Complete the table below by writing the symbols for the cation and anion that mak ionic compound NaCI NH
CI Cr(NO
)
Mn(OH)
CrBr
Na
NH
Cr
Mn
Cr
cationanionCI
CI
OH
Br
The Correct Answer and Explanation is:
✅ Corrected Table:
| Ionic Compound | Cation | Anion |
|---|---|---|
| NaCl | Na⁺ | Cl⁻ |
| NH₄Cl | NH₄⁺ | Cl⁻ |
| Cr(NO₃)₆ | Cr⁶⁺ | NO₃⁻ |
| Mn(OH)₃ | Mn³⁺ | OH⁻ |
| CrBr₄ | Cr⁴⁺ | Br⁻ |
🔍 Explanation
In ionic compounds, the total positive charge from cations must balance the total negative charge from anions. To determine the ions in each compound, we break the formula into its constituent ions by analyzing their charges and stoichiometry.
- NaCl is a simple ionic compound. Sodium (Na) is an alkali metal that forms a +1 cation (Na⁺), and chloride (Cl) forms a -1 anion (Cl⁻). Since their charges are equal and opposite, the compound is neutral.
- NH₄Cl contains the polyatomic ion ammonium (NH₄⁺) and the chloride ion (Cl⁻). Ammonium is a common polyatomic cation with a +1 charge, balancing the -1 charge of chloride.
- Cr(NO₃)₆ contains six nitrate ions (NO₃⁻), each with a -1 charge. The total negative charge is -6. Therefore, the chromium ion must have a +6 charge to balance it, resulting in Cr⁶⁺.
- Mn(OH)₃ includes three hydroxide ions (OH⁻), each carrying a -1 charge. This gives a total of -3. To balance this, manganese must be in the +3 oxidation state, giving Mn³⁺.
- CrBr₄ has four bromide ions (Br⁻), each with a -1 charge, for a total of -4. Thus, chromium must be in the +4 state, making the cation Cr⁴⁺.
Understanding the charges and the ratios of the ions helps deduce the correct oxidation states of the metal cations. This skill is crucial in naming and forming ionic compounds, balancing reactions, and understanding compound properties in chemistry.
