Review: Naming Ionic Compounds - Free Printable

Here is the complete solution for the "Review: Naming Ionic Compounds" worksheet, with explanations for each answer.

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Part 1: Write the formulas of the following ionic compounds

To write the formula of an ionic compound, you must:
- Identify the ions and their charges.
- Use subscripts to make the total positive charge equal the total negative charge (net charge = 0).
- Use parentheses around polyatomic ions if more than one is needed.

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1) iron (II) arsenide

- Iron (II) = Fe²⁺
- Arsenide = As³⁻ (from arsenic, group 15; gains 3 electrons)
- To balance: 3 Fe²⁺ ions (total +6) and 2 As³⁻ ions (total -6)
- Formula: Fe₃As₂

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2) lead (II) sulfate

- Lead (II) = Pb²⁺
- Sulfate = SO₄²⁻ (polyatomic ion)
- Charges are equal and opposite → 1:1 ratio
- Formula: PbSO₄

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3) lead (IV) hydroxide

- Lead (IV) = Pb⁴⁺
- Hydroxide = OH⁻
- Need 4 OH⁻ to balance Pb⁴⁺ → use parentheses since OH is polyatomic
- Formula: Pb(OH)₄

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4) copper (II) acetate

- Copper (II) = Cu²⁺
- Acetate = C₂H₃O₂⁻ (or CH₃COO⁻)
- Need 2 acetate ions to balance Cu²⁺ → use parentheses
- Formula: Cu(C₂H₃O₂)₂

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5) beryllium chloride

- Beryllium = Be²⁺
- Chloride = Cl⁻
- Need 2 Cl⁻ to balance Be²⁺
- Formula: BeCl₂

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6) ammonium chromate

- Ammonium = NH₄⁺
- Chromate = CrO₄²⁻
- Need 2 NH₄⁺ to balance CrO₄²⁻ → use parentheses
- Formula: (NH₄)₂CrO₄

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7) silver oxide

- Silver = Ag⁺ (always +1 in compounds)
- Oxide = O²⁻
- Need 2 Ag⁺ to balance O²⁻
- Formula: Ag₂O

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8) potassium sulfide

- Potassium = K⁺
- Sulfide = S²⁻
- Need 2 K⁺ to balance S²⁻
- Formula: K₂S

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Part 2: Write the names of the following ionic compounds

To name ionic compounds:
- Name the cation first (metal or polyatomic ion), then the anion.
- If the metal can have multiple charges (transition metals, Pb, Sn), include Roman numerals to indicate charge.
- For polyatomic ions, use their standard names.

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9) KI

- K⁺ = potassium
- I⁻ = iodide
- Name: potassium iodide

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10) Mn₂(SO₄)₃

- Mn = manganese (transition metal → needs Roman numeral)
- SO₄²⁻ = sulfate
- Total negative charge: 3 × (-2) = -6
- Two Mn ions → each must be +3 to balance → Mn³⁺
- Name: manganese(III) sulfate

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11) SnBr₄

- Sn = tin (can have multiple charges → needs Roman numeral)
- Br⁻ = bromide
- Four Br⁻ = total -4 → Sn must be +4
- Name: tin(IV) bromide

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12) Mg₃P₂

- Mg²⁺ = magnesium
- P³⁻ = phosphide
- Magnesium has only one common charge (+2), so no Roman numeral needed.
- Name: magnesium phosphide

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13) NaF

- Na⁺ = sodium
- F⁻ = fluoride
- Sodium has only one charge → no Roman numeral.
- Name: sodium fluoride

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14) Sr(MnO₄)₂

- Sr²⁺ = strontium
- MnO₄⁻ = permanganate (polyatomic ion)
- Strontium has only one common charge → no Roman numeral.
- Name: strontium permanganate

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15) Cr(PO₄)₂

- Cr = chromium (transition metal → needs Roman numeral)
- PO₄³⁻ = phosphate
- Two PO₄³⁻ = total -6 → Cr must be +6 (since there’s only one Cr ion)
- Name: chromium(VI) phosphate

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16) Al₂Se₃

- Al³⁺ = aluminum
- Se²⁻ = selenide
- Aluminum has only one common charge → no Roman numeral.
- Name: aluminum selenide

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✔ Final Answer Key:

Formulas:
1) Fe₃As₂
2) PbSO₄
3) Pb(OH)₄
4) Cu(C₂H₃O₂)₂
5) BeCl₂
6) (NH₄)₂CrO₄
7) Ag₂O
8) K₂S

Names:
9) potassium iodide
10) manganese(III) sulfate
11) tin(IV) bromide
12) magnesium phosphide
13) sodium fluoride
14) strontium permanganate
15) chromium(VI) phosphate
16) aluminum selenide

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