Question

in chemistry, there are specific rules for writing the formulas of ionic compounds having a given name. one or more of these formulas are breaking the rules. select all the rule breakers. tap to select or deselect an option. select all the rule breakers. iron(ii) oxide feo₂ cobalt(ii) chloride cocl₂ titanium(iv) chloride ticl₄

Explanation:

Step1: Determine charge of iron(II)

Iron(II) has a charge of $Fe^{2 + }$, and oxide ion is $O^{2-}$. The correct formula for iron(II) oxide should balance the charges. Using the criss - cross method, the formula should be $FeO$, not $FeO_{2}$. So $FeO_{2}$ is a rule - breaker.

Step2: Determine charge of cobalt(II)

Cobalt(II) has a charge of $Co^{2+}$, and chloride ion is $Cl^{-}$. Using the criss - cross method to balance the charges, the formula $CoCl_{2}$ is correct as $1\times2$ (from $Co^{2+}$) and $2\times1$ (from $Cl^{-}$) balance each other. So $CoCl_{2}$ is not a rule - breaker.

Step3: Determine charge of titanium(IV)

Titanium(IV) has a charge of $Ti^{4+}$, and chloride ion is $Cl^{-}$. Using the criss - cross method, the formula $TiCl_{4}$ is correct as $1\times4$ (from $Ti^{4+}$) and $4\times1$ (from $Cl^{-}$) balance each other. So $TiCl_{4}$ is not a rule - breaker.

Answer:

iron(II) oxide ($FeO_{2}$)