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.

Slides:



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

The Development of a New Atomic Model.
Chapter 4: Arrangement of Electrons in Atoms
Electronic Structure of Atoms Chapter 6 BLB 12 th.
Lighten Up Quantum #’s e- Config’s Calcula- tions Wildcard Chapter 4 Jeopardy Chapter 4 Jeopardy Vital Vocab
Unanswered Questions Rutherford’s model did not address the following questions: What is the arrangement of electrons in the atom? What keeps the electrons.
Concept #4 “Electrons in the Atom” Honors Chemistry 1.
Arrangement of Electrons In Atoms
Chemistry Chapter 4 Arrangement of Electrons in Atoms
1 Ch 4 Electron Energies. 2 Electromagnetic Spectrum Electromagnetic radiation is a form of energy that exhibits wave-like behavior as it travels though.
Chapter 4 Arrangement of Electrons in Atoms. I. The Development of a New Atomic Model H Electromagnetic Radiation: H Electromagnetic Spectrum: H Electromagnetic.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 The Development of a New Atomic Model Properties of Light.
Wave Description of Light
Chapter 4: Arrangement of Electrons in Atoms Chemistry.
Electrons in Atoms By: Ms. Buroker. Okay … We now know that an element’s identity lies in its number of protons … but there is another particle which.
Chapter 4 Arrangement of Electrons in Atoms 4.1 The Development of a New Atomic Model.
Arrangement of Electrons in Atoms Chapter 4. Properties of Light Electromagnetic Radiation- which is a form of energy that exhibits wavelength behavior.
Chapter 5 : Electrons in Atoms. Problems with Rutherford’s Model Chlorine # 17 Reactive Potassium # 19 Very reactive Argon # 18 Not reactive.
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.
Electrons in Atoms. Models of the Atom – A History John Dalton John Dalton atom was solid, indivisible mass atom was solid, indivisible mass J.J. Thomson.
Electrons in Atoms Chapter 5 General Chemistry. Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic.
Mullis1 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location is described using.
Chapter 5: Electrons In Atoms. Wave Nature of Light Electromagnetic Radiation – form of energy that exhibits wavelike behaviors as it travels through.
CHAPTER 4: Section 1 Arrangement of Electrons in Atoms
Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Light is an electromagnetic wave EM wave- a form of energy that exhibits wavelike behavior as it travels through space All the forms of EM radiation form.
Mullis Chemistry Holt Ch.41 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location.
Light is an electromagnetic wave EM wave- a form of energy that exhibits wavelike behavior as it travels through space.
CHAPTER 4.1 THE DEVELOPMENT OF A NEW ATOMIC MODEL.
Chapter 4 ARRANGEMENT OF ELECTRONS IN ATOMS. Section 1 The Development of a New Atomic Model Properties of Light The Wave Description of Light Electromagnetic.
Chemistry Unit 2: the 2 nd half! Electrons and their Properties.
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.
Section 1 The Development of a New Atomic Model Properties of Light The Wave Description of Light Electromagnetic radiation is a form of energy that exhibits.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 4 Arrangement of Electrons in Atoms Section.
Chapter 5 Electrons in Atoms Honors Chemistry Section 5.1 Light and Quantized Energy At this point in history, we are in the early 1900’s. Electrons.
Unanswered Questions Rutherford’s model did not address the following questions: 1. What is the arrangement of electrons in the atom? 2. What keeps the.
Chapter 5 Review. Wave Nature of Light Wavelength- Wavelength- The distance between two consecutive peaks or troughs. Frequency- Frequency- The number.
Electrons in Atoms Chapter Wave Nature of Light  Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through.
Chapter 11 Notes Electrons in Atoms: Modern Atomic Theory.
The Development of A New Atomic Model
Bohr’s Model Rutherford’s model didn’t explain the arrangement of electrons around the nucleus.
CHAPTER 11 NOTES MODERN ATOMIC THEORY RUTHERFORD’S MODEL COULD NOT EXPLAIN THE CHEMICAL PROPERTIES OF ELEMENTS.
Chapter 4 © Houghton Mifflin Harcourt Publishing Company Section 1 The Development of a New Atomic Model Properties of Light The Wave Description of Light.
E LECTRONS IN A TOMS Chapter 5. L IGHT AND Q UANTIZED E NERGY Nuclear atom and unanswered questions Scientists found Rutherford’s nuclear atomic model.
Chapter 5 Electrons in Atoms. Wave Nature of Light Wavelength (λ) – shortest distance between equivalent points on a continuous wave (unit: m or nm) Ex:
Chapter 5.  Energy transmitted from one place to another by light in the form of waves  3 properties of a wave;  Wavelength  Frequency  Speed.
Light Light is a kind of electromagnetic radiation, which is a from of energy that exhibits wavelike behavior as it travels through space. Other forms.
CHAPTER 4 CHEMISTRY. PROPERTIES OF LIGHT (P91-93) Originally thought to be a wave It is one type of ELECTROMAGNETIC RADIATION (exhibits wavelike behavior.
Chapter 4 Electrons In Atoms.
Quiz Review.
Lesson 16 Modern View of the Atom
Arrangement of Electrons in Atoms
Click a hyperlink or folder tab to view the corresponding slides.
Chapter 5: Arrangement of Electrons in Atoms
Atomic Theory.
5-1 Quantum Theory of the atom
Electrons In Atoms.
The Atom and Unanswered Questions
Chapter 4.1 The Development of a New Atomic Model
Quantum Theory.
Electromagnetic spectrum
Arrangement of electrons
Electrons in Atoms Chapter 5.
Arrangement of Electrons in Atoms
Electrons in Atoms Chapter 5.
Chapter 4.1 The Development of a New Atomic Model
Ch 4 Arrangement of Electrons in Atoms 4
Properties of Light.
Electrons in Atoms Ch. 5 Notes.
Presentation transcript:

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 electrons- not complete model

Electromagnetic Radiation- form of energy that exhibits wavelike behavior Ex: visible light, microwaves, x-rays Wave Nature of Light

Electromagnetic Spectrum- encompasses all forms of EM radiation

Electromagnetic Spectrum

Wavelength ( λ ) - shortest distance between equivalent points on a continuous wave Measured crest to crest or trough to trough

Frequency ( ν ) - number of waves that pass a given point per second 1 Hertz (Hz) = 1 wave per second; SI unit of frequency

Amplitude- wave’s height from the origin to a crest or from origin to trough Speed of light = wavelength x frequency C = λν

Photoelectric Effect- electrons are emitted from a metal’s surface when light of a certain frequency shines on the surface Ex: calculator with photoelectric cell

Particle Nature of Light Quantum concept- produces glowing light of hot objects Quantum- minimum amount of energy that can be gained or lost by an atom

E quantum = hv E = energy V = frequency h = Planck’s constant; x Js J is joule; SI unit for energy

Photon- particle of EM radiation with no mass that carries a quantum of energy E photon = hv

Ground State- lowest allowable energy state of an atom Excited State- when an atom gains energy

Line Emission Spectrum- set of frequencies of the EM waves emitted by atoms of the element Unique to each element, used for identification Continuous spectrum

Bohr Model of the Atom- proposed that hydrogen atom has only certain allowable energy states

Sect. 4-2: The Quantum Model of the Atom Electrons as waves…De Broglie applies light’s wave-particle duality to electrons/Bohr’s model

Heisenberg Uncertainty Principle – impossible to know position and velocity at same time Schrödinger wave equation

Quantum theory – describes mathematically the wave properties of electrons Orbital – probable location of electron around nucleus

Atomic Orbitals and Quantum numbers Quantum numbers – specify properties of atomic orbitals and electrons in orbitals solutions to Schrödinger wave equation

Principal quantum number (n) – represents main energy level (shell) & tells how many sublevels Positive integers (1,2,3,etc.) Total # orbitals per shell = n 2 Total # electrons per shell =2n 2

Angular momentum quantum number (l) – indicates shape of orbital (sublevel) l = zero and all positive integers less than or equal to n-1 l=0, s orbital (spherical) l=1, p orbital (dumbbell) l=2, d orbital l=3, f orbital

Magnetic quantum number (m) – indicates the orientation of orbital around nucleus range from -2 to +2, depending on sublevels

Spin Quantum number – indicates spin state of electron can only equal ½ or -½ orbital holds 2 max electrons & they must have opposite spins

Sect. 4-3: Electron Configurations Electron configuration – arrangement of electrons in an atom

Rules for Electron Configurations Aufbau principle – lowest energy level fills first Pauli exclusion principle – electrons in same orbital, opposite spin Hund’s rule – orbitals of equal energy must all have 1 electrons before a second can be added

Orbital Notation (Diagram) – lines, arrows, principal quantum #, and sublevel letter Electron Configuration Notation – principal quantum #, sublevel letter, and superscript (# e-) Noble Gas Notation – shortened version of electron configuration notation

Deviations from normal electron configurations (more stable with pulling one from s to half- fill or fill d) Chromium Copper