1. Electronic Configuration of Bromine (Br)
* Bromine has an atomic number of 35, meaning it has 35 protons and 35 electrons in its neutral state.
* Its electronic configuration is: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵
2. Formation of the Bromide Ion (Br⁻)
* Bromine gains one electron to achieve a stable octet (8 electrons) in its outermost shell.
* The added electron goes into the 4p subshell.
3. Electronic Configuration of Bromide Ion (Br⁻)
* The electronic configuration of Br⁻ becomes: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶
4. Number of Electrons in the Second Shell
* The second shell consists of the 2s and 2p subshells.
* The bromide ion has 8 electrons in the second shell (2s² 2p⁶).
Therefore, there are 8 electrons in the second shell of the bromide ion (Br⁻).
