The Atom. Atomic States An atom can be in one of two states: 1.Ground State: When an atom has the lowest possible amount of energy. 2.Excited State: When.

Slides:

Advertisements

Similar presentations

Objectives To learn about the shapes of the s, p and d orbitals

Advertisements

Quantum Theory and the Atom

Chemistry Daily 10’s Week 5.

Electrons. Wave model – scientist say that light travels in the form of a wave.

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?

1. To describe Rutherford’s model of the atom 2. To explore the nature of electromagnetic radiation 3. To see how atoms emit light 11.1 Objectives.

Objectives To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy To learn about Bohr’s model of the hydrogen.

Emission and Absorption of Electromagnetic Energy

Modern Theory of the Atom Quantum Mechanical Model Or Wave Mechanical Model Or Schrodinger’s Model.

Zumdahl • Zumdahl • DeCoste

Quantum Mechanical Model

Entry Task: October 15 th Monday Question: Does it take more energy for the painter to get to the middle of the ladder or the top? You have 5 minutes!!

Zumdahl • Zumdahl • DeCoste

ELECTRONS IN THE ATOM UNIT 4.

General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.1 Chapter 3 Atoms and Elements 3.6 Electron Energy Levels.

10.7 The Hydrogen Orbitals  In the Wave Mechanical model of the atom an orbital represents the space around the nucleus occupied by an electron.  An.

Chapter. 5: Electrons in Atoms

© Copyright Pearson Prentice Hall Slide 1 of 26 Light and Atoms. 5.1.

Day 1. Move like planets around the sun.  In specific circular paths, or orbits, at different levels.  An amount of fixed energy separates one level.

Rutherford’s Atom Electromagnetic Radiation Emission of Energy by Atoms Energy Levels of Hydrogen Atomic Models Hydrogen Orbitals Electron Arrangements.

CHEMISTRY World of Zumdahl Zumdahl DeCoste. Copyright© by Houghton Mifflin Company. All rights reserved. Chapter 11 Modern Atomic Theory.

Chapter 4 Electron Configurations. Early thoughts Much understanding of electron behavior comes from studies of how light interacts with matter. Early.

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.

Section 11.1 Atoms and Energy 1.To describe Rutherford’s model of the atom 2.To explore the nature of electromagnetic radiation 3.To see how atoms emit.

Chemistry 12-5 Aim: Explain energy changes of electrons as they move from the nucleus Do Now: Contemplate 2 things to be thankful for. Which electron has.

Development of Atomic Models

The Hydrogen Atom. Quantum Theory of Atom.

5.1 Revising the Atomic Model > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5 Electrons In Atoms 5.1 Revising.

Explain why different colors of light result

End Show Slide 1 of 20 Ch. 5: Models of the Atom What you need to know: Chapter 5 Timeline pp (theory and people) Definitions: quantum mechanical.

Neils Bohr What keeps the negative electrons from falling toward the positive nucleus?

 What are the components of an atom?  What is in the nucleus?  What are the charges of the subatomic particles?  Where are the electrons?

Chapter 5: Electrons in Atoms

Chapter Rutherford’s Atom: To describe Rutherford’s model of the atom Energy and Light: To explore the nature of electromagnetic radiation.

AtomsSection 3 Modern Models of the Atom 〉 What is the modern model of the atom? 〉 In the modern atomic model, electrons can be found only in certain energy.

Chapter 13 Notes Electron Models. Evolution of Electron Models The first model of the electron was given by J.J. Thompson—the electron’s discoverer. His.

The Electronic structure of an atom. Bohr’s model of an Atom Electrons located in circular orbits around an atom When an electron absorbs or emits energy.

Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s.

Chapter 11 Modern Atomic Theory Rutherford’s Atom  The nuclear atom (atom with a nucleus) resulted from Ernest Rutherford’s Gold Foil Experiment.

Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing.

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.

Unit 4 Energy and the Quantum Theory. I.Radiant Energy Light – electrons are understood by comparing to light 1. radiant energy 2. travels through space.

Quantum Mechanics. Electromagnetic Spectrum Visible Spectrum.

Modern Model of the Atom The emission of light is fundamentally related to the behavior of electrons.

Chapter 7 Atomic Structure. Electromagnetic Radiation Light is a form of electromagnetic (EM) radiation –All forms of EM radiation are types of kinetic.

1 Modern Atomic Theory. 2 In the Rutherford model electrons traveled about the nucleus in an orbit. The Problem with Rutherford Scientists know that just.

Chapter 11 Modern Atomic Theory. EXIT Copyright © by McDougal Littell. All rights reserved.2 Figure 11.1: The Rutherford atom.

Quantums numbers & the probability of where an electron may be found

Electron Configurations

The Bohr Model, Wave Model, and Quantum Model

5-1 Quantum Theory of the atom

Chapter 3 Atoms and Elements

Zumdahl Zumdahl DeCoste

Bohr & Schrödinger.

Electrons in Atoms.

Quantum Theory.

Wave-Particle Duality

The Bohr Model (1913) revolve sun energy

5.2 QUANTUM THEORY & ATOM.

The Bohr Model of the Hydrogen Atom

Light and Quantized Energy

Ms. Hoang’s ACP Chemistry

Section 3: Modern Atomic Theory

5.1 Light and Atoms ..

Electrons in Atoms Rutherford’s model has some limitations

Electron Configuration

Section 3: Modern Atomic Theory

Electrons in Atoms Ch. 13.

Quantum Mechanical Model

Development of Quantum Mechanics Bohr’s Contribution

Presentation transcript:

The Atom

Atomic States An atom can be in one of two states: 1.Ground State: When an atom has the lowest possible amount of energy. 2.Excited State: When an atom has excess energy.

Excited vs. Ground State An atom without energy begins at ground state. When an atom absorbs energy from an outside source, it enters an excited state. When an atom emits a photon of light, it returns back to it’s ground state.

Energy Level Diagram Energy in the photon that is emitted corresponds to the energy used by the atom to get to the excited state.

The Hydrogen Atom Only certain types of photons are produced when Hydrogen atoms release energy. This is because only certain energy changes are occurring. Hydrogen has certain discrete energy levels.

The Hydrogen Atom If a hydrogen atom emits a red photon, it has released a small amount of energy. If a hydrogen atom emits a blue photon, it has released a larger amount of energy.

The Hydrogen Atom Each photon (or packet of light energy) corresponds to a particular energy change in the hydrogen atom. From this diagram, one can see the 4 discrete energy levels of Hydrogen that correspond to the 4 colors of visible light emitted.

The Wave Mechanical Model Scientists knew that the Bohr model was incorrect. They needed a better model. The Wave Mechanical Model described the atomic states by using ORBITALS. Orbitals are NOT like orbits.

The Wave Mechanical Model The Wave Mechanical Model, using the orbital, suggests there is the highest probability of finding the electron at any particular moment near the center of the atom. You can’t be sure the electron will be near the center of the atom, but it probably will. The electron’s path cannot be precisely described, only a prediction of it’s probability. The model gives NO information about when the electron occupies a certain point in space or how it moves.

The Hydrogen Orbitals We have already discussed that the Hydrogen atom has 4 discrete energy levels. These are called “Principal Energy Levels” These energy levels are labeled with whole numbers

The Hydrogen Energy Levels The energy levels are then further divided into sublevels. Principal Energy Level 1, consists of one sublevel: 1s. Principal Energy Level 2, consists of two sublevels: 2s and 2p.

The Hydrogen Energy Levels Principal Energy Level 3, consists of three sublevels: 3s, 3p, and 3d. Principal Energy Level 4, consists of four sublevels: 4s, 4p, 4d, and 4f.

Energy Levels & Orbitals These sublevels contain spaces for the electron that we call orbitals. Principal energy level 1 consists of just one sublevel or one type of orbital. This orbital is spherical in shape. We label this orbital 1s. The number 1 is for the principal energy level. The s labels the particular sublevel.

Energy Levels & Orbitals Principal Energy Level 2 has 2 sublevels: 2s & 2p. The 2s sublevel consists of one orbital: 2s. The 2p sublevel consists of three orbitals: 2p x, 2p y, 2p z.

Orbitals Different orbitals have different shapes. The s orbital is always a sphere. It can hold 2 electrons. The p orbital has 2 lobes. Each set of lobes: x, y, & z can hold 2 electrons, so the p orbital can hold a total of 6 electrons. The d and f orbitals have other shapes.