Chart displaying the chemical formulas of ionic compounds formed by different cations and anions, including examples like NaCl, MgO, and Al₂O₃.

Problem Analysis:

The task involves understanding and completing a table of ionic compounds formed by combining cations (positively charged ions) and anions (negatively charged ions). The tables provided show how different cations react with various anions to form specific compounds. The goal is to ensure that the chemical formulas are correctly written based on the charges of the ions involved.

Key Concepts:

1. Ionic Compounds: Formed when a metal (cation) transfers electrons to a nonmetal (anion), resulting in a neutral compound.
2. Charge Balance: The total positive charge of the cations must equal the total negative charge of the anions in a compound.
3. Polyatomic Ions: Some anions, like oxide (\(O^{2-}\)), have multiple atoms but act as a single unit with a specific charge.
4. Variable Oxidation States: Some metals (e.g., iron, copper) can exist in multiple oxidation states, leading to different compounds.

Solution Approach:

We will verify the correctness of the given tables by ensuring that the chemical formulas are balanced according to the charges of the ions.

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#### Table 1: Anions - Chloride, Oxide, Iodide, Hydride

| Cations | Chloride (\(Cl^-\)) | Oxide (\(O^{2-}\)) | Iodide (\(I^-\)) | Hydride (\(H^-\)) |
|---------|---------------------|--------------------|-------------------|--------------------|
| Sodium (\(Na^+\)) | \(NaCl\) | \(Na_2O\) | \(NaI\) | \(NaH\) |
| Potassium (\(K^+\)) | \(KCl\) | \(K_2O\) | \(KI\) | \(KH\) |
| Magnesium (\(Mg^{2+}\)) | \(MgCl_2\) | \(MgO\) | \(MgI_2\) | \(MgH_2\) |
| Calcium (\(Ca^{2+}\)) | \(CaCl_2\) | \(CaO\) | \(CaI_2\) | \(CaH_2\) |
| Copper(II) (\(Cu^{2+}\)) | \(CuCl_2\) | \(CuO\) | \(CuI_2\) | \(CuH_2\) |
| Iron(II) (\(Fe^{2+}\)) | \(FeCl_2\) | \(FeO\) | \(FeI_2\) | \(FeH_2\) |
| Iron(III) (\(Fe^{3+}\)) | \(FeCl_3\) | \(Fe_2O_3\) | \(FeI_3\) | \(FeH_3\) |
| Silver (\(Ag^+\)) | \(AgCl\) | \(Ag_2O\) | \(AgI\) | \(AgH\) |
| Zinc (\(Zn^{2+}\)) | \(ZnCl_2\) | \(ZnO\) | \(ZnI_2\) | \(ZnH_2\) |
| Aluminum (\(Al^{3+}\)) | \(AlCl_3\) | \(Al_2O_3\) | \(AlI_3\) | \(AlH_3\) |

Verification:
- Chloride (\(Cl^-\)): Each cation combines with one or more chloride ions to balance the charge.
- For example, \(Mg^{2+}\) requires 2 \(Cl^-\) ions to balance: \(MgCl_2\).
- Oxide (\(O^{2-}\)): Each cation combines with one or more oxide ions.
- For example, \(Fe^{3+}\) requires \(\frac{3}{2}\) oxide ions, so the formula is \(Fe_2O_3\).
- Iodide (\(I^-\)): Similar to chloride, each cation combines with iodide ions to balance the charge.
- Hydride (\(H^-\)): Each cation combines with hydride ions to balance the charge.

All formulas in Table 1 are correct based on charge balancing.

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#### Table 2: Anions - Bromide, Oxide, Fluoride, Astatide

| Cations | Bromide (\(Br^-\)) | Oxide (\(O^{2-}\)) | Fluoride (\(F^-\)) | Astatide (\(At^-\)) |
|---------|---------------------|--------------------|---------------------|---------------------|
| Lithium (\(Li^+\)) | \(LiBr\) | \(Li_2O\) | \(LiF\) | \(LiAt\) |
| Barium (\(Ba^{2+}\)) | \(BaBr_2\) | \(BaO\) | \(BaF_2\) | \(BaAt_2\) |
| Cesium (\(Cs^+\)) | \(CsBr\) | \(Cs_2O\) | \(CsF\) | \(CsAt\) |
| Strontium (\(Sr^{2+}\)) | \(SrBr_2\) | \(SrO\) | \(SrF_2\) | \(SrAt_2\) |
| Copper(I) (\(Cu^+\)) | \(CuBr\) | \(Cu_2O\) | \(CuF\) | \(CuAt\) |
| Copper(II) (\(Cu^{2+}\)) | \(CuBr_2\) | \(CuO\) | \(CuF_2\) | \(CuAt_2\) |
| Lead(II) (\(Pb^{2+}\)) | \(PbBr_2\) | \(PbO\) | \(PbF_2\) | \(PbAt_2\) |
| Lead(IV) (\(Pb^{4+}\)) | \(PbBr_4\) | \(PbO_2\) | \(PbF_4\) | \(PbAt_4\) |
| Gallium (\(Ga^{3+}\)) | \(GaBr_3\) | \(Ga_2O_3\) | \(GaF_3\) | \(GaAt_3\) |
| Nickel(II) (\(Ni^{2+}\)) | \(NiBr_2\) | \(NiO\) | \(NiF_2\) | \(NiAt_2\) |

Verification:
- Bromide (\(Br^-\)): Each cation combines with bromide ions to balance the charge.
- For example, \(Pb^{4+}\) requires 4 \(Br^-\) ions: \(PbBr_4\).
- Oxide (\(O^{2-}\)): Each cation combines with oxide ions.
- For example, \(Ga^{3+}\) requires \(\frac{3}{2}\) oxide ions: \(Ga_2O_3\).
- Fluoride (\(F^-\)): Similar to bromide, each cation combines with fluoride ions.
- Astatide (\(At^-\)): Each cation combines with astatide ions to balance the charge.

All formulas in Table 2 are also correct based on charge balancing.

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Final Answer:

Both tables are correctly filled out. The chemical formulas are balanced according to the charges of the ions involved.

\[
\boxed{\text{Both tables are correct.}}
\]