Chemical Formula Worksheet: Write Cation-Anion Combos | PDF ... - Free Printable

To solve the problem of determining the chemical formulas for each cation-anion combination, we need to follow these steps:

1. Understand the charges of the ions:
- Cations (positively charged ions) and anions (negatively charged ions) combine in such a way that the total charge is neutral.
- The combining power (or oxidation state) of some elements is given in the problem:
- Silver: +1
- Zinc: +2

2. Use the periodic table or common ion charges:
- Common charges for some ions are as follows:
- Chloride (Cl⁻): -1
- Oxide (O²⁻): -2
- Iodide (I⁻): -1
- Hydride (H⁻): -1
- Sulfide (S²⁻): -2
- Nitride (N³⁻): -3
- Bromide (Br⁻): -1
- Fluoride (F⁻): -1
- Astatide (At⁻): -1
- Selenide (Se²⁻): -2
- Phosphide (P³⁻): -3

3. Balance the charges:
- Combine the cations and anions so that the total positive charge equals the total negative charge.

Solution for Set 1

| Anions | Chloride (Cl⁻) | Oxide (O²⁻) | Iodide (I⁻) | Hydride (H⁻) | Sulfide (S²⁻) | Nitride (N³⁻) |
|--------|-----------------|--------------|--------------|---------------|----------------|----------------|
| Sodium (Na⁺) | NaCl | Na₂O | NaI | NaH | Na₂S | NaN₃ |
| Potassium (K⁺) | KCl | K₂O | KI | KH | K₂S | KN₃ |
| Magnesium (Mg²⁺) | MgCl₂ | MgO | MgI₂ | MgH₂ | MgS | Mg₃N₂ |
| Calcium (Ca²⁺) | CaCl₂ | CaO | CaI₂ | CaH₂ | CaS | Ca₃N₂ |
| Copper(II) (Cu²⁺) | CuCl₂ | CuO | CuI₂ | CuH₂ | CuS | Cu₃N₂ |
| Iron(II) (Fe²⁺) | FeCl₂ | FeO | FeI₂ | FeH₂ | FeS | Fe₃N₂ |
| Iron(III) (Fe³⁺) | FeCl₃ | Fe₂O₃ | FeI₃ | FeH₃ | Fe₂S₃ | FeN |
| Silver (Ag⁺) | AgCl | Ag₂O | AgI | AgH | Ag₂S | Ag₃N |
| Zinc (Zn²⁺) | ZnCl₂ | ZnO | ZnI₂ | ZnH₂ | ZnS | Zn₃N₂ |
| Aluminum (Al³⁺) | AlCl₃ | Al₂O₃ | AlI₃ | AlH₃ | Al₂S₃ | AlN |

Explanation for Set 1:

- Sodium (Na⁺): Sodium has a +1 charge. To balance:
- Cl⁻ (-1): NaCl
- O²⁻ (-2): Na₂O (2 Na⁺ × +1 = +2; O²⁻ × -2 = -2)
- I⁻ (-1): NaI
- H⁻ (-1): NaH
- S²⁻ (-2): Na₂S
- N³⁻ (-3): NaN₃ (3 Na⁺ × +1 = +3; N³⁻ × -3 = -3)

- Magnesium (Mg²⁺): Magnesium has a +2 charge. To balance:
- Cl⁻ (-1): MgCl₂ (2 Mg²⁺ × +2 = +4; 2 Cl⁻ × -1 = -2)
- O²⁻ (-2): MgO
- I⁻ (-1): MgI₂
- H⁻ (-1): MgH₂
- S²⁻ (-2): MgS
- N³⁻ (-3): Mg₃N₂ (3 Mg²⁺ × +2 = +6; 2 N³⁻ × -3 = -6)

Solution for Set 2

| Anions | Bromide (Br⁻) | Oxide (O²⁻) | Fluoride (F⁻) | Astatide (At⁻) | Selenide (Se²⁻) | Phosphide (P³⁻) |
|--------|----------------|--------------|----------------|-----------------|------------------|-------------------|
| Lithium (Li⁺) | LiBr | Li₂O | LiF | LiAt | Li₂Se | Li₃P |
| Barium (Ba²⁺) | BaBr₂ | BaO | BaF₂ | BaAt₂ | BaSe | Ba₃P₂ |
| Cesium (Cs⁺) | CsBr | Cs₂O | CsF | CsAt | Cs₂Se | Cs₃P |
| Strontium (Sr²⁺) | SrBr₂ | SrO | SrF₂ | SrAt₂ | SrSe | Sr₃P₂ |
| Copper(I) (Cu⁺) | CuBr | Cu₂O | CuF | CuAt | Cu₂Se | Cu₃P |
| Copper(II) (Cu²⁺) | CuBr₂ | CuO | CuF₂ | CuAt₂ | CuSe | Cu₃P₂ |
| Lead(II) (Pb²⁺) | PbBr₂ | PbO | PbF₂ | PbAt₂ | PbSe | Pb₃P₂ |
| Lead(IV) (Pb⁴⁺) | PbBr₄ | PbO₂ | PbF₄ | PbAt₄ | PbSe₂ | PbP |
| Gallium (Ga³⁺) | GaBr₃ | Ga₂O₃ | GaF₃ | GaAt₃ | Ga₂Se₃ | GaP |
| Nickel(II) (Ni²⁺) | NiBr₂ | NiO | NiF₂ | NiAt₂ | NiSe | Ni₃P₂ |

Explanation for Set 2:

- Lithium (Li⁺): Lithium has a +1 charge. To balance:
- Br⁻ (-1): LiBr
- O²⁻ (-2): Li₂O
- F⁻ (-1): LiF
- At⁻ (-1): LiAt
- Se²⁻ (-2): Li₂Se
- P³⁻ (-3): Li₃P

- Barium (Ba²⁺): Barium has a +2 charge. To balance:
- Br⁻ (-1): BaBr₂
- O²⁻ (-2): BaO
- F⁻ (-1): BaF₂
- At⁻ (-1): BaAt₂
- Se²⁻ (-2): BaSe
- P³⁻ (-3): Ba₃P₂

Final Answer:

\boxed{
\begin{array}{c|c|c|c|c|c|c}
\text{Anions} & \text{Chloride (Cl⁻)} & \text{Oxide (O²⁻)} & \text{Iodide (I⁻)} & \text{Hydride (H⁻)} & \text{Sulfide (S²⁻)} & \text{Nitride (N³⁻)} \\
\hline
\text{Sodium (Na⁺)} & \text{NaCl} & \text{Na₂O} & \text{NaI} & \text{NaH} & \text{Na₂S} & \text{NaN₃} \\
\text{Potassium (K⁺)} & \text{KCl} & \text{K₂O} & \text{KI} & \text{KH} & \text{K₂S} & \text{KN₃} \\
\text{Magnesium (Mg²⁺)} & \text{MgCl₂} & \text{MgO} & \text{MgI₂} & \text{MgH₂} & \text{MgS} & \text{Mg₃N₂} \\
\text{Calcium (Ca²⁺)} & \text{CaCl₂} & \text{CaO} & \text{CaI₂} & \text{CaH₂} & \text{CaS} & \text{Ca₃N₂} \\
\text{Copper(II) (Cu²⁺)} & \text{CuCl₂} & \text{CuO} & \text{CuI₂} & \text{CuH₂} & \text{CuS} & \text{Cu₃N₂} \\
\text{Iron(II) (Fe²⁺)} & \text{FeCl₂} & \text{FeO} & \text{FeI₂} & \text{FeH₂} & \text{FeS} & \text{Fe₃N₂} \\
\text{Iron(III) (Fe³⁺)} & \text{FeCl₃} & \text{Fe₂O₃} & \text{FeI₃} & \text{FeH₃} & \text{Fe₂S₃} & \text{FeN} \\
\text{Silver (Ag⁺)} & \text{AgCl} & \text{Ag₂O} & \text{AgI} & \text{AgH} & \text{Ag₂S} & \text{Ag₃N} \\
\text{Zinc (Zn²⁺)} & \text{ZnCl₂} & \text{ZnO} & \text{ZnI₂} & \text{ZnH₂} & \text{ZnS} & \text{Zn₃N₂} \\
\text{Aluminum (Al³⁺)} & \text{AlCl₃} & \text{Al₂O₃} & \text{AlI₃} & \text{AlH₃} & \text{Al₂S₃} & \text{AlN} \\
\end{array}
}
\boxed{
\begin{array}{c|c|c|c|c|c|c}
\text{Anions} & \text{Bromide (Br⁻)} & \text{Oxide (O²⁻)} & \text{Fluoride (F⁻)} & \text{Astatide (At⁻)} & \text{Selenide (Se²⁻)} & \text{Phosphide (P³⁻)} \\
\hline
\text{Lithium (Li⁺)} & \text{LiBr} & \text{Li₂O} & \text{LiF} & \text{LiAt} & \text{Li₂Se} & \text{Li₃P} \\
\text{Barium (Ba²⁺)} & \text{BaBr₂} & \text{BaO} & \text{BaF₂} & \text{BaAt₂} & \text{BaSe} & \text{Ba₃P₂} \\
\text{Cesium (Cs⁺)} & \text{CsBr} & \text{Cs₂O} & \text{CsF} & \text{CsAt} & \text{Cs₂Se} & \text{Cs₃P} \\
\text{Strontium (Sr²⁺)} & \text{SrBr₂} & \text{SrO} & \text{SrF₂} & \text{SrAt₂} & \text{SrSe} & \text{Sr₃P₂} \\
\text{Copper(I) (Cu⁺)} & \text{CuBr} & \text{Cu₂O} & \text{CuF} & \text{CuAt} & \text{Cu₂Se} & \text{Cu₃P} \\
\text{Copper(II) (Cu²⁺)} & \text{CuBr₂} & \text{CuO} & \text{CuF₂} & \text{CuAt₂} & \text{CuSe} & \text{Cu₃P₂} \\
\text{Lead(II) (Pb²⁺)} & \text{PbBr₂} & \text{PbO} & \text{PbF₂} & \text{PbAt₂} & \text{PbSe} & \text{Pb₃P₂} \\
\text{Lead(IV) (Pb⁴⁺)} & \text{PbBr₄} & \text{PbO₂} & \text{PbF₄} & \text{PbAt₄} & \text{PbSe₂} & \text{PbP} \\
\text{Gallium (Ga³⁺)} & \text{GaBr₃} & \text{Ga₂O₃} & \text{GaF₃} & \text{GaAt₃} & \text{Ga₂Se₃} & \text{GaP} \\
\text{Nickel(II) (Ni²⁺)} & \text{NiBr₂} & \text{NiO} & \text{NiF₂} & \text{NiAt₂} & \text{NiSe} & \text{Ni₃P₂} \\
\end{array}
}