Question

decide whether each pair of elements in the table below will form an ionic compound. if they will, write the empirical formula of the compound formed in the space provided.

Explanation:

Bromine and Sulfur

• Bromine (\(Br\)) and sulfur (\(S\)) are both non - metals. Ionic compounds are formed between metals and non - metals. So, they do not form an ionic compound.

Barium and Sulfur

• Barium (\(Ba\)) is a metal (Group 2) and sulfur (\(S\)) is a non - metal (Group 16). Barium loses 2 electrons to form \(Ba^{2+}\) and sulfur gains 2 electrons to form \(S^{2 -}\).
• Using the criss - cross method (the magnitude of the charge of one ion becomes the subscript of the other ion), the empirical formula is \(BaS\).

Iodine and Sodium

• Sodium (\(Na\)) is a metal (Group 1) and iodine (\(I\)) is a non - metal (Group 17). Sodium loses 1 electron to form \(Na^{+}\) and iodine gains 1 electron to form \(I^{-}\).
• Using the criss - cross method, the empirical formula is \(NaI\).

Sodium and Strontium

• Both sodium (\(Na\)) and strontium (\(Sr\)) are metals. Ionic compounds are formed between metals and non - metals. So, they do not form an ionic compound.

Answer:

element #1	element #2	Forms ionic compound?	empirical formula of ionic compound
barium	sulfur	yes	\(BaS\)
iodine	sodium	yes	\(NaI\)
sodium	strontium	no