Bohr Model of Atom: electrons move around nucleus in orbits similar to how planets orbit the sun energy levels for electrons are quantized
|
|
|
- Estella Alaina Ford
- 5 years ago
- Views:
Transcription
1 Chemistry I: Quantum Mechanics Notes Bohr Model of Atom: electrons move around nucleus in orbits similar to how planets orbit the sun energy levels for electrons are quantized Major developments that put Bohr s Model into question: Einstein: Light energy exhibits properties of matter. Matter and energy are different forms of the same thing. De Broglie: Electrons move around nucleus in waves. Heisenberg: Uncertainty Principle: it is impossible to measure the momentum (velocity) and location of an electron at the same time. Max Born: Interpreted an equation discovered by Schrodinger to mean that although we cannot predict the exact location and path of an electron, we can describe its path in terms of probability. This is the fundamental concept behind Quantum Mechanics. Bohr Model of Atom: Quantum Mechanical Model of Atom: How is Quantum mechanics similar to Bohr Model? 1. There are quantized energy levels. 2. Electrons jump from level to level when excited. How is Quantum Mechanics different from Bohr Model? 1. We can describe an electron s path in terms of probability, not precise orbits. 2. Each energy level (shell) is divided into sublevels (subshells). 3. Each sublevel is made up of 1 or more orbital. 4. Each subshell corresponds to a different shape of the orbital. (Not always spherical!)
2 Electron Configuration Notes Important: As you increase in atomic number, each atom adds a new electron: Every successive element has the same electron configuration as the previous element, plus the additional electron. (Some exceptions) The energy level (shell) of this electron is described by the row where the atom is on the periodic table. (Exceptions (which won t make sense to you now, but they will someday): d subshell is always 1 level behind; f subshell is always 2 levels behind.) The sublevel (subshell) of this electron is described by the group of columns where the atom is on the periodic table. Energy Levels are represented by numbers: 1, 2, 3, 4 Subshells are represented by letters: s, p, d, f Examples: H: Si: He: P: Li: S: Be: Cl: B: Ar: C: K: N: Ca: O: Sc: F: Ti: Ne: Zn: Na: Ga: Mg: Kr: Al:
3 Orbital Notes Remember how each energy level is divided into subshells? Subshells are also divided! Subshells are divided into orbitals. Each orbital contains 2 electrons. (of opposite spins) So, in summary: are divided into, which are divided into, each of which contains. Each type of subshell contains a certain number of orbitals: subshell # of orbitals # of electrons s p d f Hund s Rule: When filling a subshell, electrons enter each orbital until all orbitals contain one electron with their spins parallel. ORBITAL BOX DIAGRAM. This uses a little circle, O, to represent each orbital. We group the orbitals of a subshell together, and label them. An orbital with no electrons in it (an empty house ) is left as a circle: O. With one electron we put a diagonal line in to show one electron in the orbital. The line can slant either way; one way, it's spinning one direction, the other slant represents an electron spinning the other way; or Ø. Two electrons in an orbital need both diagonal lines. Let's take an example; Na, sodium, element #11. Electron Configuration: 1s 2 2s 2 2p 6 3s 1 Its orbital box diagram looks like this: 1s 2s 2p 3s Ø Do other examples!
4 Probability Diagram Notes Most of the orbitals for a particular subshell are shaped the same: subshell shape s p d f Draw probability diagrams for Na and Mg: Bonding Electrons (also called valence electrons): Electrons involved in bonding The electrons in the s and p subshells of the highest energy level. Examples: How many bonding electrons are there Na? Mg? Lewis Dot diagrams : Represent the bonding electrons
5 Stability Rule: atoms/ions are stable when ½ of a subshell is filled atoms/ions are even more stable when a subshell is entirely filled atoms/ions are the most stable when the valence shell (valence electrons) are entirely filled (Octet Rule) Examples of atoms with unusual electron configurations: Cr Zn More Examples: Use electron configuration and orbital box diagrams to explain why: Noble gases like Kr do not form ions Nitride is a 3- ion Sulfide is a 2- ion Iodide is a 1- ion Potassium is a 1+ ion Magnesium is a 2+ ion Aluminum is a 3+ ion
ELECTRONIC STRUCTURE OF ATOMS
ELECTRONIC STRUCTURE OF ATOMS Electron Spin The electron: spins around its own axis acts as an tiny magnet (any moving electrical charge creates a magnetic field around itself) can spin in either of 2
The orbitals in an atom are arranged in shells and subshells. orbital 3s 3p 3d. Shell: all orbitals with the same value of n.
Shells and Subshells The orbitals in an atom are arranged in shells and subshells. n=3 orbital 3s 3p 3d Shell: all orbitals with the same value of n n=3 3s 3p 3d Subshell: all orbitals with the same value
4.2 WHERE are the electrons in the { atom???? QUANTUM NUMBERS
4.2 WHERE are the electrons in the { atom???? QUANTUM NUMBERS Bohr s Model Contradicts Common Sense If only certain orbits with definite energies are allowed and the electrons constantly gives off radiation,
LIMITATIONS OF RUTHERFORD S ATOMIC MODEL
ELECTRONS IN ATOMS LIMITATIONS OF RUTHERFORD S ATOMIC MODEL Did not explain the chemical properties of atoms For example, it could not explain why metals or compounds of metals give off characteristic
LABELING ELECTRONS IN ATOMS
Date: Name: LABELING ELECTRONS IN ATOMS The location of each electron in an atom is determined by a few different factors. Each factor is represented by a QUANTUM NUMBER. Prediction: What do you think
Atoms, Electrons and Light MS. MOORE CHEMISTRY
Atoms, Electrons and Light MS. MOORE CHEMISTRY Atoms Remember Rutherford??? What did he discover with his gold foil experiment. A: Atoms contain a dense nucleus where the protons and neutrons reside. ATOMS
Chem I - Wed, 9/16/15
Chem I - Wed, 9/16/15 Do Now Complete the back of worksheet 4.5 Homework Pennium Lab if not Finished E- Config POGIL Agenda Return Papers Wks 4.5 Pennium Lab Electron Config Chapter 5 Quantum Theory and
Quantum Theory and Electron Configurations
Chapter 5 Chapter 5 Quantum Theory and Electron Configurations It s all about color In terms of atomic models, so far: Dalton (1803) = Tiny, solid particle Thomson (1897) = Plum Pudding model Electrons
Unit Two: Elements & Matter. February 1, 2016
Unit Two: Elements & Matter February 1, 2016 Warm-Up: 2/1/2016 1. Fill in the following information: Atomic Symbol Ca 2+ Atomic Number Proton Neutron Electron 34 36 Mass Num. 2. Identify which family the
8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37
Electronic Structure Worksheet 1 Given the following list of atomic and ionic species, find the appropriate match for questions 1-4. (A) Fe 2+ (B) Cl (C) K + (D) Cs (E) Hg + 1. Has the electron configuration:
Electron Configuration
Electron Configuration Electrons as Waves Review Louis de Broglie (1924) Applied wave-particle theory to electrons ELECTRONS EXHIBIT WAVE PROPERTIES Louis de Broglie ~1924 QUANTIZED WAVELENGTHS 200 Fundamental
Chapter 3: Electron Structure and the Periodic Law
Chapter 3: Electron Structure and the Periodic Law PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form the statement is:
Quantum Theory & Electronic Structure of Atoms. It s Unreal!! Check your intuition at the door.
Quantum Theory & Electronic Structure of Atoms It s Unreal!! Check your intuition at the door. 1 Quantum Theory of the Atom Description of the atom and subatomic particles. We will focus on the electronic
Particle Behavior of Light 1. Calculate the energy of a photon, mole of photons 2. Find binding energy of an electron (know KE) 3. What is a quanta?
Properties of Electromagnetic Radiation 1. What is spectroscopy, a continuous spectrum, a line spectrum, differences and similarities 2. Relationship of wavelength to frequency, relationship of E to λ
Provide a short and specific definition in YOUR OWN WORDS. Do not use the definition from the book. Electromagnetic Radiation
Name: Provide a short and specific definition in YOUR OWN WORDS. Do not use the definition from the book Additional Notes: Electromagnetic Radiation Electromagnetic Spectrum Wavelength Frequency Photoelectric
Chapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
Where are the s, p, d, f orbitals located on the periodic table? Identify them on the diagram below.
Chapter 4 Arrangement of Electrons in Atoms Section 3: Electron Configuration Objectives: Be able to define: Aufbau Principle, Pauli Exclusion Principle, Hund s rule. Be able to list the number of electrons
CHAPTER 5. Electrons in Atoms. Rutherford Model. Bohr Model. Plum Pudding Model. 5.1 Atomic Models
CHAPTER 5 Electrons in Atoms 5.1 Atomic Models The Chemical properties of atoms, ions, and molecules are related to the arrangement of the electrons within them. The first model of the atom was Dalton
Creating Energy-Level Diagrams Aufbau (building up) Principle Electrons are added to the lowest energy orbital available.
3.6 Atomic Structure and the Periodic Table Bohr's Theory Was Incorrect Because... Only explained the line spectrum of hydrogen Position and motion of an e cannot be specified (since the e is so small,
Electron Configurations
Electron Configurations Electron Arrangement in an Atom The arrangement of electrons in an atom is its electron configuration. It is impossible to know where an electron is or how fast it is traveling
Development of the Periodic Table. Chapter 5. Light and the EM Spectrum. Light
Chapter 5 Periodic Table Song Periodicity and Atomic Structure Development of the Periodic Table Mid-1800 s, several scientists placed known elements in order based on different criteria. Mendeleev s and
- Light has properties of WAVES such as DIFFRACTION (it bends around small obstructions).
170 LIGHT wavelength Diffraction frequency = wavelengths / time = - Light has properties of WAVES such as DIFFRACTION (it bends around small obstructions). - Einstein noted that viewing light as a particle
Name Chemistry-PAP Period. Notes: Electrons. Light travels through space as a wave. Waves have three primary characteristics:
Name Chemistry-PAP Period The Wave Nature of Light Notes: Electrons Light travels through space as a wave. Waves have three primary characteristics: Wavelength (λ): the distance between 2 consecutive crests
ELECTRON CONFIGURATIONS... WHY BOHR RUTHERFORD DIAGRAMS JUST WON T CUT IT ANYMORE!
ELECTRON CONFIGURATIONS... WHY BOHR RUTHERFORD DIAGRAMS JUST WON T CUT IT ANYMORE! REPRESENTING ELECTRONS... Now that you know what an orbital is, you need to be able to use that to describe the electronic
-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
175 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
2 e. 14 e. # e # orbitals. 10 e 5. sublevel. shape of orbital. Orbital Shapes. Notes Orbital Notation; e Config; NGN.
How to build an atom: The bigger (more massive) the atom, the more protons (and neutrons) The bigger the atom, the more electrons Electrons fill lower energy levels first "Aufbau" Principle ("To build
Chapter 6 Part 3; Many-electron atoms
Chapter 6 Part 3; Many-electron atoms Read: BLB 6.7 6.9 HW: BLB 6:59,63,64,67,71b-d,74,75,90,97; Packet 6:10 14 Know: s & atoms with many electrons Spin quantum number m s o Pauli exclusion principle o
Mendeleev s Periodic Law
Mendeleev s Periodic Law Periodic Law When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically. Mendeleev s Periodic Law allows us to predict what
General Rules. Pauli Exclusion Principle. Each orbital can hold TWO electrons with opposite spins. Wolfgang Pauli
General Rules Pauli Exclusion Principle Each orbital can hold TWO electrons with opposite spins. Wolfgang Pauli General Rules Aufbau Principle Electrons fill the lowest energy orbitals first. Lazy Tenant
5.1 Light & Quantized Energy
5.1 Light & Quantized Energy Objectives: 1. Describe electromagnetic (EM) wave properties & measures 2. Relate visible light to areas of the EM spectrum with higher & lower energy 3. Know the relationship
The Periodic Table & Electronic Structure
Periodic Table The Periodic Table & Electronic Structure Is there an overall reason that the elements are arranged in the order that they are? Yes! We ve seen that the elements are arranged in order of
Chapter 11. What subatomic particles do you get to play with? Protons Neutrons Eletrons
Chapter 11 What subatomic particles do you get to play with? Protons Neutrons Eletrons changes the element isotopes: only mass is different what we play with in chemistry Bohr Model of the Atom electrons
AP Chemistry - Problem Drill 10: Atomic Structures and Electron Configuration
AP Chemistry - Problem Drill 10: Atomic Structures and Electron Configuration No. 1 of 10 Instructions: (1) Read the problem statement and answer choices carefully (2) Work the problems on paper as 1.
Quantum Model & Configurations
Quantum Model & Configurations Bohr s Energy Levels: Bohr was able to tell us the electrons are found in layers around the nucleus based on the following: Each element gives off a unique emission spectrum
Chemistry- Unit 3. Section II - Chapter 7 ( , 7.11) Quantum Mechanics
Chemistry- Unit 3 Section II - Chapter 7 (7.6-7.8, 7.11) Quantum Mechanics Atomic Review What subatomic particles do you get to play with? Protons Neutrons Electrons NO! It would change the element Don
- Why are phase labels required? Because phase changes either absorb or release energy. ... what does this mean?
157 SINCE the enthalpy change does NOT depend on path, this means that we can use standard values for enthalpy to predict the heat change in reactions that we have not tested in a calorimeter. THERMOCHEMICAL
Electrons and Periodic Behavior. Cartoon courtesy of NearingZero.net
Electrons and Periodic Behavior Cartoon courtesy of NearingZero.net Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel
Notes: Unit 6 Electron Configuration and the Periodic Table
Name KEY Block Notes: Unit 6 Electron Configuration and the Periodic Table In the 1790's Antoine Lavoisier compiled a list of the known elements at that time. There were only 23 elements. By the 1870's
Electronic Structure of Atoms and the Periodic table. Electron Spin Quantum # m s
Electronic Structure of Atoms and the Periodic table Chapter 6 & 7, Part 3 October 26 th, 2004 Homework session Wednesday 3:00 5:00 Electron Spin Quantum # m s Each electron is assigned a spinning motion
2.12 Electronic Structure
2.12 Electronic Structure In this chapter we are going to look at electronic structure in atoms. This is actuall a ver comple area of chemistr because it is ver hard, if not impossible, to describe the
Starter # (1) Why was Rutherford s model not good enough and need to be modified by scientists?
1. (1) Why was Rutherford s model not good enough and need to be modified by scientists? It could not explain or predict any chemical behavior of any elements 2. (1) What is one of the only things that
The Electronic Theory of Chemistry
JF Chemistry CH1101 The Electronic Theory of Chemistry Dr. Baker bakerrj@tcd.ie Module Aims: To provide an introduction to the fundamental concepts of theoretical and practical chemistry, including concepts
Electron Configurations
Section 3 Electron Configurations Key Terms electron configuration Pauli exclusion principle noble gas Aufbau principle Hund s rule noble-gas configuration Main Ideas Electrons fill in the lowest-energy
CDO AP Chemistry Unit 5
1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic
1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions
Pre-AP Chemistry 11 Atomic Theory II Name: Date: Block: 1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions Electronic
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY Note: For all questions referring to solutions, assume that the solvent is water unless otherwise stated. 1. The nuclide is radioactive and decays by the
CHAPTER 5 Electrons in Atoms
CHAPTER 5 Electrons in Atoms 5.1 Light & Quantized Energy Was the Nuclear Atomic model incomplete? To most scientists, the answer was yes. The arrangement of electrons was not determined > Remember...the
Chapter 5. Periodicity and the Electronic Structure of Atoms
Chapter 5 Periodicity and the Electronic Structure of Atoms Electron Spin experiments by Stern and Gerlach showed a beam of silver atoms is split in two by a magnetic field the experiment reveals that
-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
170 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
Chapter 3: Electron Structure and the Periodic Law
PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form the statement is: Elements with similar chemical properties occur at
Name: Unit 3 Guide-Electrons In Atoms
Name: Unit 3 Guide-Electrons In Atoms Importance of Electrons Draw a complete Bohr model of the atom. Write an element s electron configuration. Know how the symbols used in ECs relate to electron properties
ELEMENTS & MATTER. September 7, 2016
ELEMENTS & MATTER September 7, 2016 Review Problems: 9/7/2016 1. Fill in the following information: Atomic Symbol Atomic Number Proton Neutron Electron Mass Num. Atomic Mass 34 36 Ca 2+ 2. Identify which
UNIT 2 PART 1: ELECTRONS
UNIT 2 PART 1: ELECTRONS Electrons in an Atom Bohr s Model: Electrons resided in an allowed orbit. Quantum Mechanics Model: Probability of finding an electron in an area around the nucleus. This area around
CHEMISTRY 113 EXAM 3(A)
Summer 2003 CHEMISTRY 113 EXAM 3(A) 1. Specify radiation with the greatest energy from the following list: A. ultraviolet B. gamma C. infrared D. radio waves 2. The photoelectric effect is: A. reflection
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE What Makes Red Light Red? (4.1) Electromagnetic Radiation: energy that travels in waves (light) Waves Amplitude: height
Modern Atomic Theory. (a.k.a. the electron chapter!) Chemistry 1: Chapters 5, 6, and 7 Chemistry 1 Honors: Chapter 11
Modern Atomic Theory (a.k.a. the electron chapter!) 1 Chemistry 1: Chapters 5, 6, and 7 Chemistry 1 Honors: Chapter 11 ELECTROMAGNETIC RADIATION 2 Electromagnetic radiation. 3 4 Electromagnetic Radiation
The structure of the atom
The structure of the atom 1.Rutherford s model of the atom 2. Quantum-mechanics model of the atom The wave nature of microparticles motion The electron cloud The quantum numbers 1. Rutherford s model of
Model 1: Orbitals. 1. What is an atomic orbital? What are the four different orbitals?
Name: Date: Period: POGIL: Electron Configuration and Orbitals Model 1: Orbitals The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron
Chapter 4. Table of Contents. Section 1 The Development of a New Atomic Model. Section 2 The Quantum Model of the Atom
Arrangement of Electrons in Atoms Table of Contents Section 1 The Development of a New Atomic Model Section 2 The Quantum Model of the Atom Section 3 Electron Configurations Section 1 The Development of
Unit 3: The Periodic Table and Atomic Theory
Name: Period: Unit 3: The Periodic Table and Atomic Theory Day Page # Description IC/HW 1 2-3 Periodic Table and Quantum Model Notes IC 1 4-5 Orbital Diagrams Notes IC 1 14 3-A: Orbital Diagrams Worksheet
Topic 2 Atomic Structure. IB Chemistry SL Coral Gables Senior High School Ms. Kiely
Topic 2 Atomic Structure IB Chemistry SL Coral Gables Senior High School Ms. Kiely Bell Ringer (i) Calculate the number of neutrons and electrons in one atom of ⁶⁵Cu. (ii) State one difference in the physical
Unit 7. Atomic Structure
Unit 7. Atomic Structure Upon successful completion of this unit, the students should be able to: 7.1 List the eight regions of the electromagnetic spectrum in the designated order and perform calculations
Electrons! Chapter 5, Part 2
Electrons! Chapter 5, Part 2 3. Contained within sublevels are orbitals: pairs of electrons each having a different space or region they occupy a. Each sublevel contains certain orbitals: i. s sublevel
Arrangement of Electrons in Atoms
CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. In what way does the photoelectric effect support the particle theory
The element having chemical properties most similar to As is. The properties of the elements are determined by the arrangement of in their atoms.
Group 17 (7A) Halogens - Colorful and corrosive nonmetals - Found in nature only in with other elements, such as with sodium in table salt (sodium chloride, NaCl) - All except At are as pure elements.
heat of formation of carbon dioxide
163 FORMATION REACTIONS - A reaction that forms exactly one mole of the specified substance from its elements at their STANDARD STATE at 25C and 1 atm pressure. heat of formation of carbon dioxide you
Chemistry 101 Chapter 11 Modern Atomic Theory
Chemistry 101 Chapter 11 Modern Atomic Theory Electromagnetic radiation: energy can be transmitted from one place to another by lightmore properly called electromagnetic radiation. Many kinds of electromagnetic
AP Chapter 6 Study Questions
Class: Date: AP Chapter 6 Study Questions True/False Indicate whether the statement is true or false. 1. The wavelength of radio waves can be longer than a football field. 2. Black body radiation is the
Topic 12: Quantum numbers. Heisenberg, Schrodinger, Quantum Theory, Quantum numbers, Practice
Topic 12: Quantum numbers Heisenberg, Schrodinger, Quantum Theory, Quantum numbers, Practice Quantum Mechanics We left off by saying Bohr s model only explained the electron arrangement of Hydrogen...
Worksheet #1: Atomic Spectra Answer the following questions using your Unit 3 notes.
Worksheet #1: Atomic Spectra 1. How did Bohr expand on Rutherford s model of the atom? 2. Compare the energy of an electron in the ground state and an electron in the excited state. 3. When an electron
Quantum Mechanics/Trends Lab
NAME Quantum Mechanics/Trends Lab Quantum mechanics: The electron orbit model (Bohr Model) that was proposed for hydrogen, does not work for any other atom. This model does give us the idea of quantization:
protons electrons neutrons nucleus Center of the atom; contains protons and neutrons. The Atom Molecules are made up of two or more atoms.
_ Period: The Atom Ch. 18:1 Everything is made of atoms. Atoms are the smallest part of matter. Atoms are made up of 3 subatomic particles (particles smaller than the atom): electrons, protons, and neutrons.
Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation.
Preview Objectives Properties of Light Wavelength and Frequency The Photoelectric Effect The Hydrogen-Atom Line-Emission Spectrum Bohr Model of the Hydrogen Atom Photon Emission and Absorption Section
A.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity
A.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity 1) Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is MHz. A) 50 B) 20 C)
E J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
Chapter 4 Section 2 Notes
Chapter 4 Section 2 Notes Vocabulary Heisenberg Uncertainty Principle- states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. Quantum
Electron Arrangement - Part 2
Brad Collins Electron Arrangement - Part 2 Chapter 9 Some images Copyright The McGraw-Hill Companies, Inc. Review Energy Levels Multi-electron 4d 4d 4d 4d 4d n = 4 4s 4p 4p 4p 3d 3d 3d 3d 3d n=3, l = 2
1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a.
CHEMISTRY 123-07 Midterm #3 solution key December 02, 2010 Statistics: Average: 77 p (77%); Highest: 100 p (100%); Lowest: 33 p (33%) Number of students performing at or above average: 54 (52%) Number
Chapter 7. Characteristics of Atoms. 7.1 Electromagnetic Radiation. Chapter 7 1. The Quantum Mechanical Atom. Atoms: How do we study atoms?
Chapter 7 The Quantum Mechanical Atom 1 Characteristics of Atoms Atoms: possess mass contain positive nuclei contain electrons occupy volume have various properties attract one another combine to form
Unit 3: Electron configuration and periodicity
Unit 3: Electron configuration and periodicity Group 1 BOHR MODELS Group 18 H Group 2 Group 13 Group 14 Group 15 Group 16 Group 17 He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca His theory couldn t
Professor K. Section 8 Electron Configuration Periodic Table
Professor K Section 8 Electron Configuration Periodic Table Schrödinger Cannot be solved for multielectron atoms We must assume the orbitals are all hydrogen-like Differences In the H atom, all subshells
Electronic configuration
Electronic configuration The energy of electrons The electrons of an atom all have the same charge and the same mass, but each electron has a different amount of energy. Electrons that have the lowest
Atomic Structure Chapter 4 Mr. Hines
Atomic Structure Chapter 4 Mr. Hines Part A Standard model of the atom Learning Targets and I can statements 1 List, label, and describe the parts of an atom. 2 Identify the atomic number and the atomic
2) The energy of a photon of light is proportional to its frequency and proportional to its wavelength.
Advanced Chemistry Chapter 13 Review Name Per Show all work Wave Properties 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c 2) The energy of a photon of
9/13/2011. The Greek Philosophers. Atomic Structure & The Periodic Table. Dalton s Atomic Theory. J. J. Thomson. Thomson s Experiment
Atomic Structure & The Periodic Table The Greek Philosophers Democritus believed that all matter is made up of tiny particles that could not be divided Aristotle -- thought that matter was made of only
Atomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons?
Name Chemistry Atomic Structure Essential Question: How was the structure of the atom determined? Vocabulary: bright-line spectrum electron configuration excited state ground state orbital wave-mechanical
1.1 Atomic Structure Details of the three Sub-atomic (fundamental) Particles
1.1 Atomic Structure Details of the three Sub-atomic (fundamental) Particles Particle Position Relative Mass Relative Charge Proton Nucleus 1 +1 Neutron Nucleus 1 0 Electron Orbitals 1/1800-1 An atom of
Chapter 2 Atoms and Elements. Electromagnetic Radiation. Electromagnetic Spectrum. Electron Energy Levels. 2.6 Electron Energy Levels
Chapter 2 Atoms and Elements Electromagnetic Radiation 2.6 Electron Energy Levels Electromagnetic radiation Consists of energy particles called photons that travel as waves. Includes low energy particles
Exam 2 Practice Problems (Key) 1. An electron has an n value of 3. What are the possible l values? What are the possible m l values?
Exam 2 Practice Problems (Key) 1. An electron has an n value of 3. What are the possible l values? What are the possible m l values? l = 0, 1, 2 m l = 0 (for s) m l = 1, 0, +1 (for p) m l = 2, 1, 0, +1,
Electron Configurations: Assigning each electron in an atom to the energy level and sublevel it occupies in the atom. Number of Electrons
First some terms and more information about the structure of the atom: 1) Energy level is no longer an orbit but more like a boundary or maximum distance from the nucleus that electrons occupy. 1, 2, 3
CHAPTER 4 Arrangement of Electrons in Atoms
CHAPTER 4 Arrangement of Electrons in Atoms SECTION 1 The Development of a New Atomic Model OBJECTIVES 1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic
Quantum Electron Model Chapter 5 Mr. Hines
Quantum Electron Model Chapter 5 Mr. Hines Part A - INTRODUCTION TO THE QUANTUM ELECTRON MODEL 1 Recall basic knowledge from chapter 4 energy levels, valence electrons, periods, and groups 2 Describe atoms
When I lecture we will add more info, so leave spaces in your notes
Title and Highlight Topic: EQ: Date Reflect Question: Reflect on the material by asking a question (its not suppose to be answered from notes) NOTES: Write out the notes from my website. Use different
CHAPTER 4 10/11/2016. Properties of Light. Anatomy of a Wave. Components of a Wave. Components of a Wave
Properties of Light CHAPTER 4 Light is a form of Electromagnetic Radiation Electromagnetic Radiation (EMR) Form of energy that exhibits wavelike behavior and travels at the speed of light. Together, all
Chapter 8. Periodic Properties of the Elements
Chapter 8 Periodic Properties of the Elements Mendeleev (1834 1907) Ordered elements by atomic mass. Saw a repeating pattern of properties. Periodic Law When the elements are arranged in order of increasing
Modern Atomic Theory and the Periodic Table
Modern Atomic Theory and the Periodic Table Chapter 10 the exam would have to be given earlier Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons,
Atomic Theory. H. Cannon, C. Clapper and T. Guillot Klein High School
Atomic Theory Unit 3 Development of the Atomic Theory 1. Where is the mass of the atom concentrated? 2. What is located in the nucleus? 3. What is the negative particle that orbits the nucleus? 4. What
Objectives: Learn how to show Electron configuration using:
4 WAYS to SHOW the Electron Configuration(Electron arrangement) Objectives: Learn how to show Electron configuration using: 1. Using Aufbau Energy Diagrams 2. Orbital Diagrams 3. Long hand Electron configuration
Molecular structure and bonding
Molecular structure and bonding To understand the formation and structure of molecular compounds, first one has to learn, recognize, use, count, take into account: the periodic table with groups and periods,
Unit 8: Atomic Theory. Quantum Mechanics
Unit 8: Atomic Theory Quantum Mechanics 1 Unit 8: Atomic Theory 1. Historical Views of the Atom 2. The 'New' Look Atom 3. Electron Configurations 4. Electron Configurations & the Periodic Table 5. Quantum