To determine the electron configuration of bromine, first, we should know bromine's atomic number, which is 35. This means bromine has 35 electrons.
The electron configuration follows the Aufbau principle, filling the lowest energy orbitals first. Here is the step-by-step filling of orbitals for bromine:
1. 1s orbital: This can hold 2 electrons.
[tex]\[ 1s^2 \][/tex]
2. 2s orbital: This can hold 2 electrons.
[tex]\[ 2s^2 \][/tex]
3. 2p orbitals: These can hold 6 electrons.
[tex]\[ 2p^6 \][/tex]
4. 3s orbital: This can hold 2 electrons.
[tex]\[ 3s^2 \][/tex]
5. 3p orbitals: These can hold 6 electrons.
[tex]\[ 3p^6 \][/tex]
6. 4s orbital: This can hold 2 electrons.
[tex]\[ 4s^2 \][/tex]
7. 3d orbitals: These can hold 10 electrons.
[tex]\[ 3d^{10} \][/tex]
8. 4p orbitals: These will hold the remaining 7 electrons.
[tex]\[ 4p^5 \][/tex]
Adding all together, bromine's electron configuration is:
[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5 \][/tex]
Comparing this configuration to the options given, we can see that the correct electron configuration is:
[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5 \][/tex]
So, the correct option is:
[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5 \][/tex]
