Predict the ion generally formed by strontium.

Question

BlackTom AI · Accepted Answer

The task asks us to predict the ion generally formed by strontium.
Option 1: 'Sr2+' — This is the correct choice. Strontium is in Group 2 (the alkaline earth metals) and tends to lose two electrons to achieve a stable noble-gas electron configuration, forming Sr2+. This mirrors the common 2+ oxidation state observed for Group 2 elements.
Option 2: 'Sr3+' — This is unlikely. Strontium would need to lose three electrons to reach a stable configuration, which is uncommon for Group 2 elements; there is no typical Sr3+ species under ordinary conditions.
Option 3: 'Sr+' — A single positive charge would correspond to losing only one electron, which is characteristic of Group 1 alkali metals, not strontium. Strontium’s chemistry does not favor Sr+ as a stable ion.
Option 4: 'Sr–' — This implies strontium gaining electrons to form a negative ion. Strontium is highly electropositive and forms cations rather than anions; Sr– would be counter to its typical oxidation behavior.
Overall, understanding periodic trends explains why Sr2+ is the standard oxidation state: the loss of two valence electrons yields a stable electron configuration, accompanied by a relatively low ionization energy compared to heavier or differently grouped elements, reinforcing the 2+ ionic state as the general form for strontium.

Predict the ion generally formed by strontium.

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