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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine Selenium's Position on the Periodic Table
- Selenium (Se) is located in Group 16 (also known as the chalcogen group) on the periodic table - It is in Period 4
Step 3:: Identify Selenium's Electron Configuration
- Its electron configuration is $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{4}
- Selenium's atomic number is 34
Step 4:: Determine Valence Electrons
- Selenium has 6 valence electrons in its outer shell (4p^{4} subshell) - To achieve a stable electron configuration, it typically needs to gain 2 electrons
Step 5:: Calculate Ion Charge
- When selenium gains 2 electrons, it becomes a stable $$Se^{2-}$$ ion
- This represents a charge of negative two
Final Answer
The charge on a selenium ion is 2 -.
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