Naming Ionic Compounds Practice Worksheet - Solutions - Free Printable

Task: Naming Ionic Compounds and Writing Formulas

The worksheet provided involves two main sections:
1. Naming Ionic Compounds: Converting chemical formulas into their corresponding names.
2. Writing Formulas for Ionic Compounds: Converting compound names into their corresponding chemical formulas.

Below is the step-by-step solution for each part:

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Section 1: Naming Ionic Compounds

#### Rules for Naming Ionic Compounds:
- Metal + Nonmetal: The metal is named first, followed by the nonmetal with an "-ide" ending.
- Polyatomic Ions: Use the name of the polyatomic ion (e.g., nitrate, sulfate).
- Roman Numerals: Used for transition metals that can have multiple oxidation states.
- Acids: If the compound contains hydrogen and a polyatomic ion, it may be an acid.

#### Solutions:

1. NH₄Cl
- NH₄⁺ is ammonium.
- Cl⁻ is chloride.
- Name: Ammonium chloride.

2. Fe(NO₃)₃
- Fe³⁺ is iron(III) (since there are three nitrate ions, indicating a +3 charge on iron).
- NO₃⁻ is nitrate.
- Name: Iron(III) nitrate.

3. TiBr₄
- Ti⁴⁺ is titanium.
- Br⁻ is bromide.
- Name: Titanium(IV) bromide.

4. Cu₂P
- Cu²⁺ is copper.
- P³⁻ is phosphide.
- Since copper has a variable oxidation state, we use Roman numerals to specify Cu²⁺.
- Name: Copper(II) phosphide.

5. SnSe₂
- Sn²⁺ is tin.
- Se²⁻ is selenide.
- Tin has a +2 charge here.
- Name: Tin(II) selenide.

6. GaAs
- Ga³⁺ is gallium.
- As³⁻ is arsenide.
- Gallium has a +3 charge.
- Name: Gallium arsenide.

7. Pt(SO₄)₂
- Pt²⁺ is platinum.
- SO₄²⁻ is sulfate.
- Platinum has a +2 charge.
- Name: Platinum(II) sulfate.

8. Be(HCO₃)₂
- Be²⁺ is beryllium.
- HCO₃⁻ is bicarbonate (hydrogen carbonate).
- Beryllium has a +2 charge.
- Name: Beryllium bicarbonate.

9. Mn₂(SO₃)₃
- Mn²⁺ or Mn³⁺ is manganese.
- SO₃²⁻ is sulfite.
- To balance charges, Mn must have a +3 charge (since 2 × +3 = +6, which balances 3 × -2 from sulfite).
- Name: Manganese(III) sulfite.

10. Al(CN)₃
- Al³⁺ is aluminum.
- CN⁻ is cyanide.
- Aluminum has a +3 charge.
- Name: Aluminum cyanide.

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Section 2: Writing Formulas for Ionic Compounds

#### Rules for Writing Formulas:
- Charges Balance: The total positive charge must equal the total negative charge.
- Polyatomic Ions: Keep the polyatomic ion as a group (e.g., NO₃⁻, SO₄²⁻).
- Roman Numerals: Indicate the charge of transition metals using Roman numerals.

#### Solutions:

11. Chromium (VI) phosphate
- Chromium(VI) means Cr⁶⁺.
- Phosphate is PO₄³⁻.
- To balance charges: 2 × +6 = 12, and 3 × -4 = -12.
- Formula: Cr₂(PO₄)₃.

12. Vanadium (IV) carbonate
- Vanadium(IV) means V⁴⁺.
- Carbonate is CO₃²⁻.
- To balance charges: 2 × +4 = 8, and 2 × -2 = -4.
- Formula: V₂(CO₃)₂ or V₂CO₃.

13. Tin (II) nitrite
- Tin(II) means Sn²⁺.
- Nitrite is NO₂⁻.
- To balance charges: 1 × +2 = 2, and 1 × -2 = -2.
- Formula: Sn(NO₂)₂.

14. Cobalt (III) oxide
- Cobalt(III) means Co³⁺.
- Oxide is O²⁻.
- To balance charges: 2 × +3 = 6, and 3 × -2 = -6.
- Formula: Co₂O₃.

15. Titanium (II) acetate
- Titanium(II) means Ti²⁺.
- Acetate is CH₃COO⁻.
- To balance charges: 1 × +2 = 2, and 2 × -1 = -2.
- Formula: Ti(CH₃COO)₂.

16. Vanadium (V) sulfide
- Vanadium(V) means V⁵⁺.
- Sulfide is S²⁻.
- To balance charges: 2 × +5 = 10, and 5 × -2 = -10.
- Formula: V₂S₅.

17. Chromium (III) hydroxide
- Chromium(III) means Cr³⁺.
- Hydroxide is OH⁻.
- To balance charges: 1 × +3 = 3, and 3 × -1 = -3.
- Formula: Cr(OH)₃.

18. Lithium iodide
- Lithium is Li⁺.
- Iodide is I⁻.
- Charges already balance: 1 × +1 = 1, and 1 × -1 = -1.
- Formula: LiI.

19. Lead (II) nitride
- Lead(II) means Pb²⁺.
- Nitride is N³⁻.
- To balance charges: 3 × +2 = 6, and 2 × -3 = -6.
- Formula: Pb₃N₂.

20. Silver bromide
- Silver is Ag⁺.
- Bromide is Br⁻.
- Charges already balance: 1 × +1 = 1, and 1 × -1 = -1.
- Formula: AgBr.

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Final Answers:

#### Section 1: Naming Ionic Compounds
1. Ammonium chloride
2. Iron(III) nitrate
3. Titanium(IV) bromide
4. Copper(II) phosphide
5. Tin(II) selenide
6. Gallium arsenide
7. Platinum(II) sulfate
8. Beryllium bicarbonate
9. Manganese(III) sulfite
10. Aluminum cyanide

#### Section 2: Writing Formulas for Ionic Compounds
11. Cr₂(PO₄)₃
12. V₂(CO₃)₂
13. Sn(NO₂)₂
14. Co₂O₃
15. Ti(CH₃COO)₂
16. V₂S₅
17. Cr(OH)₃
18. LiI
19. Pb₃N₂
20. AgBr

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Boxed Final Answer:

\[
\boxed{
\begin{array}{ll}
\text{1.} & \text{Ammonium chloride} \\
\text{2.} & \text{Iron(III) nitrate} \\
\text{3.} & \text{Titanium(IV) bromide} \\
\text{4.} & \text{Copper(II) phosphide} \\
\text{5.} & \text{Tin(II) selenide} \\
\text{6.} & \text{Gallium arsenide} \\
\text{7.} & \text{Platinum(II) sulfate} \\
\text{8.} & \text{Beryllium bicarbonate} \\
\text{9.} & \text{Manganese(III) sulfite} \\
\text{10.} & \text{Aluminum cyanide} \\
\hline
\text{11.} & \text{Cr}_2(\text{PO}_4)_3 \\
\text{12.} & \text{V}_2(\text{CO}_3)_2 \\
\text{13.} & \text{Sn(NO}_2)_2 \\
\text{14.} & \text{Co}_2\text{O}_3 \\
\text{15.} & \text{Ti}(\text{CH}_3\text{COO})_2 \\
\text{16.} & \text{V}_2\text{S}_5 \\
\text{17.} & \text{Cr}(\text{OH})_3 \\
\text{18.} & \text{LiI} \\
\text{19.} & \text{Pb}_3\text{N}_2 \\
\text{20.} & \text{AgBr} \\
\end{array}
}
\]