Write the formula for the following ionic compounds
9. Lead (IV) oxide
10. Sodium sulfate
11. Iron (II) sulfide
12. Magnesium carbonate
13. Potassium bromide

Write the names for the following compounds
14. $\mathrm{NaF}$
15. $\mathrm{Be}(\mathrm{OH})_{2}$
16. $\mathrm{FeCO}_{3}$
17. $\mathrm{Ni}(\mathrm{CN})_{2}$
18. $\mathrm{CuCl}_{2}$

Question

Write the formula for the following ionic compounds
9. Lead (IV) oxide
10. Sodium sulfate
11. Iron (II) sulfide
12. Magnesium carbonate
13. Potassium bromide

Write the names for the following compounds
14. $\mathrm{NaF}$
15. $\mathrm{Be}(\mathrm{OH})_{2}$
16. $\mathrm{FeCO}_{3}$
17. $\mathrm{Ni}(\mathrm{CN})_{2}$
18. $\mathrm{CuCl}_{2}$

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Identify the formula for Lead (IV) oxide**: Lead (IV) indicates a +4 oxidation state for lead. Oxygen typically has a -2 oxidation state. To balance the charges, we need two oxygen atoms for every lead atom. The formula is $PbO_2$. ‖ ‖ 2 ⋮ **Identify the formula for Sodium sulfate**: Sodium has a +1 charge, and sulfate ($SO_4$) has a -2 charge. To balance the charges, we need two sodium atoms for every sulfate ion. The formula is $Na_2SO_4$. ‖ ‖ 3 ⋮ **Identify the formula for Iron (II) sulfide**: Iron (II) indicates a +2 oxidation state for iron. Sulfide has a -2 charge. The charges are already balanced with one iron atom and one sulfide ion. The formula is $FeS$. ‖ ‖ 4 ⋮ **Identify the formula for Magnesium carbonate**: Magnesium has a +2 charge, and carbonate ($CO_3$) has a -2 charge. The charges are balanced with one magnesium atom and one carbonate ion. The formula is $MgCO_3$. ‖ ‖ 5 ⋮ **Identify the formula for Potassium bromide**: Potassium has a +1 charge, and bromide has a -1 charge. The charges are balanced with one potassium atom and one bromide ion. The formula is $KBr$. ‖ ‖ 6 ⋮ **Identify the name for $NaF$**: Sodium has a +1 charge, and fluoride has a -1 charge. The compound is named Sodium fluoride. ‖ ‖ 7 ⋮ **Identify the name for $Be(OH)_2$**: Beryllium has a +2 charge, and hydroxide has a -1 charge. The compound is named Beryllium hydroxide. ‖ ‖ 8 ⋮ **Identify the name for $FeCO_3$**: Iron (II) indicates a +2 oxidation state for iron, and carbonate has a -2 charge. The compound is named Iron (II) carbonate. ‖ ‖ 9 ⋮ **Identify the name for $Ni(CN)_2$**: Nickel (II) indicates a +2 oxidation state for nickel, and cyanide has a -1 charge. The compound is named Nickel (II) cyanide. ‖ ‖ 10 ⋮ **Identify the name for $CuCl_2$**: Copper (II) indicates a +2 oxidation state for copper, and chloride has a -1 charge. The compound is named Copper (II) chloride. ‖ ∻Answer∻ ⚹ - Lead (IV) oxide: $PbO_2$ - Sodium sulfate: $Na_2SO_4$ - Iron (II) sulfide: $FeS$ - Magnesium carbonate: $MgCO_3$ - Potassium bromide: $KBr$ - $NaF$: Sodium fluoride - $Be(OH)_2$: Beryllium hydroxide - $FeCO_3$: Iron (II) carbonate - $Ni(CN)_2$: Nickel (II) cyanide - $CuCl_2$: Copper (II) chloride ⚹ ∻Key Concept∻ ⚹ Ionic compounds are formed by the electrostatic attraction between cations and anions, and their formulas are determined by balancing the charges of the ions. ⚹ ∻Explanation∻ ⚹ The names and formulas of ionic compounds are derived from the charges of the ions involved. For example, Lead (IV) oxide is $PbO_2$ because lead has a +4 charge and oxygen has a -2 charge, requiring two oxygen atoms to balance one lead atom. ⚹◊What is the formula for Potassium bromide?⍭ Generate me a similar question◊

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