6.3 Q UANTUM N UMBERS, O RBITALS, AND P ROBABILITY P ATTERNS Chemistry Ms. Pollock 2013 - 2014.

Slides:

Advertisements

Similar presentations

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

Advertisements

LECTURE Sixteen CHM 151 ©slg

Electron Configuration Mapping the electrons. Electron Configuration The way electrons are arranged around the nucleus.

Chapter 5 Electronic Structure and Periodic Trends

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

Quantum Mechanical Model of the Atom

-The Bohr Model -The Quantum Mechanical Model Chemistry.

The Quantum Mechanical Model

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.

Electron Configuration Notation (ECN). Bohr’s Model - electrons travel in definite orbits around the nucleus. Move like planets around the sun. Energy.

Electrons in Atoms. Models of the Atom – I can identify the inadequacies in the Rutherford atomic model I can identify the new proposal.

-The Bohr Model -The Quantum Mechanical Model Mrs. Coyle Chemistry.

1 Mr. ShieldsRegents Chemistry U06 L03 2 Bohr Model e - transitions from a higher energy levels to lower energy levels release energy in the form of.

Arrangement of Electrons in Atoms

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

Quantum Mechanical Model

Explain why different colors of light result

Electrons as waves Scientists accepted the fact that light has a dual wave- particle nature. De Broglie pointed out that in many ways the behavior of the.

Electrons in the Atom. Heisenberg Uncertainty Principle This is the theory that states that it is impossible to determine simultaneously both the position.

Quantum Mechanics Unit 4 – The Electron. 12/22/2015Free PowerPoint Template from Quantum Mechanics Werner Heisenberg – Father of.

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

Text page Applying Quantum Mechanics to Electrons in Atoms Quantum Numbers In an atom, these three-dimensional electron waves or orbitals are more.

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

Electrons in Atoms. Flaws in Rutherford’s Atomic Model Discovered dense positive piece at the center of the atom- “nucleus” Atom is mostly empty space.

Bohr’s Model - electrons travel in definite orbits around the nucleus. Move like planets around the sun. Energy levels – the region around the nucleus.

Electron Configuration. Objectives Describe the relationship between orbitals and energy levels for the electrons of an atom Describe the relationship.

Slide 1 of 26 chemistry. Slide 2 of 26 © Copyright Pearson Prentice Hall Models of the Atom > The Development of Atomic Models The timeline shoes the.

Chapter 5.  From Democritus to Rutherford, models of the atom have changed due to new experiments.  As technology develops, a more complete model of.

QUANTUM MECHANICAL MODEL  Determines the allowed energies an electron can have  Determines how likely it is to find the electron in various locations.

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.

Electron Configuration Quantum Mechanics (Ohh scary)

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.

The Quantum Mechanical Model of the Atom. Schrodinger The quantum mechanical model determines the energy an electron can have and the PROBABILITY of finding.

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:

Quantum theory Electron Clouds and Probability. Bohr’s model of the atom is unable to describe electron (e - ) behavior in an atom Problem: multiple spectral.

Electrons in Atoms Chapter Wave Nature of Light  Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through.

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.

4.2b Quantum Numbers and Atomic Orbitals. POINT > Describe the Principle Quantum number as an energy level POINT > Calculate number of electrons at different.

Slide 1 of 26 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 26 Models of the Atom The scale model shown is a physical model. However, not all.

The Quantum Mechanical Picture of the Atom

Models of the Atom.

Orbitals and Quantum Numbers

3.4 Quantum Numbers.

Quantum Mechanical Model of the Atom

4.2b Quantum Numbers and Atomic Orbitals

Basic Chemistry Chapter 5 Electronic Structure and Periodic Trends

Electronic Structure of Atoms

Electronic Structure of Atoms

Section 3: The Quantum Mechanical Model of the Atom

III. Quantum Model of the Atom (p )

The Quantum Mechanical Model

QUANTUM MECHANICAL MODEL OF THE ATOM

The Heisenberg Uncertainty Principle states that it is impossible to know with high levels of certainty both the location and the velocity of an electron.

QUANTUM MECHANICAL MODEL OF THE ATOM

Electron Configuration

Electron Configuration

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

The Quantum Mechanical Model

Section 1: Revising the Atomic Model

Ms. Hoang’s ACP Chemistry

Atomic Orbitals.

Atomic Orbitals and Electron Arrangement

Electron Arrangement.

Electron Configuration

QUANTUM MECHANICS VIEW OF THE ATOM.

III. Quantum Model of the Atom (p )

III. Quantum Model of the Atom (p )

Electrons in the Atom.

Presentation transcript:

6.3 Q UANTUM N UMBERS, O RBITALS, AND P ROBABILITY P ATTERNS Chemistry Ms. Pollock

Introduction ▪ Schrodinger’s wave equation gave correct description for electron behavior in almost every case ▪ Few scientists able to describe electron behavior during bonding or reactions – best understood by considering electrons to be particles ▪ Schrodinger’s equations used by Max Born to show probability of finding electron at point in space for which equation was solved

Introduction

Probability Patterns ▪ Dots represent position of electron at different points in time ▪ Electron spending more time near nucleus than anywhere else ▪ Boundary of atom placed at 90% of probability

Probability Patterns ▪ No actual boundary in atom ▪ Simple for first electron in atom ▪ More complicated atoms = more complicated probability plots

Probability Patterns

The Principal Quantum Number ▪ Quantum numbers solutions to Schrodinger’s equation ▪ Completely describe energy of electron ▪ No two electrons same four quantum numbers – Pauli exclusion principle (Wolfgang Pauli)

The Principal Quantum Number ▪ Number of Sub-levels and Electrons by Principal Quantum Number ▪ Principal quantum number positive integer that indicates main energy level within atom ▪ Sub-levels within every principle quantum number ▪ Principal number equal to number of sub-levels within energy level Principal Quantum Number Number of Sub-Levels Total Number of Electrons

The Principal Quantum Number ▪ Largest known atom just over 100 electrons ▪ 7 principal energy levels in known atoms ▪ Sub-levels identified by letters s, p, d, f, g, h, i ▪ Only currently described for four energy levels

Orbitals ▪ Defined in quantum mechanics as area in electron cloud where probability of finding electron high ▪ Number of orbitals in energy level = square of principal quantum number

Orbitals Principal Energy Level (n) Number of Orbitals Present S p d f Total Number of Orbitals (n 2 ) Maximum Number of Electrons (2n 2 ) Relationship between n (principal quantum number), number of orbitals, and maximum number of electrons in principal energy level

Orbitals ▪ Each orbital probability pattern determined by intepreting Schrodinger’s equation ▪ Each shape representative of single orbital ▪ Probability pattern result of various positions of electrons

Orbitals