Calculating avg distance from nucleus

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In summary, the conversation discusses calculating the average distance from the Hydrogen nucleus for an electron in the 2p state. The relevant equation for this is <r> = int[r^3 |R|^2]dr from 0->infinity. However, this equation is only valid for spherically symmetric wavefunctions. For the 2p state, the wavefunction is not spherically symmetric, so a more general equation must be used, which takes into account all three dimensions. The given solution for the 2p state, R = (1/a)^3/2 (1/(2*sqrt(sigma))*sigma*exp(-sigma/2), does not seem to be correct.
  • #1
jaejoon89
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Homework Statement



Calculate the avg. distance from the Hydrogen nucleus for an electron in 2p.

Homework Equations



<r> = int[r^3 |R|^2]dr from 0->infinity

For Hydrogen 2p, R = (1/a)^3/2 (1/(2*sqrt(sigma))*sigma*exp(-sigma/2)

where sigma = r/a

The Attempt at a Solution



I get 1/4a^4 (24 a^5) = 6a but the answer's supposed to be 5a. (5a for 2p is supposed to be less than 6a, which is the avg distance for 2s.) What am I doing wrong?
 
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  • #2
jaejoon89 said:
<r> = int[r^3 |R|^2]dr from 0->infinity

That's only true when the wavefunction is spherically symmetric. In general,

[tex]\langle r\rangle=\int_{\text{all space}}r|\psi(\textbf{r})|^2d^3\textbf{r}=\int_0^{\infty}\int_0^{\pi}\int_0^{2\pi}|\psi(\textbf{r})|^2r^3\sin\theta dr d\theta d\phi[/tex]

For Hydrogen 2p, R = (1/a)^3/2 (1/(2*sqrt(sigma))*sigma*exp(-sigma/2)

where sigma = r/a

That doesn't look quite right. Where did you get this from?
 
Last edited:

1. What is the formula for calculating the average distance from the nucleus?

The formula for calculating the average distance from the nucleus is given by the Bohr model of the atom, which states that the average distance is equal to the product of the principal quantum number (n) and the Bohr radius (a0). Mathematically, it can be represented as r = n*a0.

2. How is the average distance from the nucleus related to the energy level of an electron?

The average distance from the nucleus is directly related to the energy level of an electron. As the energy level increases, the average distance from the nucleus also increases. This is because higher energy levels have larger values of n, which leads to a greater distance from the nucleus according to the Bohr model.

3. Can the average distance from the nucleus be calculated for all types of atoms?

Yes, the average distance from the nucleus can be calculated for all types of atoms. The Bohr model can be applied to any atom, regardless of its atomic number or electron configuration. However, it should be noted that the Bohr model is a simplified representation of atomic structure and does not fully account for the complexities of electron behavior.

4. How does the average distance from the nucleus change for different electron orbitals?

The average distance from the nucleus varies for different electron orbitals. According to the quantum mechanical model of the atom, each electron orbital has a specific shape and size, with the most probable distance from the nucleus being different for each orbital. For example, the 1s orbital has the smallest average distance from the nucleus, while the 7s orbital has the largest.

5. Does the average distance from the nucleus affect the reactivity of an atom?

Yes, the average distance from the nucleus can affect the reactivity of an atom. Atoms with a smaller average distance from the nucleus tend to be more reactive, as their outermost electrons are held less tightly and are therefore more easily involved in chemical reactions. This is why elements in the same group of the periodic table have similar reactivity, as they have the same number of electrons in their outermost energy level and therefore similar average distances from the nucleus.

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