, including negative and fractional values. If one of the variables in eq319 is equal to one and the absolute value of the other variable is less than one, the binomial series provides a way to express an infinite series that converges:

 

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Generating function for the Legendre Polynomials

The generating function for the Legendre polynomials is a mathematical tool that, when expanded as a power series, produces Legendre polynomials as its coefficients in terms of a variable.

Legendre polynomials often arise in problems involving spherical harmonics. An example (see diagram above) is the multipole expansion . As the two points and the angle between them form a triangle, the Legendre polynomials are related to the cosine rule , which can be rearranged to

where and .

Since , we have and hence . This implies that we can expand the RHS of eq343 as a binomial series:

The coefficients of are the Legendre polynomials. Therefore, the generating function for the Legendre polynomials is

 

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Recurrence relations of the Legendre Polynomials

The recurrence relations of the Legendre polynomials describe how each polynomial in the sequence can be obtained from its predecessors.

Some useful recurrence relations of the Legendre polynomials include

where .

To derive these relations, we differentiate eq345 with respect to and to give

and

respectively.

Substituting eq345 in eq346f yields

Equating the coefficents of gives

Substituting eq346e in eq346f results in . When we equate the coefficients of in this equation, we get eq346b. Combining eq346b and eq346g gives eq346a. Substracting eq346b from eq346a yields eq346c.

The last recurrence relation is obtained by substituting eq345 in eq346e to give . Expanding and equating coefficients of , we have eq346d.

 

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