Chapter 7: Quantum Mechanical Model of Atom CHE 123: General Chemistry I Dr. Jerome Williams, Ph.D. Saint Leo University.

Slides:

Advertisements

Similar presentations

Quantum mechanics and electron structure The missing link in Bohr’s model was the quantum nature of the electron Quantum mechanics yields a viable model.

Advertisements

1 Vanessa N. Prasad-Permaul Valencia Community College CHM 1045.

Lecture 2210/26/05. Moving between energy levels.

Quantum numbers.

Quantum Mechanics  Bohr’s theory established the concept of atomic energy levels but did not thoroughly explain the “wave-like” behavior of the electron.

Chapter 5 Periodicity and Atomic Structure. Q UANTUM M ECHANICS AND THE H EISENBERG U NCERTAINTY P RINCIPLE In 1926 Erwin Schrödinger proposed the quantum.

Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave.

C h a p t e rC h a p t e r C h a p t e rC h a p t e r 5 5 Periodicity & Atomic Structure Chemistry, 4th Edition McMurry/Fay Chemistry, 4th Edition McMurry/Fay.

Electronic Structure of Atoms © 2009, Prentice-Hall, Inc. Chapter 6 Electronic Structure of Atoms Chemistry, The Central Science, 11th edition Theodore.

Periodicity and Atomic Structure

Chapter 3: Periodicity and the Electronic Structure of Atoms

Chapter 5 Section 5.3 & 5.4 The Quantum Model. Problems with the Bohr Model 1. Worked well for predicting hydrogen spectrum, but not for elements with.

Chapter 4 Notes for those students who missed Tuesday notes.

MULTIELECTRON ATOMS l ELECTRON SPIN: Electron has intrinsic angular momentum - “spin”; it behaves as if it were “spinning”, i.e. rotating around its axis.

The Quantum Model of the Atom

CHEMISTRY T HIRD E DITION Gilbert | Kirss | Foster | Davies © 2012 by W. W. Norton & Company CHAPTER 7-B Quantum Numbers.

Chapter 4-2 The Quantum Model of the Atom Coach Kelsoe Chemistry Pages 104–110.

Quantum Mechanical Theory. Bohr Bohr proposed that the hydrogen atom has only certain _________________. Bohr suggested that the single electron in a.

The Wave Nature of Light. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance.

Chapter 6 Electronic Structure of Atoms

Chapter 6 Electronic Structure of Atoms. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation.

Quantum Mechanical Model of the Atom Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found. These.

Electromagnetic Spectrum Atomic Emission Spectrum.

Quantum Cloud Model Why did Bohr propose the orbit or planetary model? Why did Bohr propose the orbit or planetary model? He based it on experiments with.

Electronic Structure of Atoms © 2009, Prentice-Hall, Inc. Chapter 7 Electronic Structure of Atoms.

Chapter 5/1© 2012 Pearson Education, Inc. Wavelike Properties of Matter The de Broglie equation allows the calculation of a “wavelength” of an electron.

PART 2 QUANTUM THEORY.

Quantum Numbers and Electronic Configuration

Quantum Theory the modern atomic model. Bohr Model of the Atom a quantum model proposed by Niels Bohr in 1913 It helped to explain why the atomic emission.

Aufbau Principle An electron occupies the lowest energy orbital that can receive it.

Quantum Atom. Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement.

Arrangement of Electrons in Atoms

1 Atomic Spectra Blackbody radiation is the visible glow that solid objects emit when heated. Max Planck (1858–1947): proposed the energy is only emitted.

The Quantum Model of the Atom Section 4.2. Bohr’s Problems Why did hydrogen’s electron exist around the nucleus only in certain allowed orbits? Why couldn’t.

1 Chapter 7: Periodicity and Atomic Structure Renee Y. Becker Valencia Community College CHM 1045.

River Dell Regional High School Unit 3 – Electron Configurations Part C: Quantum Mechanical Model.

Warm Up9/20 Draw the Bohr Model for Aluminum What is the difference between a hypothesis and a theory?

Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave. 

Atomic Orbitals And Quantum Numbers. Quantum Numbers A series of 4 numbers (and/or letters) that specify the properties of an electron in its orbit The.

Section 11.3 Atomic Orbitals 1.To identify the shapes of the s, p, d, and f orbitals 2.To describe the energy levels and orbitals of the wave mechanical.

November 13, Please staple both labs together and place in basket. a.Spectra lab 1 st, Flame test 2 nd 2.Then review by completing the following:

The Quantum Model of the Atom CP Chemistry. Louie de Broglie Proposed that all particles of matter that move exhibit wave like behavior (even a baseball!)

Chapter 5: Periodicity and Atomic Structure

Electron Orbitals Cartoon courtesy of lab-initio.com.

Quantum Atom. Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement.

Bulls-eye Activity. Did the pennies consistently drop in the same ring? Can we use our empirical evidence to predict exactly where a penny would land?

Quantum Mechanical Model of Atom. Name This Element.

Louis de Broglie, (France, ) Wave Properties of Matter (1923) -Since light waves have a particle behavior (as shown by Einstein in the Photoelectric.

Its all about the Electron. Bohr’s Model Planetary model Electrons follow a spherical path around the nucleus called Orbits –Known as Energy levels –Has.

The Quantum Mechanical Model of the Atom

The Bohr Model, Wave Model, and Quantum Model

Quantum Mechanical Model of the Atom

the quantum model of the atom

Electronic Structure of Atoms

Historical Overview of Quantum Mechanical Discoveries

The Quantum Mechanical Model

Quantum Theory Light Theory Part 4.

Electron Orbitals Heisenberg 1. The ____________ ______________ principle states that it is impossible to determine simultaneously both the position and.

Chapter 4 Electrons as Waves

Electronic structure in atoms

Chapter 4 ARRANGEMENT OF ELECTRONS IN ATOMS.

Chapter 4 Quantum Numbers and e- configurations

Electrons in the Atom.

The Bohr Model, Wave Model, and Quantum Model

Presentation transcript:

Chapter 7: Quantum Mechanical Model of Atom CHE 123: General Chemistry I Dr. Jerome Williams, Ph.D. Saint Leo University

Overview Bohr Model of Hydrogen Atom Quantum Mechanical Model of Atom Quantum Numbers

Bohr Model of Hydrogen Atom Niels Bohr - described atom as electrons circling around a nucleus and concluded that electrons have specific energy levels. Limited only to Hydrogen atom or Hydrogen like ion.

Bohr Model of Hydrogen Atom Energy levels evaluated using the following equation E = x J (Z 2 / n 2 ) ΔE = E (final) – E (initial) = x J [ (1 / n final 2 – 1 / n inital 2 ) ]

Quantum Mechanical Model of Atom Erwin Schrödinger - proposed quantum mechanical model of atom, which focuses on wavelike properties of electrons.

Quantum Mechanical Model of Atom Werner Heisenberg - showed that it is impossible to know (or measure) precisely both the position and velocity (or the momentum) at the same time. The simple act of “seeing” an electron would change its energy and therefore its position.

Quantum Mechanical Model of Atom Erwin Schrödinger - developed a compromise which calculates both the energy of an electron and the probability of finding an electron at any point in the molecule. This is accomplished by solving the Schrödinger equation, resulting in the wave function, .

Quantum Numbers Wave functions describe the behavior of electrons. Each wave function contains three variables called quantum numbers: – Principal Quantum Number (n) – Angular-Momentum Quantum Number (l) – Magnetic Quantum Number (m l )

Quantum Numbers Principal Quantum Number (n): Defines the size and energy level of the orbital. n = 1, 2, 3,  As n increases, the electrons get farther from the nucleus. As n increases, the electrons’ energy increases. Each value of n is generally called a shell.

Quantum Numbers Angular-Momentum Quantum Number (l): Defines the three- dimensional shape of the orbital. For an orbital of principal quantum number n, the value of l can have an integer value from 0 to n – 1. This gives the subshell notation: l = 0 = s - orbital l = 1 = p - orbital l = 2 = d - orbital l = 3 = f - orbital l = 4 = g - orbital

Quantum Numbers Magnetic Quantum Number (m l ): Defines the spatial orientation of the orbital. For orbital of angular-momentum quantum number, l, the value of m l has integer values from –l to +l. This gives a spatial orientation of: l = 0 giving m l = 0 l = 1 giving m l = –1, 0, +1 l = 2 giving m l = –2, –1, 0, 1, 2, and so on…...

Quantum Numbers

Why can’t an electron have the following quantum numbers? – (a) n = 2, l = 2, m l = 1(b) n = 3, l = 0, m l = 3 – (c) n = 5, l = –2, m l = 1 Give orbital notations for electrons with the following quantum numbers: – (a) n = 2, l = 1, m l = 1(b) n = 4, l = 3, m l = –2 – (c) n = 3, l = 2, m l = –1

Quantum Numbers Spin Quantum Number (m s ): The Pauli Exclusion Principle states that no two electrons can have the same four quantum numbers.