Warmup Use the periodic table and the diagram below to write and sketch (when possible) the orbitals for: Na P Ag.

Slides:

Advertisements

Similar presentations

Aim: How can we explain energy transitions in an atom? Do Now: What were the limitations of the Rutherford model of the atom and how did the Bohr model.

Advertisements

BUSINESS 1.EXAM 2THURSDAY NOVEMBER 4, MATERIAL COVERED: CHAPTERS 4, 5 & 6 3.TIME:7:00PM-8:00PM 4.WHERE:(TO BE ANNOUNCED LATER) 5.WHAT TO BRING:CALCULATOR,

Light as a Wave Waves are traveling disturbances that carry energy from one place to another The speed of a wave is calculated by using the equation: V.

What do you see? Old woman? Or young girl?  Is turning a light on and off a chemical or physical change? ◦ Physical change  What creates light?

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

The Hydrogen Spectrum Experiment 6 amplitude Wavelength -λ.

wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Lecture 15: Bohr Model of the Atom

Lecture 2110/24/05. Light Emission vs. Absorption Black body.

THE BOHR MODEL OF THE ATOM October 23, The Bohr Model of Hydrogen Atom Light absorbed or emitted is from electrons moving between energy levels.

Lecture 2010/19/05. wavelength Amplitude Node Electromagnetic Radiation (Light as waves) Moving Waves.

Modern Atomic Theory Ms. Hoang ACP Chemistry. Summary  Visible light is a small section of the EM spectrum  Light exhibits wave-like and particle-like.

The Bohr Model: Orbits and Line Spectra. Understand the historical development of the Quantum Mechanical Model of the atom. Describe how a produced line.

Physics 1C Lecture 29A.

2.3 Electron Arrangement Atomic Emission Spectra &

Electron Configurations & the Periodic Table Chapter 7.

Electronic Structure of Atoms Chapter 6 BLB 12 th.

Chapter 3 The Structure of the Atom In order to explain much of what is observed in chemistry, we need to adopt a model for the atom where the atom has.

Atomic Theory and Spectroscopy Clues to the Nature of Atoms.

Electromagnetic Spectra Review Game. When do electrons emit light? Moving from higher to lower energy levels.

The Electromagnetic Spectrum and Light. Wavelength - The distance between two consecutive peaks of a wave.

1 Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Quantum Theory and the Electronic Structure of.

Electromagnetic Radiation and Light

Quantization of Energy. When the atom gets excited… To help visualize the atom think of it like a ladder. The bottom of the ladder is called GROUND STATE.

Lab 12 Atomic spectra and atomic structure

Chapter 10: Modern atomic theory Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Quantum Chemistry Chapter 6. Copyright © Houghton Mifflin Company. All rights reserved.6 | 2 Electromagnetic Radiation.

Electronic Structure. Bohr Bohr proposed that the __________ atom has only certain allowable energy states.

Atomic spectra 10/2/14. The Dual Nature of Light: The Particle and The Wave Ancient Greeks people thought of light as a stream of tiny particles -like.

Bellwork What is the majority of the volume of an atom?

The Electromagnetic Spectrum, Planck, and Bohr Honors Coordinated Science II Wheatley-Heckman.

Photons, Electrons, and Atoms. Visible and non-visable light Frequencies around Hz Much higher than electric circuits Theory was about vibrating.

Quantum Theory and the Electronic Structure of Atoms Chapter 7.

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

Quantum Theory and the Electronic Structure of Atoms Chapter 6.

Chapter 7. Electromagnetic Radiation  aka. Radiant energy or light  A form of energy having both wave and particle characteristics  Moves through a.

Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Electrons and Light. Light’s relationship to matter Atoms can absorb energy, but they must eventually release it When atoms emit energy, it is released.

Chapter 5 – Electronic Structure Question: How exactly are electrons arranged around the nucleus of the atom? Answer: It’s pretty complicated.

Light, Energy, & Electrons. Discrepant Events/Questions.

4.1 Refinements of the Atomic Model

Chapter 7: Quantum theory of the atom Chemistry 1061: Principles of Chemistry I Andy Aspaas, Instructor.

Emission Spectra and Bohr-Rydberg

1 2. Atoms and Electrons How to describe a new physical phenomenon? New natural phenomenon Previously existing theory Not explained Explained New theoryPredicts.

Models, Waves, and Light Models of the Atom Many different models: – Dalton-billiard ball model (1803) – Thompson – plum-pudding model (1897) – Rutherford.

Electromagnetic Radiation. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance.

Prepared by Lawrence Kok Tutorial on Electromagnetic Radiation, Emission Line spectrum and Bohr Model.

Electrons in Atoms Chapter 4.

Wave-Particle Nature of Light

Chapter 6 Electronic Structure of Atoms

Arrangement of Electrons in Atoms

Chapter 6: Electromagnetic Radiation

Atomic Structure the wave nature of light 1 2 3 2 Hz 4 Hz 6 Hz 

Electromagnetic Radiation

Chemistry 141 Monday, October 30, 2017 Lecture 23 Light and Matter

Orbits and Line Spectra

Learning Outcomes Emission and absorption spectra of the hydrogen atom . Balmer series in the emission spectrum as an example. Line spectra as evidence.

The Electronic Structure of Atoms

Chapter 2 Notes: electron configuration

Valence Shell Electron Pair Repulsion (VSEPR) Theory

Quantum Theory.

Unit 3: Light and Electrons

Absorption & Emission.

Chapter 4 Arrangement of Electrons in Atoms

Unit 3: Light and Electrons

Chapter 6: Electromagnetic Radiation

Presentation transcript:

Warmup Use the periodic table and the diagram below to write and sketch (when possible) the orbitals for: Na P Ag

Warmup Solutions Na 1s 2 2s 2 p 6 3s 1 P Ag

Warmup 2 Wave Equation 1)An ocean wave has a velocity of 15 m/s and a wavelength of 30 m. What is the frequency in Hz? 2)A light wave has a wavelength of 660 nm. What is its frequency? Planck’s Equation 3) h  Planck’s Constant (6.63 * J*s) f  frequency (Hz) use answer from problem 2. What is the energy of this photon?

SEPTEMBER 20 TH 2010 Bohr Model: Quantized Orbits Rydberg Formula Emission Spectra Flame Test

Bohr Model: Quantized Orbits Main Principles: Atoms have discrete electron orbital patterns. Higher orbits hold more potential energy. A fall from a higher orbital to a lower one releases energy as light. (Energy is conserved) Visible Ultraviolet Infrared

Relevant Equations Potential Energy PE = F * dPE  Potential Energy (J) F  Force of attraction (N) d  Distance (m) Waves v = λ * fv  velocity (3*10 8 m/s) λ  wavelength (m) f  frequency (Hz) Quantization of Photons E = h * fE  Energy (J) h  Planck’s Constant (6.63 * J*s) f  frequency (Hz) Rydberg Formula 1/ λ = R Z 2 (n 1 -2 – n 2 -2 )λ  wavelength (m) R  Rydberg’s Constant (1.1*10 -7 m -1 ) Z  Atomic number n  electron orbital number

Flame Test Goals: 1) Measure the emission spectrum of a particular element. 2) Calculate the frequency and energy of the photons emitted. 3) Compare the measured wavelength to the Rydberg Formula prediction, and identify the line. Assumptions: 1) All visible lines are in the Balmer series (n=2). (Probably true) 2) Each element is ionized down to a single valence electron. (?!) Materials: Metal salts or nitrates Wire or heat-resistant ladles Propane torches Diffraction grating spectroscopes Backup: Spectroscopy tubes Resources:

Data Table Sample ElementMeasured λ (nm) Predicted λ (nm) Upper “n” number Frequency (Hz) Energy (J)