🎯⭐ INTERACTIVE LESSON

Net Ionic Equations and Spectator Ions

Learn step-by-step with interactive practice!

← Back to Standard Lesson

Net Ionic Equations and Spectator Ions - Complete Interactive Lesson

Part 1: Molecular Equations

🧪 Molecular vs. Ionic Equations

Part 1 of 7 — Writing Full Molecular Equations

Topics in This Part

Section
⚖️ Full Molecular Equations
Example
Key Features
Phase Labels Review
🔋 Electrolytes and Dissociation

🔑 Key Concept: Mastering this material will strengthen your foundation for both the AP Chemistry exam and more advanced chemistry topics.

What You'll Master in Part 1

Understanding the core concepts covered in Part 1
Applying these ideas to solve practice problems
Building toward AP exam readiness for this topic

⚖️ Full Molecular Equations

A molecular equation (also called a formula equation) shows all reactants and products as complete, neutral formulas — just like the balanced equations you've written before.

Example

$\boxed{\text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) + \text{NaNO}_3(aq)}$

🔋 Electrolytes and Dissociation

To move beyond molecular equations, you must know which substances dissociate (break apart) into ions when dissolved.

Strong Electrolytes — Fully Dissociate

Category	Examples
Strong acids	HCl, HBr, HI, $HNO_{3}$ , $H_{2}SO_{4}$ ,

✍️ Writing Balanced Molecular Equations

Steps

Identify reactants and products (predict products using reaction type rules)
Write correct formulas for each compound (use charges to determine subscripts)
Balance the equation
Add phase labels — $(aq)$ for dissolved species, $(s)$ for precipitates, etc.

Problem: Write the balanced molecular equation for the reaction of silver nitrate with sodium chloride.

Solution:

Step 1: Reactants: $AgNO_{3}$ and NaCl (both in aqueous solution)

Molecular Equations Concept Quiz 🎯

Electrolyte Classification 🧮

Classify each substance as strong, weak, or non (electrolyte).

1) KBr dissolved in water

2) $CH_{3}COOH$ (acetic acid) in water

3) $C_{2}H_{5}OH$ (ethanol) in water

Fill in the Blanks — Molecular Equations 🔽

Exit Quiz — Molecular Equations ✅

Part 2: Complete Ionic Equations

🧪 Complete Ionic Equations

Part 2 of 7 — Breaking Strong Electrolytes into Ions

Topics in This Part

Section
✍️ Rules for Writing Complete Ionic Equations
What Gets Split into Ions?
The Six Strong Acids (memorize these!)
Strong Bases
📏 Solubility Rules

🔑 Key Concept: Mastering this material will strengthen your foundation for both the AP Chemistry exam and more advanced chemistry topics.

What You'll Master in Part 2

Understanding the core concepts covered in Part 2
Applying these ideas to solve practice problems
Building toward AP exam readiness for this topic

✍️ Rules for Writing Complete Ionic Equations

What Gets Split into Ions?

Only aqueous strong electrolytes are written as separated ions:

Split into ions	Keep as molecular formula
Soluble ionic compounds — $(aq)$

Part 3: Spectator Ions

🧪 Net Ionic Equations

Part 3 of 7 — Removing Spectator Ions

Topics in This Part

Section
⚛️ Spectator Ions
Example
Removing Spectators
Net Ionic Equation
📋 Steps to Write a Net Ionic Equation

🔑 Key Concept: Mastering this material will strengthen your foundation for both the AP Chemistry exam and more advanced chemistry topics.

What You'll Master in Part 3

Understanding the core concepts covered in Part 3
Applying these ideas to solve practice problems
Building toward AP exam readiness for this topic

⚛️ Spectator Ions

🔑 Key Concept: Spectator ions are ions that appear in the same form on both sides of the complete ionic equation. They don't participate in the actual reaction.

Example

Complete ionic equation:

${Ag}^{+} (a q) + \underset{}{{NO}_{3}^{-}(aq)}$

Part 4: Writing Net Ionic Equations

🧪 Precipitation Reactions

Part 4 of 7 — Using Solubility Rules to Predict Precipitates

Topics in This Part

Section
⚗️ Predicting Precipitation Reactions
Strategy: The Ion-Swap Method
Example: Mix $AgNO_{3}(aq)$ and NaCl(aq)
📌 Common Precipitates on the AP Exam
Net Ionic Patterns

🔑 Key Concept: Mastering this material will strengthen your foundation for both the AP Chemistry exam and more advanced chemistry topics.

Part 5: Solubility & Driving Forces

🧪 Acid-Base Net Ionic Equations

Part 5 of 7 — Strong and Weak Acid-Base Reactions

Topics in This Part

Section
🧪 Strong Acid + Strong Base
The Universal Net Ionic Equation
🧪 Weak Acid + Strong Base
Example: Acetic acid + Sodium hydroxide
🧪 Strong Acid + Weak Base

🔑 Key Concept: Mastering this material will strengthen your foundation for both the AP Chemistry exam and more advanced chemistry topics.

What You'll Master in Part 5

Understanding the core concepts covered in Part 5
Applying these ideas to solve practice problems
Building toward AP exam readiness for this topic

🧪 Strong Acid + Strong Base

The Universal Net Ionic Equation

When a strong acid reacts with a strong base:

Molecular: $HCl (a q) + NaOH (a q) \to NaCl (a q) + H_{2} O (l)$

Part 6: Problem-Solving Workshop

🧪 Problem-Solving Workshop

Part 6 of 7 — Writing Net Ionic Equations for Various Reaction Types

Practice Makes Perfect

This workshop features multi-step problems that mirror the AP Chemistry exam format. Each problem requires you to combine concepts from previous parts and show your work clearly.

🔑 Why this matters: The AP Chemistry exam rewards students who can apply concepts to unfamiliar problems — structured practice is the best preparation.

What You'll Master in Part 6

Working through complete multi-step problems from start to finish
Building problem-solving strategies you can apply on the AP exam
Identifying which concepts to apply and in what order

⚗️ Gas-Forming Reactions

Some double-replacement reactions produce an unstable compound that decomposes into a gas and water. These are important driving forces.

Common Gas-Forming Patterns

Unstable Product	Decomposes Into	Gas Produced
$H_{2}CO_{3}$

Part 7: Synthesis & AP Review

🧪 Synthesis & AP Review

Part 7 of 7 — AP-Style Net Ionic Equation Problems

Bringing It All Together

This comprehensive review connects every concept from Parts 1–6 with AP-style problems. The questions are designed to mirror what you'll see on the actual exam — multi-step, multi-concept, and requiring clear written explanations.

🔑 Why this matters: AP Chemistry exam questions rarely test one concept in isolation — success requires connecting ideas across topics.

What You'll Master in Part 7

Solving AP-style questions that integrate multiple concepts from this unit
Writing clear, concise explanations using proper chemistry terminology
Identifying and avoiding common AP exam traps and mistakes

⚛️ AP Exam Tips for Net Ionic Equations

What the AP Exam Expects

On the AP Chemistry exam, you may be asked to:

Write the balanced net ionic equation for a described reaction
Identify spectator ions
Predict whether a reaction occurs
Identify driving forces

Common AP Formats

Prompt Style	What They Want
"Write the net ionic equation for..."	Net ionic only — no molecular needed
"Equal volumes of 0.1 M solutions are mixed..."	Identify reaction, write net ionic
"Identify the spectator ions..."	Find ions unchanged on both sides

Feature	Description
Formulas	Written as complete neutral compounds
Phase labels	$(s)$ , $(l)$ , $(g)$ , $(aq)$ are included
Balanced	Atoms and charge are balanced
Simplest form	Easiest to read, but hides ionic details

Symbol	Meaning
$(s)$	Solid
$(l)$	Liquid (pure)
$(g)$	Gas
$(aq)$	Aqueous (dissolved in water)

💡 Tip: Phase labels are critical on the AP exam — they determine how each species is written in ionic equations.

$\boxed{\text{NaCl}(aq) \rightarrow \text{Na}^+(aq) + \text{Cl}^-(aq)}$

Weak Electrolytes — Partially Dissociate

Category	Examples
Weak acids	HF, $CH_{3}COOH$ , $H_{2}CO_{3}$
Weak bases	$NH_{3}$ , amines

These remain mostly as intact molecules in solution and are written in molecular form.

Non-Electrolytes — Do Not Dissociate

Category	Examples
Molecular compounds	Sugar $(C_{6}H_{12}O_{6})$ , ethanol
Water	$H_{2}O$

🔑 Key Concept: Only strong electrolytes in aqueous solution are written as separated ions. Solids, liquids, gases, weak electrolytes, and non-electrolytes stay as complete formulas.

Step 2: Products: The cations and anions swap partners → AgCl and $NaNO_{3}$

Step 3: Already balanced: $\text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) + \text{NaNO}_3(aq)$

Step 4: AgCl is insoluble (precipitate → solid), everything else is aqueous.

⚠️ Warning: Always check solubility to assign correct phase labels. A reaction may not occur if no precipitate, gas, or water forms!

The Six Strong Acids (memorize these!)

$\boxed{\text{HCl, HBr, HI, HNO}_3\text{, H}_2\text{SO}_4\text{, HClO}_4}$

💡 Tip: Memorize these six strong acids — everything else is weak. A common mnemonic: HCl, HBr, HI (the binary acids) + $HNO_{3}$ , $H_{2}SO_{4}$ , $HClO_{4}$ (the oxy-acids).

$\boxed{\text{LiOH, NaOH, KOH, Ca(OH)}_2\text{, Sr(OH)}_2\text{, Ba(OH)}_2}$

⚠️ Warning: Weak acids (HF, $CH_{3}COOH$ , $H_{2}CO_{3}$ , $H_{3}PO_{4}$ ) and weak bases $(NH_{3})$ are NOT split into ions — they stay as complete formulas. This is the #1 AP exam mistake!

📏 Solubility Rules

To determine if an ionic compound is $(aq)$ or $(s)$ , use the solubility rules:

Generally Soluble (aqueous)

Ion	Exception
$Na^{+}$ , $K^{+}$ , $NH_{4}^{+}$	No exceptions — always soluble
$NO_{3}^{-}$ (nitrate)	No exceptions
$CH_{3}COO^{-}$ (acetate)	No exceptions
$Cl^{-}$ , $Br^{-}$ , $I^{-}$
$SO_{4}^{2-}$	Except with $Ba^{2+}$ , $P^{}$ , ,

Generally Insoluble (solid precipitate)

Ion	Exception
$OH^{-}$	Except with Group 1 metals, $Ba^{2+}$ , $Sr^{2+}$ , (slightly)

🔑 Key Concept: If an ionic compound is soluble → label $(aq)$ → split into ions. If an ionic compound is insoluble → label $(s)$ → keep as formula.

🧪 Worked Example

Problem: Write the complete ionic equation for:

$\text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) + \text{NaNO}_3(aq)$

Solution:

Step 1: Identify what splits

Species	Type	Action
$AgNO_{3}(aq)$	Soluble salt	Split → $Ag^{+}$ +

Step 2: Write the complete ionic equation

$\boxed{\text{Ag}^+(aq) + \text{NO}_3^-(aq) + \text{Na}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s) + \text{Na}^+(aq) + \text{NO}_3^-(aq)}$

Step 3: Verify

Atoms balanced ✓
Charges balanced: $(+1) + (-1) + (+1) + (-1) = 0$ on left; $0 + (+ 1) + (- 1)$ on right ✓

Complete Ionic Equations Quiz 🎯

Solubility Predictions 🧮

For each ionic compound, type soluble or insoluble.

1) $PbCl_{2}$

2) $Na_{2}CO_{3}$

3) $Fe(OH)_{3}$

Complete Ionic Equation Practice 🔽

Exit Quiz — Complete Ionic Equations ✅

Ag^{+} (a q) + spectator NO_{3}^{-} (a q) + spectator Na^{+} (a q) + Cl^{-} (a q) \to AgCl (s) + spectator Na^{+} (a q) + spectator NO_{3}^{-} (a q)

$Na^{+}$ appears on both sides → spectator
$NO_{3}^{-}$ appears on both sides → spectator
$Ag^{+}$ reacts with $Cl^{-}$ to form AgCl(s) → NOT spectators

Cancel ions that appear identically on both sides:

$\text{Ag}^+(aq) + \cancel{\text{NO}_3^-(aq)} + \cancel{\text{Na}^+(aq)} + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s) + \cancel{\text{Na}^+(aq)} + \cancel{\text{NO}_3^-(aq)}$

$\boxed{\text{Ag}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s)}$

This is the simplest representation showing only what changes.

📋 Steps to Write a Net Ionic Equation

The Complete Process

Step	Action
1	Write the balanced molecular equation with phase labels
2	Split all aqueous strong electrolytes into ions → complete ionic equation
3	Identify and cancel spectator ions (same on both sides)
4	Write the remaining species → net ionic equation
5	Verify: atoms balanced and charge balanced

Driving Forces

A reaction occurs (and a net ionic equation exists) when at least one of these forms:

Driving Force	Example
Precipitate (insoluble solid)	AgCl(s), $BaSO_{4}(s)$
Water (from acid-base)	$H_{2}O(l)$
Gas	$CO_{2}(g)$ , $H_{2}S(g)$

🔑 Key Concept: If none of these forms, there is no reaction (NR) and all ions are spectators.

🧪 Worked Example: No Reaction

Problem: Mix NaCl(aq) and $KNO_{3}(aq)$ . Write the net ionic equation.

Solution:

Step 1 — Predict products: Swapping ions gives $NaNO_{3}$ and KCl.

Step 2 — Check solubility: $NaNO_{3}$ is soluble. KCl is soluble. No precipitate forms!

Step 3 — Complete ionic equation:

$\text{Na}^+(aq) + \text{Cl}^-(aq) + \text{K}^+(aq) + \text{NO}_3^-(aq) \rightarrow \text{Na}^+(aq) + \text{NO}_3^-(aq) + \text{K}^+(aq) + \text{Cl}^-(aq)$

Step 4: Every ion is a spectator! All ions appear identically on both sides.

Conclusion: No net ionic equation — no reaction (NR).

⚠️ Warning: Just because you can write a double-replacement equation doesn't mean a reaction occurs. You must have a driving force (precipitate, water, or gas).

Net Ionic Equations Concept Quiz 🎯

Identify Spectator Ions 🧮

For the reaction: $\text{CaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{CaCO}_3(s) + 2\text{NaCl}(aq)$

List the spectator ions (type the ion formula without charge, in alphabetical order separated by a comma — e.g., "Cl, Na"):

1) The two spectator ions are:

For the net ionic equation $\text{Ca}^{2+}(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{CaCO}_3(s)$ :

2) The sum of charges on the reactant side is:

3) The sum of charges on the product side is:

Net Ionic Equation Concepts 🔽

Exit Quiz — Net Ionic Equations ✅

What You'll Master in Part 4

Understanding the core concepts covered in Part 4
Applying these ideas to solve practice problems
Building toward AP exam readiness for this topic

⚗️ Predicting Precipitation Reactions

Strategy: The Ion-Swap Method

When two ionic compounds in solution are mixed:

List all ions present in solution
Swap partners — combine each cation with each new anion
Check solubility of each possible product
If any product is insoluble → precipitation occurs!

Example: Mix $AgNO_{3}(aq)$ and NaCl(aq)

Ions present: $Ag^{+}$ , $NO_{3}^{-}$ , $Na^{+}$ , $Cl^{-}$

Possible new combinations:

$Ag^{+}$ + $Cl^{-}$ → AgCl — Check: $Cl^{-}$ with is an exception → ✓

Result: AgCl precipitates!

$\boxed{\text{Ag}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s)}$

📌 Common Precipitates on the AP Exam

Precipitate	Formula	Color
Silver chloride	AgCl	White
Silver bromide	AgBr	Pale yellow
Silver iodide	AgI	Yellow
Lead(II) iodide	$PbI_{2}$	Bright yellow
Lead(II) chloride	$PbCl_{2}$	White
Barium sulfate	$BaSO_{4}$	White
Lead(II) sulfate	$PbSO_{4}$	White
Calcium carbonate	$CaCO_{3}$	White
Iron(III) hydroxide	$Fe(OH)_{3}$	Rust brown
Copper(II) hydroxide	$Cu(OH)_{2}$	Blue
Iron(II) sulfide	FeS	Black

Net Ionic Patterns

All precipitation reactions follow the same net ionic pattern:

$\boxed{\text{cation}(aq) + \text{anion}(aq) \rightarrow \text{insoluble salt}(s)}$

🔑 Key Concept: The spectator ions are always the "other" pair that forms a soluble compound.

🧪 Multi-Step Example

Problem: Mix $\text{FeCl}_3(aq) + 3\text{NaOH}(aq) \rightarrow$ ? Write the net ionic equation.

Solution:

Step 1: Identify ions

$Fe^{3+}$ , $Cl^{-}$ , $Na^{+}$ , $OH^{-}$

Step 2: Swap partners

$Fe^{3+}$ + $OH^{-}$ → $Fe(OH)_{3}$ — Solubility? insoluble with most metals →

Step 3: Molecular equation

$\text{FeCl}_3(aq) + 3\text{NaOH}(aq) \rightarrow \text{Fe(OH)}_3(s) + 3\text{NaCl}(aq)$

Step 4: Complete ionic equation

$\text{Fe}^{3+}(aq) + 3\text{Cl}^-(aq) + 3\text{Na}^+(aq) + 3\text{OH}^-(aq) \rightarrow \text{Fe(OH)}_3(s) + 3\text{Na}^+(aq) + 3\text{Cl}^-(aq)$

Cancel spectators: $\text{Fe}^{3+}(aq) + \cancel{3\text{Cl}^-(aq)} + \cancel{3\text{Na}^+(aq)} + 3\text{OH}^-(aq) \rightarrow \text{Fe(OH)}_3(s) + \cancel{3\text{Na}^+(aq)} + \cancel{3\text{Cl}^-(aq)}$

Step 5: Net ionic equation

$\boxed{\text{Fe}^{3+}(aq) + 3\text{OH}^-(aq) \rightarrow \text{Fe(OH)}_3(s)}$

Charge check: (+3) + 3(−1) = 0 on left; 0 on right ✓

Precipitation Reactions Quiz 🎯

Predict the Precipitate 🧮

For each pair of solutions mixed, write the formula of the precipitate that forms. If no reaction occurs, type NR.

1) $\text{CaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow$

2) $\text{KNO}_3(aq) + \text{NaBr}(aq) \rightarrow$

3) $\text{Cu(NO}_3)_2(aq) + 2\text{NaOH}(aq) \rightarrow$

Precipitation Concepts 🔽

Exit Quiz — Precipitation Reactions ✅

HCl (a q) + NaOH (a q) \to NaCl (a q) + H_{2} O (l)

Complete ionic: $\text{H}^+(aq) + \text{Cl}^-(aq) + \text{Na}^+(aq) + \text{OH}^-(aq) \rightarrow \text{Na}^+(aq) + \text{Cl}^-(aq) + \text{H}_2\text{O}(l)$

Cancel spectators: $\text{H}^+(aq) + \cancel{\text{Cl}^-(aq)} + \cancel{\text{Na}^+(aq)} + \text{OH}^-(aq) \rightarrow \cancel{\text{Na}^+(aq)} + \cancel{\text{Cl}^-(aq)} + \text{H}_2\text{O}(l)$

Net ionic: $\boxed{\text{H}^+(aq) + \text{OH}^-(aq) \rightarrow \text{H}_2\text{O}(l)}$

🔑 Key Concept: Every strong acid–strong base reaction has the same net ionic equation! The identity of the acid and base doesn't matter because the salt ions are always spectators.

Reaction	Same Net Ionic
HCl + NaOH	$H^{+}$ + $OH^{-}$ → $H_{2}O$
$HNO_{3}$ + KOH	$H^{+}$ + $OH^{-}$ →
$H_{2}SO_{4}$ + 2NaOH	$H^{+}$ + →
$HClO_{4}$ + $Ba(OH)_{2}$	+ →

🧪 Weak Acid + Strong Base

When a weak acid reacts with a strong base, the weak acid is NOT split into ions — it stays molecular.

Example: Acetic acid + Sodium hydroxide

Molecular: $\text{CH}_3\text{COOH}(aq) + \text{NaOH}(aq) \rightarrow \text{NaCH}_3\text{COO}(aq) + \text{H}_2\text{O}(l)$

Complete ionic: $\text{CH}_3\text{COOH}(aq) + \text{Na}^+(aq) + \text{OH}^-(aq) \rightarrow \text{Na}^+(aq) + \text{CH}_3\text{COO}^-(aq) + \text{H}_2\text{O}(l)$

Net ionic $(cancel Na^{+})$ : $\boxed{\text{CH}_3\text{COOH}(aq) + \text{OH}^-(aq) \rightarrow \text{CH}_3\text{COO}^-(aq) + \text{H}_2\text{O}(l)}$

⚠️ Warning: The weak acid doesn't fully dissociate, so it cannot be written as $H^{+}$ + anion. It must appear as the complete molecule. The net ionic equation is unique to each weak acid — a critical AP exam distinction!

🧪 Strong Acid + Weak Base

When a strong acid reacts with a weak base, the weak base stays molecular.

Example: HCl + Ammonia

Molecular: $\text{HCl}(aq) + \text{NH}_3(aq) \rightarrow \text{NH}_4\text{Cl}(aq)$

Complete ionic: $\text{H}^+(aq) + \text{Cl}^-(aq) + \text{NH}_3(aq) \rightarrow \text{NH}_4^+(aq) + \text{Cl}^-(aq)$

Net ionic $(cancel Cl^{-})$ : $\boxed{\text{H}^+(aq) + \text{NH}_3(aq) \rightarrow \text{NH}_4^+(aq)}$

Summary Table

Acid	Base	Net Ionic Form
Strong	Strong	$\text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O}$

Acid-Base Net Ionic Quiz 🎯

Acid-Base Classification 🧮

For each net ionic equation scenario, type strong-strong, weak-strong, or strong-weak.

1) HCl(aq) + NaOH(aq) → NaCl(aq) + $H_{2}O(l)$

2) HF(aq) + KOH(aq) → KF(aq) + $H_{2}O(l)$

3) $HClO_{4}(aq)$ + $NH_{3}(aq)$ →

Acid-Base Net Ionic Concepts 🔽

Exit Quiz — Acid-Base Net Ionic ✅

Example: Acid + Carbonate

$2\text{HCl}(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow 2\text{NaCl}(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g)$

Net ionic: $\boxed{2\text{H}^+(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{H}_2\text{O}(l) + \text{CO}_2(g)}$

💡 Tip: The fizzing you see when acid hits baking soda is $CO_{2}$ gas escaping!

🛠️ Systematic Problem-Solving Approach

The 5-Step Method

Step	Action	Example
1	Identify reaction type	Double replacement
2	Write balanced molecular equation	Include phase labels
3	Split aqueous strong electrolytes	Ions for soluble salts, strong acids/bases
4	Cancel spectator ions	Same ion on both sides
5	Verify net ionic equation	Atoms and charges balanced

🔑 Decision Tree for Splitting:

A solid, liquid, or gas? → Keep molecular

A weak electrolyte? → Keep molecular

An aqueous strong electrolyte? → Split into ions

⚠️ Common AP Mistakes:

Splitting a precipitate into ions (NO — it's a solid!)

Splitting a weak acid like HF or $CH_{3}COOH$ (NO — weak electrolyte!)

Forgetting to balance the molecular equation first

Not checking charge balance in the net ionic equation

Mixed Practice Quiz 🎯

Write the Products 🧮

Identify the precipitate or gas formed. Type the chemical formula (no phase labels).

1) What precipitate forms when $Pb(NO_{3})_{2}(aq)$ is mixed with KI(aq)?

2) What gas is produced when HCl(aq) reacts with $NaHCO_{3}(aq)$ ?

3) What precipitate forms when $CuSO_{4}(aq)$ is mixed with NaOH(aq)?

Reaction Classification 🔽

Challenge Problems 🏆

Exit Quiz — Problem-Solving Workshop ✅

💡 AP Scoring Tips:

Correct formulas — wrong formula = wrong answer

Correct charges — always include charges on ions

Correct phases — $(s)$ , $(l)$ , $(g)$ , $(aq)$ matter

Balanced — both atoms and charges must balance

Lowest whole-number coefficients — simplify the equation

🔄 Complete Review: Types of Net Ionic Equations

Summary of All Patterns

Reaction Type	Driving Force	Net Ionic Pattern
Precipitation	Insoluble solid	Cation + Anion → Solid
Strong acid + Strong base	Water	$H^{+}$ + $OH^{-}$ → $H_{2}O$
Weak acid + Strong base	Water	HA + $OH^{-}$ → $A^{-}$ + $H_{2}O$
Strong acid + Weak base	Proton transfer	$H^{+}$ + B → $BH^{+}$
Acid + Carbonate	Gas + Water	$2H^{+}$ + $CO_{3}^{2-}$ → $H_{2}$ +
Acid + Bicarbonate	Gas + Water	$H^{+}$ + $HCO_{3}^{-}$ → $H_{2} O$ +
Acid + Sulfide	Gas	$2H^{+}$ + $S^{2-}$ → $H_{2}S(g)$

🔑 Quick Solubility Rules:

Always soluble: $Na^{+}$ , $K^{+}$ , $NH_{4}^{+}$ ,

AP-Style Questions — Set 1 🎯

AP-Style Free Response Practice 🧮

For each scenario, identify the precipitate formed (write formula) or type NR if no reaction occurs.

1) Solutions of iron(III) nitrate and sodium hydroxide are mixed.

2) Solutions of ammonium chloride and potassium nitrate are mixed.

3) Solutions of lead(II) nitrate and sodium sulfate are mixed.

AP Concept Review 🔽

AP-Style Questions — Set 2 🏆

Final Exit Quiz — Net Ionic Equations Mastery ✅

0 + (+ 1) + (- 1) = 0

Na^{+}

NO_{3}^{-}

→

NaNO_{3}

— Check:

Na^{+}

always soluble → soluble

Na^{+}

Cl^{-}

→ NaCl — Solubility?

Na^{+}

always soluble → soluble

CH3COOH(aq)+OH−(aq)→CH3COO−(aq)+H2O(l)

H+(aq)+NH3(aq)→NH4+(aq)

Usually soluble:

Cl^{-}

Br^{-}

I^{-}

(except

Ag^{+}

Pb^{2+}

Hg_{2}^{2+}

)

Usually soluble:

SO_{4}^{2-}

(except

Ba^{2+}

Pb^{2+}

Ca^{2+}

Sr^{2+}

)

Usually insoluble:

OH^{-}

S^{2-}

CO_{3}^{2-}

PO_{4}^{3-}

(except Group 1,

NH_{4}^{+}

)

Net Ionic Equations and Spectator Ions

Net Ionic Equations and Spectator Ions - Complete Interactive Lesson

Part 1: Molecular Equations

🧪 Molecular vs. Ionic Equations

Topics in This Part

What You'll Master in Part 1

⚖️ Full Molecular Equations

Example

🔋 Electrolytes and Dissociation

Strong Electrolytes — Fully Dissociate

✍️ Writing Balanced Molecular Equations

Steps

Part 2: Complete Ionic Equations

🧪 Complete Ionic Equations

Topics in This Part

What You'll Master in Part 2

✍️ Rules for Writing Complete Ionic Equations

What Gets Split into Ions?

Part 3: Spectator Ions

🧪 Net Ionic Equations

Topics in This Part

What You'll Master in Part 3

⚛️ Spectator Ions

Example

Part 4: Writing Net Ionic Equations

🧪 Precipitation Reactions

Topics in This Part

Part 5: Solubility & Driving Forces

🧪 Acid-Base Net Ionic Equations

Topics in This Part

What You'll Master in Part 5

🧪 Strong Acid + Strong Base

The Universal Net Ionic Equation

Part 6: Problem-Solving Workshop

🧪 Problem-Solving Workshop

Practice Makes Perfect

What You'll Master in Part 6

⚗️ Gas-Forming Reactions

Common Gas-Forming Patterns

Part 7: Synthesis & AP Review

🧪 Synthesis & AP Review

Bringing It All Together

What You'll Master in Part 7

⚛️ AP Exam Tips for Net Ionic Equations

What the AP Exam Expects

Common AP Formats

Key Features

Phase Labels Review

Weak Electrolytes — Partially Dissociate

Non-Electrolytes — Do Not Dissociate

The Six Strong Acids (memorize these!)

Strong Bases

📏 Solubility Rules

Generally Soluble (aqueous)

Generally Insoluble (solid precipitate)

🧪 Worked Example

Step 1: Identify what splits

Step 2: Write the complete ionic equation

Step 3: Verify

Removing Spectators

Net Ionic Equation

📋 Steps to Write a Net Ionic Equation

The Complete Process

Driving Forces

🧪 Worked Example: No Reaction

What You'll Master in Part 4

⚗️ Predicting Precipitation Reactions

Strategy: The Ion-Swap Method

Example: Mix AgNO3(aq)AgNO_{3}(aq)AgNO3​(aq) and NaCl(aq)

📌 Common Precipitates on the AP Exam

Net Ionic Patterns

🧪 Multi-Step Example

Step 1: Identify ions

Step 2: Swap partners

Step 3: Molecular equation

Step 4: Complete ionic equation

Step 5: Net ionic equation

🧪 Weak Acid + Strong Base

Example: Acetic acid + Sodium hydroxide

🧪 Strong Acid + Weak Base

Example: Mix $AgNO_{3}(aq)$ and NaCl(aq)