Atomic DM

🟠 Iron Replaces Copper – A Single Displacement Reaction

Copper sulfate (CuSO₄) consists of Cu²⁺ and SO₄²⁻ ions. The attraction between these oppositely charged ions holds the compound together in solution. When an iron (Fe) nail is placed into copper sulfate solution, iron is more reactive than copper. Iron atoms lose electrons to form Fe²⁺ ions, while Cu²⁺ ions gain those electrons and are deposited as reddish-brown copper metal. The sulfate ion (SO₄²⁻) then associates with the newly formed Fe²⁺ ions, producing iron(II) sulfate (FeSO₄).
💡 Key Concept:
The sulfate ion does not “choose” iron over copper on its own. The reaction occurs because iron is more reactive than copper, so it displaces copper from the solution through an electron-transfer (redox) process.

🔴 ⚡ FARADAY’S FIRST LAW OF ELECTROLYSIS
Faraday’s First Law of Electrolysis states that the mass of a substance deposited or liberated at an electrode is directly proportional to the total electric charge passed through the electrolyte. In simple words, the greater the electric charge, the greater the amount of substance deposited.

🔴 📐 FORMULA

m = ZIt

Where:
🔹 m = Mass deposited
🔹 Z = Electrochemical equivalent
🔹 I = Electric current
🔹 t = Time

🔴 💡 KEY CONCEPT

⚡ More Electric Charge = More Substance deposited

🌊⚛️ Dual Nature of Matter – de Broglie Hypothesis

In 1924, Louis de Broglie proposed that every moving particle, such as an electron, exhibits both particle-like and wave-like behavior. This revolutionary idea introduced the concept of matter waves, with wavelength given by:

λ = h / p

where λ is the wavelength, h is Planck’s constant, and p is the momentum of the particle.

This concept laid the foundation for quantum mechanics and explained phenomena such as electron diffraction, proving that matter can behave like waves under suitable conditions.

⚛️ Bohr’s Model of the Atom

Bohr’s atomic model (1913) explains that electrons move around the nucleus in fixed energy levels (shells) without losing energy. Electrons absorb or emit specific amounts of energy when they jump between these levels, explaining the line spectrum of hydrogen. This model laid the foundation for modern atomic theory.