Question

Write the net ionic equation for this reaction occurring in water: ammonium fluoride and magnesium chloride are mixed to form magnesium fluoride and ammonium chloride. 1. no reaction occurs. 2. 2 nh+ 4 + 2 cl− → 2 nh4cl 3. 2 f− + mg2+ → mgf2 4. 2 nh4f + 2 cl− → 2 f− + 2 nh4cl 5. 2 f− + mgcl2 → mgf2 + 2 cl−

Answer 1

The correct net ionic equation for the reaction of ammonium fluoride with magnesium chloride in water is 2 F− (aq) + Mg2+ (aq) → MgF2 (s), which represents the formation of solid magnesium fluoride, while the other ions remain as spectators.

Step-by-step explanation:

When mixing ammonium fluoride (NH4F) and magnesium chloride (MgCl2) to form magnesium fluoride (MgF2) and ammonium chloride (NH4Cl), the net ionic equation represents the formation of the solid precipitate if any. According to solubility rules, both ammonium (NH4+) and chloride (Cl−) ions are soluble in water, as are most compounds containing these ions. Magnesium fluoride, on the other hand, is poorly soluble in water and hence can form a precipitate under the right conditions.

Consulting the given information and options, the correct net ionic equation for this reaction occurring in water is option 3:
2 F− (aq) + Mg2+ (aq) → MgF2 (s)

This equation reflects that magnesium ions (Mg2+) and fluoride ions (F−) combine to form solid magnesium fluoride, which is the precipitate. The ammonium (NH4+) and chloride (Cl−) ions remain in the solution as spectator ions and do not appear in the net ionic equation.

Answer 2

Correct answer: 3.
`Mg^(2+)(aq) + 2 F^(-)(aq) --> MgF_(2)(s)`

The given chemical reaction is between ammonium fluoride and magnesium chloride to form magnesium fluoride and ammonium chloride.

The balanced chemical equation representing the reaction will be,

`2NH_(4)F (aq) + MgCl_(2)(aq) -->MgF_(2) (s) + 2NH_(4)Cl (aq)`

The complete ionic equation for the reaction: All the compounds soluble in water (aqueous) will split into ions,
`MgF_(2)` will not split into ions as it is insoluble in water.

`2 NH_(4)^(+)(aq) + 2 F^(-)(aq) + Mg^(2+)(aq) + 2 Cl^(-)(aq) --> MgF_(2)(s) + 2 NH_(4)^(+)(aq) + 2 Cl^(-)(aq)`

The net ionic equation will be:

`Mg^(2+)(aq) + 2 F^(-)(aq) --> MgF_(2)(s)`

Here the spectator ions are
`NH_(4)^(+) and Cl^(-)`