# Question #03a79

##### 1 Answer

#### Answer:

#### Explanation:

I will give an explanation for the basis of Slater's Rules which I have given in a previous answer.

Then I will apply this to a 4p electron in selenium (Z=34).

Consider an atom like sodium in the gaseous state:

Sodium has 11 protons in its nucleus i.e

The presence of the other 10 electrons has the effect of "shielding" or "screening" the outer electron from the attractive force of the nucleus.

This means that it experiences an attraction for the nucleus which is less than you would expect from the 11 protons.

This is referred to as the "effective nuclear charge" or

So we can write:

Where

In 1930 John Slater worked out a method of calculating this screening effect which are known as "Slater's Rules".

Electrons are grouped together in increasing order of

Each group has its own shielding constant. This depends on the sum of these contributions:

**1.**

The number of electrons in the **same** group.

You might think that the 2 electrons in helium are not able to shield each other since they are the same distance from the nucleus using the Bohr model:

However if you look at the probability of finding an

Point C is referred to as "The Bohr Radius" but you can see that there is some probability of the electron being at points closer to the nucleus such as A and B.

This means that the

**2.**

The number and type of electrons in the preceding groups.

The total shielding constant is, therefore, the overall shielding effect from

For

0.35 for each other electron within the same group, except for

For

For

Now we can apply these rules to a 4p electron in selenium.

First, group the electrons as described above:

For a 4p electron there are 5 other electrons in the same group. This gives:

For the

For the [3s 3p] group we get

For the [2s 2p] group we get

For the [1s] group we get

This gives the total screening constant to be: