To determine which element is most likely to form a strong ionic bond and take on electrons, we can look at the electronegativity values of the given elements.
- Electronegativity generally increases across a period from left to right and decreases down a group in the periodic table.
- Elements that are more electronegative can attract electrons more strongly.
- Helium (He): A noble gas with a complete electron shell, it does not form bonds in typical circumstances and does not take on electrons.
- Cesium (Cs): An alkali metal with low electronegativity, it is more likely to lose an electron than take on electrons, thus forming positive ions.
- Fluorine (F): A halogen and one of the most electronegative elements, it has a strong tendency to gain electrons to achieve a stable electron configuration, making it very likely to form ionic bonds by taking electrons from metals.
- Hydrogen (H): While it can gain an electron to form H⁻, its electronegativity is not as high as fluorine's.
Based on this analysis, C. fluorine (F) is the element most likely to form a strong ionic bond and take on electrons due to its high electronegativity.
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