# Bromine orbital diagram

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In the bromine orbital diagram, the 1s subshell holds two electrons, the 2s subshell carries another pair, the 2p subshell encompasses six electrons, the 3s subshell contains two electrons, the 3p subshell carries six electrons, the 4s subshell holds two electrons, the 3d subshell carries ten electrons, and the 4p subshell accommodates five electrons, totaling thirty-five electrons.

To illustrate the bromine orbital diagram, begin by determining the number of electrons from the periodic table. Take note of the electron configuration for reference and follow the three fundamental rules: the Aufbau principle, Pauli exclusion principle, and Hund’s rule. This systematic approach ensures an accurate representation of bromine’s orbital arrangement.

Contents

## Steps

### Find electrons

The atomic number of bromine represents the total number of electrons of bromine. Since the atomic number of bromine is 35, the total electrons of bromine are 35.

### Write electron configuration

The electron configuration of bromine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5.

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

### 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 bromine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. Hence, draw the blank orbital diagram of bromine up to 4p 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:

4p5 indicates that the 4p subshell has 5 electrons. So draw five arrows in the 4p box showing five electrons as follows:

That’s it! This is the final orbital diagram of bromine as we have used all 35 electrons.