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
- Strontium's electron configuration is $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2}
- It has 2 valence electrons in its outer shell
Step 4:: Determine typical ion formation
- Group 2 elements typically lose their 2 valence electrons to achieve a stable electron configuration - When strontium forms an ion, it loses 2 electrons
Step 5:: Calculate ion charge
- Losing 2 electrons results in a $$2^{+}$$ charge
- The ion is represented as Sr^{2 +}
Final Answer
The charge of a strontium ion in a compound is 2^{+}.
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