Answer
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Step 1:I'll solve this problem step by step:
Step 2:: Identify the element
- Strontium (Sr) is an alkaline earth metal located in Group 2 of the periodic table
Step 3:: Determine electron configuration
- Its electron configuration is $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2}
- Strontium's atomic number is 38
Step 4:: Determine ion formation
- Group 2 elements typically form ions by losing their two valence electrons - This means strontium will lose 2 electrons to achieve a stable electron configuration
Step 5:: Calculate the charge
- The ion will be represented as $$Sr^{2+}
- Losing 2 electrons results in a 2 + charge
Final Answer
Key Insight: Alkaline earth metals in Group 2 consistently form 2 + ions by losing their two outermost electrons to achieve a noble gas electron configuration.
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