Question

dissociation

• the process by which chemical compounds break apart to form separate ions.

reactions between ions
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spectator ions
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precipitate
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net ionic equations
three types of equations to represent reactions of aqueous solutions

1. complete balanced chemical equation

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1. ionic equation (more accurate representation)

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1. net ionic equation

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(remove spectator ions and re - write equation)
example: agno₃(aq) and na₂cro₄(aq)

Explanation:

1. Reactions Between Ions: Reactions where dissolved ionic compounds in aqueous solution react via their free ions, often forming a precipitate, gas, or weak electrolyte.
2. Spectator Ions: Ions present in solution that do not participate in the chemical reaction; they remain unchanged before and after the reaction.
3. Precipitate: A solid insoluble product formed from the reaction of dissolved ions in an aqueous solution.
4. Complete Balanced Chemical Equation: A chemical equation that shows all reactants and products in their neutral, undissociated molecular forms, with equal numbers of each atom on both sides.
5. Ionic Equation (more accurate representation): A chemical equation that shows all strong electrolytes as dissociated free ions in aqueous solution, while keeping weak electrolytes, solids, and gases in their molecular/undissolved forms.
6. Net Ionic Equation: A simplified ionic equation that excludes spectator ions, only showing the species that directly participate in forming the product (precipitate, gas, weak electrolyte).

Example (AgNO₃(aq) and Na₂CrO₄(aq)):

1. Complete Balanced Chemical Equation:

$$2\text{AgNO}_3(aq) + \text{Na}_2\text{CrO}_4(aq) ightarrow \text{Ag}_2\text{CrO}_4(s) + 2\text{NaNO}_3(aq)$$

1. Ionic Equation:

$$2\text{Ag}^+(aq) + 2\text{NO}_3^-(aq) + 2\text{Na}^+(aq) + \text{CrO}_4^{2-}(aq) ightarrow \text{Ag}_2\text{CrO}_4(s) + 2\text{Na}^+(aq) + 2\text{NO}_3^-(aq)$$

1. Net Ionic Equation:

$$2\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq) ightarrow \text{Ag}_2\text{CrO}_4(s)$$

Answer:

1. Reactions Between Ions: Reactions of dissolved ionic species in solution
2. Spectator Ions: Unchanged, non-participating ions in a reaction
3. Precipitate: Insoluble solid product of an ionic reaction
4. Complete Balanced Chemical Equation: Balanced equation with neutral molecular formulas
5. Ionic Equation (more accurate representation): Equation showing dissociated strong electrolytes as ions
6. Net Ionic Equation: Equation excluding spectator ions, showing only reacting species
7. Example (AgNO₃(aq) and Na₂CrO₄(aq)):

• Complete Balanced: $2\text{AgNO}_3(aq) + \text{Na}_2\text{CrO}_4(aq)

ightarrow \text{Ag}_2\text{CrO}_4(s) + 2\text{NaNO}_3(aq)$

• Ionic: $2\text{Ag}^+(aq) + 2\text{NO}_3^-(aq) + 2\text{Na}^+(aq) + \text{CrO}_4^{2-}(aq)

ightarrow \text{Ag}_2\text{CrO}_4(s) + 2\text{Na}^+(aq) + 2\text{NO}_3^-(aq)$

• Net Ionic: $2\text{Ag}^+(aq) + \text{CrO}_4^{2-}(aq)

ightarrow \text{Ag}_2\text{CrO}_4(s)$