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

Slides:

Advertisements

Similar presentations

Chapter Two …continued

Advertisements

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

Frequency and Wavelength

Light and Quantized Energy

Electromagnetic Radiation

Chapter 5 Electrons In Atoms.

ENERGY & LIGHT THE QUANTUM MECHANICAL MODEL. Atomic Models What was Rutherford’s model of the atom like? What is the significance of the proton? What.

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

ELECTROMAGNETIC RADIATION AND THE NEW ATOMIC MODEL.

Formation of Light Nucleus e e Lithium Atom + Ground State e e Excited State e Electron Returns to Ground State Light is given off e Ion is formed Li.

Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.

Ch. 6 Electronic Structure and the Periodic Table Part 1: Light, Photon Energies, and Emission Spectra.

Electromagnetic Radiation and Light

Many scientists found Rutherford’s Model to be incomplete  He did not explain how the electrons are arranged  He did not explain how the electrons were.

Section 5.3 Physics and the Quantum Mechanical Model

LIGHT AND THE ELECTRON Quantized Energy. The Wave-Particle Duality  Light sometimes behaves like a wave. At other times, it acts as a particle.  Scientists.

Electron Energy and Radiation Quantum Mechanics and Electron Movement.

Chemistry Chapter 4 Arrangement of Electrons in Atoms

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

Physics and the Quantum Mechanical Model

Atomic Emission Spectra

Electrons in Atoms Chapter 5 General Chemistry. Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic.

Waves & Electromagnetic Spectrum

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

DO NOW… Draw the diagram that reminds you of the correct order of electron orbitals. Write out the electron configuration for Pd in full form and in noble.

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

Chapter 5: Electrons In Atoms. Wave Nature of Light Electromagnetic Radiation – form of energy that exhibits wavelike behaviors as it travels through.

Electromagnetic Radiation & Light. 2 What are the atom models we know of? 2.

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

So how am I supposed to remember the order of the rooms? 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 8 46 total e - Pd orbitals? Noble Gas Notation.

CHAPTER 4: Section 1 Arrangement of Electrons in Atoms

Chapter 4 Arrangement of Electrons in Atoms. 4-1 The Development of the New Atomic Model Rutherford’s atomic model – nucleus surrounded by fast- moving.

LIGHT REVIEW MRS. ROSE HCHEM WHAT IS THE WAVELENGTH AND FREQUENCY OF LINE 1 AND LINE 2?

Electronic Structure of Atoms Chapter 4 Electronic Structure of Atoms.

Electromagnetic radiation – transmission of energy through space in the form of oscillating waves wavelength, – distance between identical points on successive.

Electrons in Atoms Light is a kind of electromagnetic radiation. All forms of electromagnetic radiation move at 3.00 x 10 8 m/s. The origin is the baseline.

Enriched Chemistry Chapter 4 – Arrangement of Electrons in Atoms

Light and Energy Electromagnetic Radiation is a form of energy that emits wave-like behavior as it travels through space. Examples: Visible Light Microwaves.

Physics and the Quantum Mechanical Model.  Light consists of waves  A wave cycle begins at zero, increases to its highest value (crest), returns to.

Electrons in Atoms Chapter Wave Nature of Light  Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through.

Electron Structure. Bohr Model Used to explain the structure of the Hydrogen Atom –Hydrogen has only one electron This electron can only circle the nucleus.

Lesson 3 : The Bohr Model. Bohr Model of an Atom  Electrons orbit the nucleus in fixed energy ranges called orbits (energy levels)  An electron can.

Electrons in Atoms. Wave Behavior of Light Day 1.

Chapter 11 Notes Electrons in Atoms: Modern Atomic Theory.

The Development of A New Atomic Model

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

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

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

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

Chapter 5.  Energy transmitted from one place to another by light in the form of waves  3 properties of a wave;  Wavelength  Frequency  Speed.

Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Electromagnetic Spectrum

Quantum Theory.

Electrons in Atoms Chapter 5.

Light, Photon Energies, and Atomic 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 )

ATOMIC STRUCTURE.

Waves and particles Ch. 4.

Electromagnetic Spectrum

Chemistry “Electrons in Atoms”

Wavelength and Frequency

5.1 – ELECTRONS IN ATOMS.

Ch. 5 - Electrons in Atoms Waves & Particles.

BIG topics... Light (electromagnetic radiation)

Arrangement of Electrons in the Atom

BIG topics... Light (electromagnetic radiation)

Presentation transcript:

BIG topics... Light (electromagnetic radiation)  particle/wave dual nature of light  c, λ, ט & E Quantum theory (wave mechanical model)  Bohr model of Hydrogen atom  absorption/emission  orbital shapes Electron configurations  orbital, e - configuration  noble gas notation  Aufbau, Pauli & Hund

Waves Wavelength ( ) - length of one complete wave. Common units: m or nm Frequency ( ) - # of waves that pass a point during a certain time period Common Units: hertz (Hz) = 1/s = s -1 Amplitude (A) - distance from the origin to the trough or crest Courtesy Christy Johannesson

Wavelength and Frequency E = h c =  c = speed of light (3.0 x 10 8 m/s)‏ = frequency (s -1 )‏  = wavelength (m)‏ E = energy (Joules or J)‏ h  = Planck’s constant (6.626 x J s)‏ = frequency (s -1 )‏ “nu” “lamda” Highest energy Moderate energy Lowest energy

Visible part of EM SPectrum PRISM Slit Ray of White Light Waves 1 / 33,000 ” long Waves 1 / 70,000 ” long R ed O range Y ellow G reen B lue I ndigo V iolet 400 nm – 700 nm

Electromagnetic Spectrum

Excitation of Hydrogen Atoms

Return to Ground State

An Excited Lithium Atom Photon of red light emitted Li atom in lower energy state Excited Li atom Energy

Quantum Theory Max Planck (1900)‏ Max Planck (1900)‏ Observed - emission of light from hot objects Observed - emission of light from hot objects Concluded - energy is emitted in small, specific amounts (quanta)‏ Concluded - energy is emitted in small, specific amounts (quanta)‏ Quantum - minimum amount of energy gained or lost by an atom Quantum - minimum amount of energy gained or lost by an atom Courtesy Christy Johannesson

Continuous vs. Quantized Energy Energy A B continuous quantized A continuous B quantized

Bohr Model of Hydrogen Nucleus Possible electron orbits e Great theory, BUT it turned out to be totally wrong!! Next week we’ll see a better theory Further away from nucleus means higher energy level…

Emission Spectrum of Hydrogen 1 nm = 1 x m = “a billionth of a meter” 410 nm434 nm486 nm656 nm

Continuous and Line Spectra light Na H Ca Hg nm Visible spectrum  (nm)

Preview....Orbital Shapes