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Glencoe Chemistry: Matter and Change Chapter 5 Section 2 De Broglie Hypothesis m = mass c = 3.00 x 108 m/s E = mc2 and E = hν E = Energy (joules) v (nu) = Frequency h = 6.626 x 10-34 joules/Hz Predicted the wavelength of a particle using: λ= λ= wavelength (meters) h = Planck’s constant m = mass (kg) v = velocity (m/s) not nu h/λm = v ℎ 𝑚𝑣 h/λv = m 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=mxv Visible objects at ordinary velocities. Quantum mechanics Extremely small particles at velocities near the speed of light. Heisenberg Uncertainty Principle ΔP Δx ≥ h ΔP = Uncertainty of momentum Δx = Uncertainty of position h = Planck’s constant ΔP Δx inversely proportional Erwin Schrödinger Treated the electron as a wave and developed a model that describes the behavior of the electron. 2𝜋2𝑚𝑒4 2 2 ℎ𝑛 m = mass of electron e = charge of electron h = Planck’s constant n = positive whole numbers (Quantum numbers) Max Born The probability of finding the electron at the point in space. Wave-mechanical view of the hydrogen atom. The electron cloud is like a fan.