# Platinum orbital diagram

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The orbital diagram of platinum shows that the 1s subshell has 2 electrons, the 2s subshell has 2 electrons, the 2p subshell has 6 electrons, the 3s subshell has 2 electrons, the 3p subshell has 6 electrons, the 4s subshell has 2 electrons, the 3d subshell has 10 electrons, the 4p subshell has 6 electrons, the 5s subshell has 2 electrons, the 4d subshell has 10 electrons, the 5p subshell has 6 electrons, the 6s subshell has 1 electron, the 4f subshell has 14 electrons, and the 5d subshell has 9 electrons.

Contents

## Steps

Here’s how you can draw the orbital diagram of platinum step by step.

#1 Find electrons of platinum
#2 Write electron configuration of platinum
#3 Draw orbital diagram of platinum

Let’s break down each step in detail.

### Find electrons

The atomic number of platinum represents the total number of electrons of platinum. Since the atomic number of platinum is 78, the total electrons of platinum are 78.

### Write electron configuration

The electron configuration of platinum is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1 4f14 5d9.

Now in the next step, start drawing the orbital diagram for platinum.

### Draw orbital diagram

Before drawing the orbital diagram, you should know the three general rules.

• Aufbau principle – electrons are first filled in lowest energy orbital and then in higher energy orbital
• Pauli exclusion principle – two electrons with the same spin can not occupy the same orbital
• Hund’s rule – each orbital should be first filled with one electron before being paired with a second electron

Also, you should know the number of orbitals in each subshell.

We can calculate the number of orbitals in each subshell using the formula: 2ℓ + 1

Where, ℓ = azimuthal quantum number of the subshell

For s subshell, ℓ = 0
For p subshell, ℓ = 1
For d subshell, ℓ = 2
For f subshell, ℓ = 3

So each s subshell has one orbital, each p subshell has three orbitals, each d subshell has five orbitals, and each f subshell has seven orbitals.

Now start to draw!

As mentioned above, the electron configuration of platinum is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1 4f14 5d9. Hence, draw the blank orbital diagram of platinum up to 5d subshell as follows:

In the above orbital diagram, the box represents an orbital. Each orbital has a capacity of two electrons. And the arrows (↑↓) are drawn inside the box to represent electrons.

Now 1s2 indicates that the 1s subshell has 2 electrons. So draw two arrows in the 1s box showing two electrons as follows:

2s2 indicates that the 2s subshell has 2 electrons. So draw two arrows in the 2s box showing two electrons as follows:

2p6 indicates that the 2p subshell has 6 electrons. So draw six arrows in the 2p box showing six electrons as follows:

3s2 indicates that the 3s subshell has 2 electrons. So draw two arrows in the 3s box showing two electrons as follows:

3p6 indicates that the 3p subshell has 6 electrons. So draw six arrows in the 3p box showing six electrons as follows:

4s2 indicates that the 4s subshell has 2 electrons. So draw two arrows in the 4s box showing two electrons as follows:

3d10 indicates that the 3d subshell has 10 electrons. So draw ten arrows in the 3d box showing ten electrons as follows:

4p6 indicates that the 4p subshell has 6 electrons. So draw six arrows in the 4p box showing six electrons as follows:

5s2 indicates that the 5s subshell has 2 electrons. So draw two arrows in the 5s box showing two electrons as follows:

4d10 indicates that the 4d subshell has 10 electrons. So draw ten arrows in the 4d box showing ten electrons as follows:

5p6 indicates that the 5p subshell has 6 electrons. So draw six arrows in the 5p box showing six electrons as follows:

6s1 indicates that the 6s subshell has 1 electron. So draw one arrow in the 6s box showing one electron as follows:

4f14 indicates that the 4f subshell has 14 electrons. So draw fourteen arrows in the 4f box showing fourteen electrons as follows:

5d9 indicates that the 5d subshell has 9 electrons. So draw nine arrows in the 5d box showing nine electrons as follows:

That’s it! This is the final orbital diagram of platinum as we have used all 78 electrons.

Question 1: Why does the 6s subshell have one electron (instead of two electrons), and the 5d subshell has nine electrons (instead of eight electrons)?

Answer: 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).

Question 2: What if the 6s subshell has zero electrons (instead of one electron), and the 5d subshell has ten electrons (instead of nine electrons)?

Answer: 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).