Problems with Rutherford’s Model Why do elements produce spectral lines instead of a continuous spectrum? And Why aren’t the negative electrons pulled.

Slides:

Advertisements

Similar presentations

Light and Quantized Energy

Advertisements

Electromagnetic Radiation

Properties of Light Is Light a Wave or a Particle?

Electrons and Light How does the arrangement of electrons in the atom determine the color of light that it emits?

ELECTROMAGNETIC RADIATION AND THE NEW ATOMIC MODEL.

Niels Bohr’s Energy Levels

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.

Light, Photon Energies, and Atomic Spectra

The Evolution of Early Atomic Models. Early Models of Atomic Structure The work of Thomson, Rutherford and Bohr…

Electromagnetic Radiation and Light

12.6 Light and Atomic Spectra

How much energy is contained in a 10 g piece of copper heated 15 degrees Celcius?

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.

Chapter 4 Arrangement of Electrons in Atoms

Light & Quantized Energy Questions about the Atom.

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

Electron Energy and Radiation Quantum Mechanics and Electron Movement.

Where are the electrons ? Rutherford found the nucleus to be in the center. He determined that the atom was mostly empty space. So, how are the electrons.

Chapter 4 Arrangement of Electrons in Atoms

Chapter 5 Section 5.1 Electromagnetic Radiation

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

Physics and the Quantum Mechanical Model

Atomic Emission Spectra

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.

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

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

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

2.2 Electrons in Atoms Niels Bohr ( ) – proposed the ‘planetary model’. Electrons have energy of motion. Electrons absorb energy and move to higher.

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

The Bohr Model of the Atom: Bohr’s major idea was that the energy of the atom was quantized, and that the amount of energy in the atom was related to the.

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

Development of a New Atomic Model Properties of Light.

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.

Quantum Theory and the Atom In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame. Analysis of the emitted.

Electromagnetic Waves Electromagnetic energy is created by objects in outer space and by humans.

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

Section 5.1 Light and Quantized Energy. Objectives Compare the wave and particle models of light Compare the wave and particle models of light Define.

Do Now: 1.If you could solve one problem using science, what would it be? 2.What branch of science do you think you would need to use to solve the problem?

Quantum Theory and the Electronic Structure of Atoms Chapter 7.

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

Observing Atomic Spectra Wave simulation Bohr’s Model 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.

Electrons in Atoms Chapter 4. RUTHERFORD MODEL A NEW ATOMIC MODEL The ____________ model of the atom was a great improvement, but it was incomplete.

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

Ch. 4-1 Models of the Atom. POINT > Describe some basic properties of light POINT > Describe the emission-line spectrum of hydrogen POINT > Identify how.

Electrons in Atoms Chapter 4.

Physics and the Quantum

Physics and the Quantum Mechanical Model

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Quantum Theory and the Electronic Structure of Atoms

Radiant Energy Objectives:

Arrangement of electrons in atoms

Ch. 4-1 Models of the Atom Atomic Structure.

Electrons in Atoms Chapter 4.

Physics and the Quantum Mechanical Model

Why Light, why now?.

Ch. 5: Electrons in the Atom

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Light, Photon Energies, and Atomic Spectra

Section 5.1 Light and Quantized Energy

Light and the electron Quest continues to discover the structure of atom and how electrons are arranged within atoms.

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.

Electromagnetic Spectrum

2.3 Light Objectives 3 and 5:b

Light and Quantized Energy

Chapter 4 Arrangement of Electrons in Atoms

Ch. 5 - Electrons in Atoms Waves & Particles.

Presentation transcript:

Problems with Rutherford’s Model Why do elements produce spectral lines instead of a continuous spectrum? And Why aren’t the negative electrons pulled into the nucleus causing the atom to collapse?

Electrons as Waves Properties of Waves –Wavelength – ( ) the distance between peaks –usually given in nanometers (nm) –Amplitude - (A) maximum displacement from zero

Electrons as Waves Frequency – ( ) the number of waves that pass a point per unit time Cycles /second = 1 Hertz (Hz) What happens to the wavelength as the frequency changes?

Electrons as Waves As decreases, increases How does the energy of the wave change as the frequency increases?

Electromagnetic Spectrum All waves that travel at the speed of light are included in the Electromagnetic Spectrum c = x c = speed of light = 3.00 x 10 8 m/s E = h = hcE = energy h = Planck's constant = x

Visible Light Which color has the greatest ? Red Which color has the greatest ? Violet Which color has the greatest E? Violet

Visible Light Continuous spectrum – emission of all wavelength of visible light Emission Spectrum (bright line spectrum) – the specific set of wavelengths of light emitted from a particular element

Visible Light Continuous Spectrum Examples: Sunlight, incandescent light Emission spectrum examples: energized elements and compounds

-Bohr explained hydrogen's emission spectrum with quantized orbits. - Every element produces a different bright line spectrum due to a different arrangement of electrons

Bohr’s Model of the Atom  The atom can only absorb and emit specific amounts of energy equal to the difference between orbitals.  The orbits are quantized and electrons can only exist in whole number orbits.  Electrons can never be between orbits.

Bohr’s Model With these conditions Bohr was able to explain the stability of atoms as well as the emission spectrum of hydrogen. According to Bohr's model only certain orbits were allowed which means only certain energies are possible. These energies naturally lead to the explanation of the hydrogen atom spectrum.