# Platinum Bohr model

In the platinum Bohr model, the nucleus comprises 78 protons and 117 neutrons. Surrounding this nucleus are six electron shells, accommodating a total of 78 electrons.

To draw the platinum Bohr model, represent the 78 protons, 117 neutrons, and 78 electrons. Begin by sketching the nucleus, and then draw the six electron shells. The first five shells should contain 2, 8, 18, 32, and 17 electrons, respectively, while the sixth shell holds the remaining 1 electron.

Contents

## Steps

### Write protons, neutrons, and electrons of platinum atom

Platinum has 78 protons, 117 neutrons, and 78 electrons.

### Draw nucleus of platinum atom

The nucleus of a platinum atom contains 78 protons and 117 neutrons. So draw the nucleus of platinum atom as follows:

Now in the next step, draw the 1st electron shell and start marking electrons.

### Draw 1st electron shell

Remember that we have a total of 78 electrons.

The 1st electron shell (containing s subshell) can hold up to a maximum of 2 electrons. So draw the 1st electron shell as follows:

In the above image, 1 represents the 1st electron shell that contains 1s subshell. And the green color represents the number of electrons in that subshell. This means that the 1st electron shell has a total of 2 electrons.

Since we have already used 2 electrons in the 1st electron shell, now we have 78 – 2 = 76 electrons left. So in the next step, we have to draw the 2nd electron shell.

### Draw 2nd electron shell

The 2nd electron shell (containing s subshell and p subshell) can hold up to a maximum of 8 electrons. So draw the 2nd electron shell as follows:

In the above image, 2 represents the 2nd electron shell that contains 2s and 2p subshells. And the green and orange color represents the number of electrons in that subshell. This means that the 2nd electron shell has a total of 8 electrons.

Now we have already used 10 electrons in 1st and 2nd electron shells, so we have 78 – 10 = 68 electrons left. So in the next step, we have to draw the 3rd electron shell.

### Draw 3rd electron shell

The 3rd electron shell (containing s subshell, p subshell, and d subshell) can hold up to a maximum of 18 electrons. So draw the 3rd electron shell as follows:

In the above image, 3 represents the 3rd electron shell that contains 3s, 3p, and 3d subshells. And the green, orange, and pink color represents the number of electrons in that subshell. This means that the 3rd electron shell has a total of 18 electrons.

Now we have already used 28 electrons in 1st, 2nd, and 3rd electron shells, so we have 78 – 28 = 50 electrons left. So in the next step, we have to draw the 4th electron shell.

### Draw 4th electron shell

The 4th electron shell (containing s subshell, p subshell, d subshell, and f subshell) can hold up to a maximum of 32 electrons. So draw the 4th electron shell as follows:

In the above image, 4 represents the 4th electron shell that contains 4s, 4p, 4d, and 4f subshells. And the green, orange, pink, and blue color represents the number of electrons in that subshell. This means that the 4th electron shell has a total of 32 electrons.

Now we have already used 60 electrons in 1st, 2nd, 3rd, and 4th electron shells, so we have 78 – 60 = 18 electrons left. So in the next step, we have to draw the 5th electron shell.

### Draw 5th electron shell

The 5th electron shell can hold up to a maximum of 50 electrons. So draw the 5th electron shell as follows:

In the above image, 5 represents the 5th electron shell that contains 5s, 5p, and 5d subshells. And the green, orange, and pink color represents the number of electrons in that subshell. This means that the 5th electron shell has a total of 17 electrons.

The 5th electron shell contains only 5s, 5p, and 5d subshells, and not a 5f subshell. This is because according to the aufbau principle, the 6s subshell is filled first and then 4f, 5d, 6p… and so on.

Now we have already used 77 electrons in 1st, 2nd, 3rd, 4th, and 5th electron shells, so we have 78 – 77 = 1 electron left. So in the next step, we have to draw the 6th electron shell.

Note 1: One partially filled 5d subshell is more stable than one empty 5d subshell. That’s why the 5d subshell has nine electrons (instead of eight electrons). And the 6s subshell has one electron (instead of two electrons).

Note 2: A partially filled 6s subshell is more stable than an empty 6s subshell. That’s why the 6s subshell has one electron (instead of zero electrons). And the 5d subshell has nine electrons (instead of ten electrons).

For a detailed explanation, check the orbital diagram of platinum.

### Draw 6th electron shell

The 6th electron shell can hold up to a maximum of 72 electrons. So draw the 6th electron shell as follows:

In the above image, 6 represents the 6th electron shell that contains 6s subshell. And the green color represents the number of electrons in that subshell. This means that the 6th electron shell has a total of 1 electron.

That’s it! This is the final Bohr model of platinum atom as we have used all 78 electrons: 2 electrons in the 1st electron shell, 8 electrons in the 2nd electron shell, 18 electrons in the 3rd electron shell, 32 electrons in the 4th electron shell, 17 electrons in the 5th electron shell, and 1 electron in the 6th electron shell.

Next: Gold Bohr model