QQuestionChemistry
QuestionChemistry
What ion does Sulfur (S) form in an ionic compound? (Indicate the charge as + or - and specify the number.)
Explain why, using electronegativity and the octet rule in your answer.
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine Sulfur's Electron Configuration
Sulfur's atomic number is 16, with electron configuration $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{4}
Step 3:: Analyze Electron Valence Shell
- Sulfur has 6 valence electrons in its outer shell (3p orbital) - To achieve a stable octet (8 electrons), Sulfur needs 2 more electrons
Step 4:: Ionic Charge Determination
- To gain 2 electrons and complete its octet, Sulfur will form a $$2^{-}$$ ion
- This means Sulfur will become a sulfide ion (S^{2 -})
Step 5:: Electronegativity Explanation
- Gaining 2 electrons completes its $$3p$$ orbital, creating a stable noble gas electron configuration
- Sulfur is less electronegative than elements like oxygen - It tends to gain electrons to achieve a stable electron configuration
Final Answer
Sulfur forms the S^{2 -} (sulfide) ion in ionic compounds, with a 2^{-} charge.
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