Question

complete the names of these compounds.
formula\tname
fecl₂\tiron
scl₂\tsulfur
cacl₂\tcalcium
answer bank
dichloride\tchloride
\t(ii) chloride

Explanation:

To solve this, we analyze each compound:

For $\boldsymbol{FeCl_2}$:

Iron (Fe) can have multiple oxidation states. In $FeCl_2$, Fe has a +2 oxidation state. When naming ionic compounds with transition metals (like Fe) with variable charges, we use Roman numerals to indicate the charge. So we use "(II) chloride" to show Fe is in the +2 state.

For $\boldsymbol{SCl_2}$:

Sulfur (S) and chlorine (Cl) form a covalent compound (since both are nonmetals). For covalent compounds, we use prefixes to indicate the number of atoms. The subscript 2 for Cl means we use the prefix "di-", so we name it "dichloride".

For $\boldsymbol{CaCl_2}$:

Calcium (Ca) is an alkaline earth metal with a fixed +2 oxidation state (no variable charge). For ionic compounds with fixed-charge metals, we simply use the anion name with the suffix "-ide". Chlorine becomes "chloride" (no prefix needed here, as Ca has a fixed charge and the formula is determined by charge balance: $Ca^{2+}$ and $Cl^-$ combine as $CaCl_2$).

Final Answers:

• $FeCl_2$: iron $\boldsymbol{(II)}$ chloride
• $SCl_2$: sulfur $\boldsymbol{dichloride}$
• $CaCl_2$: calcium $\boldsymbol{chloride}$

Answer:

To solve this, we analyze each compound:

For $\boldsymbol{FeCl_2}$:

Iron (Fe) can have multiple oxidation states. In $FeCl_2$, Fe has a +2 oxidation state. When naming ionic compounds with transition metals (like Fe) with variable charges, we use Roman numerals to indicate the charge. So we use "(II) chloride" to show Fe is in the +2 state.

For $\boldsymbol{SCl_2}$:

Sulfur (S) and chlorine (Cl) form a covalent compound (since both are nonmetals). For covalent compounds, we use prefixes to indicate the number of atoms. The subscript 2 for Cl means we use the prefix "di-", so we name it "dichloride".

For $\boldsymbol{CaCl_2}$:

Calcium (Ca) is an alkaline earth metal with a fixed +2 oxidation state (no variable charge). For ionic compounds with fixed-charge metals, we simply use the anion name with the suffix "-ide". Chlorine becomes "chloride" (no prefix needed here, as Ca has a fixed charge and the formula is determined by charge balance: $Ca^{2+}$ and $Cl^-$ combine as $CaCl_2$).

Final Answers:

• $FeCl_2$: iron $\boldsymbol{(II)}$ chloride
• $SCl_2$: sulfur $\boldsymbol{dichloride}$
• $CaCl_2$: calcium $\boldsymbol{chloride}$