Electrons in Atoms I. Waves & Particles C. Johannesson.

Slides:

Advertisements

Similar presentations

Electrons and the EM Spectrum

Advertisements

I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )

WHAT IS ENERGY? ABILITY TO DO WORK MEASURED IN JOULES (J)

Chapter Two …continued

Electrons and the EM Spectrum

Niels Bohr in 1913 proposed a quantum model for the hydrogen atom which correctly predicted the frequencies of the lines (colors) in hydrogen’s atomic.

Frequency and Wavelength

Chemistry Chapter 5 Ch5 Notes #1.

CHEMISTRY 161 Chapter 7 Quantum Theory and Electronic Structure of the Atom

Particle Nature of Light page 49 of Notebook VISIBLE LIGHT ELECTRONS.

Ch. 5- Electrons in Atoms Unit 7 Targets: The Electronic Structure of Atoms (Chap 5) I CAN Utilize appropriate scientific vocabulary to explain scientific.

Waves & Particles Ch. 4 - Electrons in Atoms.

Electron Behavior Electron absorb energy and jump to higher energy level (Excited State). Immediately fall back to original level (Ground State) emitting.

I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms.

Chapter 6 Electronic Structure of Atoms Light The study of light led to the development of the quantum mechanical model. Light is a kind of electromagnetic.

C. Johannesson Ch. 4 - Electrons in Atoms. Section 1 The Development of a New Atomic Model Objectives Explain the mathematical relationship among the.

Waves, Particles, and the Spectrum Quantum Theory.

I. Waves & Particles Ch. 6 – Electronic Structure of Atoms.

Arrangement of Electrons in Atoms The Development of a New Atomic Model.

Chapter 13 Section 3 -Quantum mechanical model grew out of the study of light -light consists of electromagnetic radiation -includes radio and UV waves,

LIGHT AND THE QUANTUM MODEL. WAVES Wavelength ( ) - length of one complete wave Frequency ( ) - # of waves that pass a point during a certain time period.

I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms yC. JOHANNESSON.

I. Waves & Particles Electrons in Atoms. A. Waves  Wavelength ( ) - length of 1 complete wave  Frequency ( ) - # of waves that pass a point during a.

Physics and the Quantum Mechanical Model Notes. Light and the Atomic Spectrum Light is composed of waves at different wavelengths The wave is composed.

Part II. Waves & Particles Ch. 5 - Electrons in Atoms.

BIG topics... Light (electromagnetic radiation)  particle/wave dual nature of light  c, λ, ט, E & h Quantum theory (wave mechanical model)  Bohr model.

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

I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms.

The Bohr Model for Nitrogen 1. Bohr Model of H Atoms 2.

Light and the Atom. Light Much of what we know about the atom has been learned through experiments with light; thus, you need to know some fundamental.

ARRANGEMENT of ELECTRONS in ATOMS CHAPTER 4. DESCRIBING THE ELECTRON Questions to be answered: How does it move? How much energy does it have? Where could.

Wavelength and Frequency E = h c =  c = speed of light (3 x 10 8 m/s) = frequency (s -1 )  = wavelength (m) E = energy (Joules or J) h  = Planck’s constant.

Chapter 5 – Electrons in Atoms text pages

Chapter 5: Electrons in Atoms

I. Waves & Particles Ch. 4 - Electrons in Atoms. Light and Electrons zBecause light and electrons have common properties, understanding one helps to understand.

BIG topics... Light (electromagnetic radiation)  particle/wave dual nature of light  c, λ, ט & E Quantum theory (wave mechanical model)  Bohr model.

ELECTROMAGNETIC RADIATION subatomic particles (electron, photon, etc) have both PARTICLE and WAVE properties Light is electromagnetic radiation - crossed.

I. Waves & Particles Ch. 6 – Electronic Structure of Atoms.

Enriched Chemistry Chapter 4 – Arrangement of Electrons in Atoms

Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.

C. Johannesson Ch. 4 - Electrons in Atoms. Section 1 The Development of a New Atomic Model Objectives Explain the mathematical relationship among the.

Chemistry – Chapter 4. Rutherford’s Atomic Model.

Gifted Chemistry - Week 8 MondayChapter 4 Test; Lesson 5-1 Vocab Sheet Tuesday Notes and Guided Practice: Electromagnetic Spectrum; Study Guide 5-1 WednesdayEM.

Electrons in Atoms. Wave Behavior of Light Day 1.

C. Johannesson I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms.

Waves & Particles Ch. 6 - Electrons in Atoms. A. WAVES zLight: a form of electromagnetic radiation yComposed of perpendicular oscillating waves, one for.

A. Waves  Wavelength ( ) - length of one complete wave  Frequency ( ) - # of waves that pass a point during a certain time period hertz (Hz) = 1/s 

Quantum Theory & Bohr’s Model of the Atom Ch. 4 - Electrons in Atoms.

C. Johannesson I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms.

Waves & Particles Electrons in Atoms. Electrons Electrons which are negatively charged, travel around the nucleus (the center of the atom).

Wavelength, Frequency, and Planck’s Constant. Formulas 1)E = hf E = energy (Joules J) h = Planck’s constant = 6.63 x J x s f = frequency (Hz) 2)

5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.

Electrons in Atoms Chapter 4.

Light: Electromagnetic Spectrum

Electromagnetic Radiation

CHAPTER 5:Electrons in Atoms Light and Quantized Energy

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Section 5.1 Light and Quantized Energy

BIG topics... Light (electromagnetic radiation)

I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )

UNIT 3 ELECTRON CONFIGURATION AND MODERN ATOMIC THEORY

Waves and particles Ch. 4.

Light and Quantized Energy

Wavelength and Frequency

5.1 – ELECTRONS IN ATOMS.

Electron Configurations

Electromagnetic Spectrum

Ch. 5 - Electrons in Atoms Waves & Particles.

BIG topics... Light (electromagnetic radiation)

Waves O 1.2 Wave Properties.

Presentation transcript:

Electrons in Atoms I. Waves & Particles C. Johannesson

A. Waves Wavelength () - length of one complete wave Frequency () - # of waves that pass a point during a certain time period hertz (Hz) = 1/s Amplitude (A) - distance from the origin to the trough or crest C. Johannesson

 A A  A. Waves crest greater amplitude (intensity) origin trough greater frequency (color) C. Johannesson

B. EM Spectrum HIGH ENERGY LOW ENERGY C. Johannesson

B. EM Spectrum HIGH ENERGY LOW ENERGY R O Y G. B I V red orange yellow green blue indigo violet C. Johannesson

c =  B. EM Spectrum c: speed of light (3.00  108 m/s) Frequency & wavelength are inversely proportional c =  c: speed of light (3.00  108 m/s) : wavelength (m, nm, etc.) : frequency (Hz) C. Johannesson

B. EM Spectrum  = ?  = c   = 434 nm = 4.34  10-7 m EX: Find the frequency of a photon with a wavelength of 434 nm. GIVEN:  = ?  = 434 nm = 4.34  10-7 m c = 3.00  108 m/s WORK:  = c   = 3.00  108 m/s 4.34  10-7 m  = 6.91  1014 Hz C. Johannesson

C. Quantum Theory Planck (1900) Observed - emission of light from hot objects Concluded - energy is emitted in small, specific amounts (quanta) Quantum - minimum amount of energy change C. Johannesson

C. Quantum Theory vs. Planck (1900) Classical Theory Quantum Theory C. Johannesson

C. Quantum Theory Einstein (1905) Observed - photoelectric effect C. Johannesson

“wave-particle duality” C. Quantum Theory Einstein (1905) Concluded - light has properties of both waves and particles “wave-particle duality” Photon - particle of light that carries a quantum of energy C. Johannesson

C. Quantum Theory The energy of a photon is proportional to its frequency. E = h E: energy (J, joules) h: Planck’s constant (6.6262  10-34 J·s) : frequency (Hz) C. Johannesson

C. Quantum Theory E = ? E = h  = 4.57  1014 Hz EX: Find the energy of a red photon with a frequency of 4.57  1014 Hz. GIVEN: E = ?  = 4.57  1014 Hz h = 6.6262  10-34 J·s WORK: E = h E = (6.6262  10-34 J·s) (4.57  1014 Hz) E = 3.03  10-19 J C. Johannesson