Chapter 4.1 The Development of a New Atomic Model

Slides:



Advertisements
Similar presentations
CH 4 NOTES HOW ELECTRONS ARE ARRANGED. ELECTROMAGNETIC SPECTRUM Includes : –Gamma rays –Xrays –Ultraviolet –Visible –Infrared –Microwaves –Radio waves.
Advertisements

Electron Configuration Notation with Atomic Structure Review
Electronic Structure of Atoms Chapter 6 BLB 12 th.
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.
Quantum Chemistry Chapter 6. Copyright © Houghton Mifflin Company. All rights reserved.6 | 2 Electromagnetic Radiation.
Chapter 4 Electron Configurations. Early thoughts Much understanding of electron behavior comes from studies of how light interacts with matter. Early.
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 13.3 Physics and the Quantum Mechanical Model
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electromagnetic Radiation Radiant energy that exhibits wavelength-like behavior and.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electromagnetic Radiation Radiant energy that exhibits wavelength-like behavior and.
Quantum Theory. The Quantum Model of the Atom Heisenberg Uncertainty Principle: This idea involves the detection of electrons. Electrons are detected.
Electrons in Atoms Chapter 5 General Chemistry. Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic.
Chapter 4.1 The Development of a New Atomic Model.
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.
Atomic Structure and Periodicity. Atoms ProtonsNeutronsElectrons 1. Where are the electrons 2. Do they have different energies.
Mullis Chemistry Holt Ch.41 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location.
CHAPTER 4.1 THE DEVELOPMENT OF A NEW ATOMIC MODEL.
Chemistry Unit 2: the 2 nd half! Electrons and their Properties.
Light and Energy Electromagnetic Radiation is a form of energy that emits wave-like behavior as it travels through space. Examples: Visible Light Microwaves.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 4 Arrangement of Electrons in Atoms Section.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electromagnetic Radiation Radiant energy that exhibits wavelength-like behavior and.
Chapter 5 Review. Wave Nature of Light Wavelength- Wavelength- The distance between two consecutive peaks or troughs. Frequency- Frequency- The number.
Chapter 11 Notes Electrons in Atoms: Modern Atomic Theory.
Properties of Light Electromagenetic Spectrum. Electromagnetic Spectrum Types of electromagnetic radiation -the range containing all of the possible frequencies.
The Development of A New Atomic Model
Bohr’s Model Rutherford’s model didn’t explain the arrangement of electrons around the nucleus.
Chapter 4.1 The Development of a New 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.
Light, Quantitized Energy & Quantum Theory EQ: What does the Modern Atom look like? CVHS Chemistry Ch 5.
IV. Electron Configuration (p , )
Electron Configuration
Arrangement of Electrons in Atoms
Chapter 5: Arrangement of Electrons in Atoms
5-1 Quantum Theory of the atom
Electrons In Atoms.
Electron Configuration
The Atom and Unanswered Questions
Electron Configuration Orbitals
Quantum Theory and the Electronic Structure of Atoms
Electromagnetic spectrum
Electron Configuration
Arrangement of electrons
The Quantum Model Chapter 4.
Quantum Model of the Atom
Chapter 5 Introductory Assignment
Unit. 5 Electron Configuration
Arrangement of Electrons in Atoms
Electrons in Atoms Chapter 5.
Electromagnetic spectrum
Arrangements of Electrons in Atoms
Energy Levels & Orbitals
Chapter 4.1 The Development of a New Atomic Model
Arrangement of Electrons in Atoms
Ch 4 Arrangement of Electrons in Atoms 4
Chapter 4 Arrangement in Electrons in Atoms
Electron Configuration
Let’s Review – orbitals defined by their shape / orientation
Chapter 4 Electron Arrangement.
Presentation transcript:

Chapter 4.1 The Development of a New Atomic Model

Properties of Light Light as a wave: Visible light is a type of electromagnetic radiation, along with X-rays, ultraviolet and infrared light, microwaves, and radio waves. These form the electromagnetic spectrum. Waves have a repetitive nature and can be measured by wavelength() & frequency(). Wavelength unit is cm or nm. Frequency unit is waves/sec or hertz (Hz).

c = speed of light or 3.00 x 108 m/s Frequency and wavelength are related to each other through the following equation: c =  c = speed of light or 3.00 x 108 m/s As wavelength increases, frequency decreases and vice versa.

Change cm to m and plug into equation Example Determine the frequency () of light whose wavelength () is 6.87 x 10-8 cm. c =  c = 3.00 x 108 m/s = c/ Change cm to m and plug into equation = 3.00 x 108 m/s 6.87 x 10-10 m  = .437 x 1018 ≈ 4.37 x 1017 Hz

Light as a particle: Photoelectric effect is the emission of electrons from metal when light shines on it. A quantum of energy is the minimum amount of energy that can be lost or gained by an atom. A photon is a particle of electromagnetic radiation with no mass and carrying a quantum of energy.

The Hydrogen-Atom Line-Emission Spectrum When current is passed through a gas, it goes from the ground state to the excited state. It emits light known as the emission-line spectrum. When an excited hydrogen atom falls to its ground state, it emits a photon of radiation.

Ch 4.2 Notes The Quantum Model of the Atom Objectives: To describe the quantum mechanical model of the atom. To describe the relative sizes and shapes of s and p orbitals.

Electrons as Waves Behavior of electrons is similar to the behavior of waves. Electron waves can only exist at certain frequencies.

Heisenberg Uncertainty Principle Werner Heisenberg had an idea on how to detect the location of electrons. Heisenberg Uncertainty Principle: it is impossible to determine simultaneously both the position and velocity (speed) of an electron.

The Schrödinger Wave Equation Developed an equation that treated electrons in atoms as waves and quantization of electron energies was an outcome of the equation. Quantum Theory: mathematically describes the wave properties of electrons and other very small particles.

Principal Quantum Number ( n ) Main energy level (shell) Size of the orbital PERIOD # Number of orbitals per main energy level is equal to n2. Number of electrons = 2n2. 1s 2s s Orbitals – Orbitals with l = 0 are s orbitals and are spherically symmetrical, with the greatest probability of finding the electron occurring at the nucleus. – All orbitals with values of n > 1 and l  0 contain one or more nodes. – Three things happen to s orbitals as n increases: 1. they become larger, extending farther from the nucleus 2. they contain more nodes 3. for a given atom, the s orbitals become higher in energy as n increases due to the increased distance from the nucleus 3s Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Angular Momentum Quantum Number Indicates the shape of the orbital, represented by l. Values of l allowed are 0 and all positive integers less than or equal to n -1. Ex. If n=2, shapes are l = 0 and l = 1 A sublevel consists of orbitals in a main energy level with the same value of l.

Magnetic Quantum Number Indicates the orientation of an orbital around the nucleus, represented by m. Values of m are whole numbers, including zero, from –l to +l

Shapes of s, p, and d-Orbitals s orbital p orbitals • p orbitals – Orbitals with l = 1 are p orbitals and contain a nodal plane that includes the nucleus, giving rise to a “dumbbell shape.” – The size and complexity of the p orbitals for any atom increase as the principal quantum number n increases. • d orbitals – Orbitals with l = 2 are d orbitals and have more complex shapes with at least two nodal surfaces. • f orbitals – Orbitals with l = 3 are f orbitals, and each f orbital has three nodal surfaces, so their shapes are complex. d orbitals

Maximum Number of Electrons In Each Sublevel Sublevel Number of Orbitals of Electrons s 1 2 p 3 6 d 5 10 f 7 14 LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 146

Copyright © 2006 Pearson Benjamin Cummings. All rights reserved.

Spin Quantum Number A single orbital has a maximum of two electrons, and those electrons must have opposite spins. It has two values +1/2 and -1/2

Ch 4.3 Electron Configurations Electron Configurations: the arrangement of electrons in an atom. Each element has a unique electron configuration. Ground-state Electron Configuration is the lowest energy arrangement of the electrons for an element.

Aufbau Principle General Rules Electrons fill the lowest energy orbitals first. “Lazy Tenant Rule”

Hund’s Rule WRONG RIGHT General Rules Within a sublevel, place one electron per orbital before pairing them. “Empty Bus Seat Rule” WRONG RIGHT Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Pauli Exclusion Principle General Rules Wolfgang Pauli Pauli Exclusion Principle Each orbital can hold TWO electrons with opposite spins. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Electron Filling in Periodic Table s s p 1 2 d 3 4 5 6 7 f

Elements in the s - blocks really should include He, but He has the properties of the noble gases, and has a full outer level of electrons. 31

The P-block p1 p2 p3 p4 p6 p5 32

Transition Metals - d block Note the change in configuration. s1 d5 s1 d10 d1 d2 d3 d5 d6 d7 d8 d10 33

F - block f1 f5 f2 f3 f4 f6 f7 f8 f9 f10 f11 f12 f14 f13 Called the “inner transition elements” Lanthanides and Actinides f1 f5 f2 f3 f4 f6 f7 f8 f9 f10 f11 f12 f14 f13 34

35

1s1 Periodic Patterns 1st Period s-block # element in block Example - Hydrogen 1s1 # element in block 1st Period s-block Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

1s2 2s2 2p3 N 1s 2s 2p 7e- Notation N Orbital Notation 14.0067 7 Notation Orbital Notation 1s 2s 2p N 7e- Electron Configuration 1s2 2s2 2p3 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Electron Filling in Periodic Table s s p 1 2 d 3 K 4s1 Ca 4s2 Sc 3d1 Ti 3d2 V 3d3 Cr 3d4 Cu 3d9 Cr 3d5 Mn 3d5 Fe 3d6 Co 3d7 Ni 3d8 Cu 3d10 Zn 3d10 Ga 4p1 Ge 4p2 As 4p3 Se 4p4 Br 4p5 Kr 4p6 4 Cr 4s13d5 Cu 4s13d10 Cr 4s13d5 4s 3d Cu 4s13d10 4s 3d

Order in which subshells are filled with electrons (Fig 19 pg 116) 2 2 6 2 6 2 10 6 2 10 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d …

Shorthand Electron Configuration Ge 72.61 32 Shorthand Electron Configuration Example - Germanium [Ar] 4s2 3d10 4p2 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

S 16e- 1s2 2s2 2p6 3s2 3p4 S 16e- [Ne] 3s2 3p4 Noble Gas Notation 32.066 16 Noble Gas Notation Longhand Configuration S 16e- 1s2 2s2 2p6 3s2 3p4 Core Electrons Valence Electrons Shorthand Configuration S 16e- [Ne] 3s2 3p4 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem