Electron Clouds and Probability

Slides:

Advertisements

Similar presentations

Quantum Mechanics Chapter 7 §4-5. The de Broglie Relation All matter has a wave-like nature… All matter has a wave-like nature… Wave-particle.

Advertisements

De Broglie combined Einstien’s E = mc 2 and Planck’s E = hv de Broglie combined Einstien’s E = mc 2 and Planck’s E = hv hv = mc 2 hv = mc 2 Substitute.

Physics and the Quantum Mechanical Model l OBJECTIVES: - Calculate the wavelength, frequency, or energy of light, given two of these values.

Pre-IB/Pre-AP CHEMISTRY

Electromagnetic Radiation and Atomic Structure EMR and Properties of Light Bohr Model of the Atom & Atomic Line Spectra Quantum Theory Quantum Numbers,

Why are electrons restricted to specific energy levels or quantized? Louis de Broglie – proposed that if waves have particle properties, possible particles.

Lecture 2210/26/05. Moving between energy levels.

Wave Nature of Light and Quantum Theory

1 Introduction to quantum mechanics (Chap.2) Quantum theory for semiconductors (Chap. 3) Allowed and forbidden energy bands (Chap. 3.1) What Is An Energy.

CHEMISTRY T HIRD E DITION Gilbert | Kirss | Foster | Davies © 2012 by W. W. Norton & Company CHAPTER 7-B Quantum Numbers.

Quantum Atom. Louis deBroglie Suggested if energy has particle nature then particles should have a wave nature Particle wavelength given by λ = h/ mv.

-The Bohr Model -The Quantum Mechanical Model Chemistry.

Chapter 29 Particles and Waves.

Electrons in Atoms Chapter 5. Duality of Light Einstein proved that matter and energy are related E = mc 2 Einstein proved that matter and energy are.

-The Bohr Model -The Quantum Mechanical Model Mrs. Coyle Chemistry.

Chapter 5/1© 2012 Pearson Education, Inc. Wavelike Properties of Matter The de Broglie equation allows the calculation of a “wavelength” of an electron.

Chapter 6 Electronic Structure of Atoms. The Wave Nature of Light The light that we can see with our eyes, visible light, is an example of electromagnetic.

Quantum Theory the modern atomic model. Bohr Model of the Atom a quantum model proposed by Niels Bohr in 1913 It helped to explain why the atomic emission.

Slide 1 of 38 chemistry. Slide 2 of 38 © Copyright Pearson Prentice Hall Physics and the Quantum Mechanical Model > Light The amplitude of a wave is the.

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

Bohr vs the quantum mechanical model of the atom

1 Chapter 7: Periodicity and Atomic Structure Renee Y. Becker Valencia Community College CHM 1045.

The Quantum Atom Weirder and Weirder. Wave-Particle Duality Louis de Broglie ( )‏

Niels Bohr Based his studies on Hydrogen Proposed energy levels

CONTENT OBJECTIVE understand the electromagnetic spectrum and the mathematical relationships between energy, frequency, and wavelength of light. WHAT.

Orbitals: What? Why? The Bohr theory of the atom did not account for all the properties of electrons and atoms.

The Quantum Model of the Atom CP Chemistry. Louie de Broglie Proposed that all particles of matter that move exhibit wave like behavior (even a baseball!)

Quantum theory Electron Clouds and Probability. Bohr’s model of the atom is unable to describe electron (e - ) behavior in an atom Problem: multiple spectral.

The Quantum Mechanical Model of the Atom = model in which e- are treated as having wave characteristics.

Quantum Atom. Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement.

WARM UP “The service we render others is the rent we pay for our room on Earth.” -Sir Wilfred Grenfell 1.What does this mean to you? 2.How can you be of.

Louis de Broglie, (France, ) Wave Properties of Matter (1923) -Since light waves have a particle behavior (as shown by Einstein in the Photoelectric.

Chemistry I Chapter 4 Arrangement of Electrons. Electromagnetic Radiation Energy that exhibits wavelike behavior and travels through space Moves at the.

Light, Quantitized Energy & Quantum Theory CVHS Chemistry Ch 5.1 & 5.2.

The Quantum Mechanical Model Chemistry Honors. The Bohr model was inadequate.

Warm-Up What is the difference between the Bohr’s Model of the Atom and the Quantum Model of the atom. What wavelength is associated with an electron.

-The Bohr Model -The Quantum Mechanical Model

Postulates of Bohr model

Electron Configurations

Hydrogen Spectrum.

Atomic Structure & Periodicity

Chapter 5: Arrangement of Electrons in Atoms

Postulates of Bohr model

Quantum Model of the Atom

The Quantum Mechanical Model

5.3 Physics and the Quantum Mechanical Model

Electrons and Light Chapter 13.3.

Bohr’s Third Postulate

Arrangement of electrons

Electron Clouds and Probability

Chapter 5 Electrons in Atoms.

Unit 3 – Electron Configurations Part C: Quantum Mechanical Model

Quantum Theory and the Atom

The Quantum Mechanical Model

Section 5.3 Physics and the Quantum Mechanical Model

Quantum Mechanical Model of the Atom

Section 5.2 Quantum Theory and the Atom

Light and Energy Electromagnetic Radiation is a form of energy that is created through the interaction of electrical and magnetic fields. It displays wave-like.

Schrödinger's/ Modern model of the atom

III. Quantum Model of the Atom (p )

Quantum Mechanical Atom Part II: Bohr vs

Niels Bohr Based his studies on Hydrogen Proposed energy levels

Chapter 4 Arrangement of Electrons in Atoms

Unit 4: Electrons in the Atom

Quantum Model of the Atom

Quantum Theory and the Atom

Quantum Mechanical Atom Part II: Bohr vs

Light and EM Spectrum Light is all thanks to electrons…well… photons…but whatever. What do you REALLY know about light?

Bohr vs the quantum mechanical model of the atom

Presentation transcript:

Electron Clouds and Probability Glencoe Chemistry: Matter and Change Chapter 5 Section 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 = 6.626 x 10-34 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

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.

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

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)

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

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