Step 1: Identify oxidation state changes Mg: +0 → +2 (oxidation, loses 2 electrons per atom) Ag: +1 → +0 (reduction, gains 1 electron per atom)
Step 2: Calculate electron transfer per compound Mg contains 1 Mg atom, each losing 2 electrons = 2 electrons lost per Mg AgNO3 contains 1 Ag atom, each gaining 1 electron = 1 electrons gained per AgNO3
Step 4: Balance electrons to determine coefficients Electrons lost per Mg: 2 Electrons gained per AgNO3: 1 The least common multiple of 2 and 1 = 2 Coefficient for Mg: 2 ÷ 2 = 1 Coefficient for AgNO3: 2 ÷ 1 = 2 Total electrons transferred: 2
Step 5: Complete mass balance Other coefficients are determined by: • Atom conservation (mass balance) • Charge neutrality • Stoichiometric relationships
Step 7: Verify balance ✓ Atoms are balanced ✓ Electrons transferred are equal ✓ Charge is conserved
Instructions for redox reaction analysis:
Enter an equation of a chemical reaction and click 'Analyze'. The answer will appear below
Always use the upper case for the first character in the element name and the lower case for the second character. Examples: Fe, Au, Co, Br, C, O, N, F. Compare: Co - cobalt and CO - carbon monoxide
To enter an electron into a chemical equation use {-} or e
To enter an ion, specify charge after the compound in curly brackets: {+3} or {3+} or {3}. Example: Fe{3+} + I{-} = Fe{2+} + I2
What are redox reactions?
Redox (reduction-oxidation) reactions are chemical reactions in which atoms have their oxidation states changed. These reactions involve the transfer of electrons between chemical species.
Key concepts:
Oxidation: Loss of electrons, increase in oxidation state
Reduction: Gain of electrons, decrease in oxidation state
Oxidizing agent: Species that causes oxidation (gets reduced itself)
Reducing agent: Species that causes reduction (gets oxidized itself)
Example: CuCl2 + Al → Cu + AlCl3
Let's analyze this step by step:
Assign oxidation states: CuCl₂: Cu = +2, Cl = -1 Al: Al = 0 Cu: Cu = 0 AlCl₃: Al = +3, Cl = -1
