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Step 1:I'll solve this problem step by step, focusing on the Lewis structure for the K+ ion.
Step 2:: Understand the Potassium Ion
- Potassium (K) is an alkali metal in Group 1 of the periodic table - When it forms an ion, it loses one electron to become K+ - K+ is a positively charged ion (cation)
Step 3:: Electron Configuration Analysis
- Neutral potassium has the electron configuration: $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1}
- When it becomes K+, it loses the 4s^{1} electron - The resulting K+ ion has a complete electron shell
Step 4:: Lewis Structure Characteristics
- K+ is a monoatomic ion - It has no valence electrons remaining - There are no bonds to draw - The Lewis structure is simply the symbol K+
Final Answer
The correct Lewis structure for K+ is just the symbol K+ with no electrons or bonds drawn around it, representing a bare potassium cation with a complete electron configuration.
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