To determine the correct formula for strontium oxide, we need to consider the charges on the ions that make up the compound.
1. Identify the charge of strontium ion (Sr):
- Strontium (Sr) is an alkaline earth metal located in Group 2 of the periodic table.
- Elements in Group 2 typically lose two electrons to achieve a stable electron configuration.
- Therefore, a strontium ion (Sr) has a charge of +2, written as [tex]\( \text{Sr}^{2+} \)[/tex].
2. Identify the charge of the oxygen ion (O):
- Oxygen (O) is a non-metal located in Group 16 of the periodic table.
- Elements in Group 16 typically gain two electrons to achieve a stable electron configuration.
- Therefore, an oxygen ion (O) has a charge of -2, written as [tex]\( \text{O}^{2-} \)[/tex].
3. Balance the charges to form a neutral compound:
- A compound is electrically neutral, meaning the total positive charge must equal the total negative charge.
- The charge on one strontium ion ([tex]\( \text{Sr}^{2+} \)[/tex]) is +2.
- The charge on one oxygen ion ([tex]\( \text{O}^{2-} \)[/tex]) is -2.
- Since the charges are equal in magnitude but opposite in sign, they combine in a 1:1 ratio to balance each other.
4. Write the formula:
- Since one [tex]\( \text{Sr}^{2+} \)[/tex] ion combines with one [tex]\( \text{O}^{2-} \)[/tex] ion, the formula for strontium oxide is [tex]\( \text{SrO} \)[/tex].
Therefore, considering the step-by-step analysis:
The correct formula for strontium oxide is:
A. SrO
