Question

decide whether each pair of elements in the table below will form an ionic compound. if space provided.
element #1 element #2 forms ionic compound? empirical formula of ionic compound
barium bromine yes no
sulfur fluorine yes no
strontium oxygen yes no
magnesium chlorine yes no

Explanation:

Step1: Recall ionic compound formation

Ionic compounds form between metals and non - metals.

Step2: Analyze barium and bromine

Barium is a metal and bromine is a non - metal. They form an ionic compound. Barium has a +2 charge ($Ba^{2 + }$) and bromine has a - 1 charge ($Br^{-}$), so the empirical formula is $BaBr_{2}$.

Step3: Analyze sulfur and fluorine

Both sulfur and fluorine are non - metals. They form a covalent compound, not an ionic one.

Step4: Analyze strontium and oxygen

Strontium is a metal and oxygen is a non - metal. They form an ionic compound. Strontium has a +2 charge ($Sr^{2+}$) and oxygen has a - 2 charge ($O^{2 - }$), so the empirical formula is $SrO$.

Step5: Analyze magnesium and chlorine

Magnesium is a metal and chlorine is a non - metal. They form an ionic compound. Magnesium has a +2 charge ($Mg^{2+}$) and chlorine has a - 1 charge ($Cl^{-}$), so the empirical formula is $MgCl_{2}$.

Answer:

element #1	element #2	Forms ionic compound?	empirical formula of ionic compound
sulfur	fluorine	no
strontium	oxygen	yes	$SrO$
magnesium	chlorine	yes	$MgCl_{2}$