1. Electron Clouds and Probability
Glencoe Chemistry: Matter and Change
Chapter 5 Section 2

2. De Broglie Hypothesis E = mc2 and E = hν E = Energy (joules) m = mass v (nu) = Frequency c = 3.00 x 108 m/s h = x joules/Hz Predicted the wavelength of a particle using: λ= ℎ 𝑚𝑣 λ= wavelength (meters) h = Planck’s constant m = mass (kg) v = velocity (m/s) not nu h/λm = v h/λv = m

3. Wave-particle duality of nature Light has the properties of both a particle as well as a wave. Newtonian Mechanics Momentum = mass x velocity P = m x v Visible objects at ordinary velocities.

4. Quantum mechanics Extremely small particles at velocities near the speed of light.

5. Heisenberg Uncertainty Principle ΔP Δx ≥ h ΔP = Uncertainty of momentum Δx = Uncertainty of position h = Planck’s constant ΔP Δx inversely proportional

6. 2𝜋2𝑚𝑒4 ℎ2𝑛2 m = mass of electron
Erwin Schrödinger
Treated the electron as a wave and developed a model that describes the behavior of the electron.
2𝜋2𝑚𝑒4 ℎ2𝑛2 m = mass of electron
e = charge of electron
h = Planck’s constant
n = positive whole numbers
(Quantum numbers)

7. Max Born The probability of finding the electron at the point in space.

8. Wave-mechanical view of the hydrogen atom
Wave-mechanical view of the hydrogen atom. The electron cloud is like a fan.