Quantum Numbers and Electronic Configuration.
|
|
|
- Rose Lynch
- 5 years ago
- Views:
Transcription
1 Quantum Numbers and Electronic Configuration. F Scullion: 1 Each electron has a set of four numbers, called quantum numbers, that specify it completely; no two electrons in the same atom can have the same four. That is essentially the Pauli Exclusion Principle. 1. The Principal Quantum Number. Given the symbol n. This denotes the energy level (shell). This has integer values 1, 2, The Angular Momentum Quantum Number. Given the symbol l It denotes the number of sub-levels (orbitals) in each energy level and the shape of these orbitals. The number of orbitals in any level = the number of the energy level. The number of electrons in any level is found by the formula: No. of electrons = 2n 2 where n is the principle quantum number (energy level) Energy level (Value of n) Number of Subshells Maximum Number of Electrons = 2n 2 s orbital Spherical p orbital Dumbell d orbital Cloverleaf F orbital Complex
2 3. The Magnetic Quantum Number. Given the symbol m. 2 This defines the number of atomic orbitals making up a sublevel. Sublevel Number of Atomic Orbitals s 1 p 3 d 5 f 7 It also describe their orientation in space. s orbital P orbital p x p y p z Each atomic orbital can hold 0, 1 or 2 electrons. 4. The Spin Quantum Number. Given the symbol s. This describes the spin of the electron in the atomic orbital. There are just 2 possible spins: clockwise and counterclockwise. Sample p orbitals Parallel spins Hund's rule: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
3 The Aufbau (building up) Principle for Electronic Configuration. 3 In the so-called ground state of an atom the electronic configuration generally follows this principle. According to this principle, electrons enter into states in order of the states increasing energy. Electrons are reluctant to pair up with another in the same atomic orbital (due to repulsions) and to go to a higher energy level than is necessary. When faced with the need to do one or other, they generally settle for pairing up with opposite spins, rather than go into the next highest energy level. Complete for Oxygen (8) Complete for Sodium (11) Exceptions to this rule include Chromium (4s 1 3d 5 ) and Copper (4s 1 3d 10 ) These result because it requires less energy to maintain an electron in a half-filled or filled d sublevel than paired in the s sublevel below. s p d and f block elements Assigned according to the oribtal getting the final electron. Colour in the chart below to show each of these blocks.
4 Complete the diagrams to show the normal electronic configurations of the elements indicated. Hydrogen (1) Helium (2) Lithium (3) 4 Beryllium (4) Boron (5) Carbon (6) Nitrogen (7) Oxygen (8) Fluorine (9) Neon (10) Sodium (11) Magnesium (12)
5 Aluminium (13) Silicon (14) Phosphorus (15) 5 Sulphur (16) Chlorine (17) Argon (18) Potassium (19) Calcium (20) Scandium (21) Chromium (24) Copper (29) Bromine (35)
6 A brief look at examples of hybridization. (This is beyond the syllabus, but helpful to know.) 6 Phosphorus (15) Ground State Hybrid State Move one of the paired 3s electrons up to one of the empty 3d orbitals There are 3 unpaired electrons giving a valency of 3, which would explain the existence PF 3 for example. The phosphorus is surrounded by 8 electrons in this molecule. This is known as a completed octet. There are 5 unpaired electrons giving a valency of 5, which would explain the existence PF 5 for example. The phosphorus is surrounded by 10 electrons in this molecule. This is known as an expanded octet. Shape of PF 5 : Trigonal Bipyramid Bonding
7 Sulphur (16) 7 Ground State Hybrid State Move one of the paired 3s electrons up to one of the empty 3d orbitals. Do the same with one of the pair in the 3p x atomic orbital. There are 2 unpaired electrons giving a valency of 2, which would explain the existence H 2 S for example. The sulphur is surrounded by 8 electrons in this molecule. This is known as a completed octet. There are 6 unpaired electrons giving a valency of 6, which would explain the existence SF 6 for example. The phosphorus is surrounded by 12 electrons in this molecule. This is known as an expanded octet. Shape of SF 6 : Octahedral Bonding
8 Now you are ready to move on to the next topic: 8 The Origin of Atomic Spectra - Atomic Absorption and Emission. When aquainted with the circumstances in which electrons can jump up and down between energy levels in an atom, you should be able to understand the origin of Atomic Spectra. An atomic line spectrum. The electrons jumps that we will learn about The Balmer Series in particular F Scullion.
#9 Modern Atomic Theory Quantitative Chemistry
Name #9 Modern Atomic Theory Quantitative Chemistry Student Learning Map Unit EQ: What is the current model of the atom? Key Learning: The current model of the atom is based on the quantum mechanical model.
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
[3.3] Energy Level Diagrams and Configurations
![[3.3] Energy Level Diagrams and Configurations](/thumbs/87/96003907.jpg "[3.3] Energy Level Diagrams and Configurations")
[3.3] Energy Level Diagrams and Configurations 1 Energy Level Diagrams Energy level diagrams are used to represent the electron arrangement in an atom 2 Pauli s Exclusion Principle No two electrons have
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
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
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
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
Electronic configurations, Auf-bau principle, Pauli principle, Hunds rule 1. Which of the following statements in relation to the hydrogen atom is correct? 1) 3s and 3p orbitals are of lower energy than
6.4 Electronic Structure of Atoms (Electron Configurations)
Chapter 6 Electronic Structure and Periodic Properties of Elements 317 Orbital n l m l degeneracy Radial nodes (no.) 4f 4 3 7 0 4p 4 1 3 2 7f 7 3 7 3 5d 5 2 5 2 Check Your Learning How many orbitals have
HL Chemistry Topic 12 Atomic Structure
Define: ionization energy - 1 - Trends in Ionization Energy in the Periodic Table Why do these trends in ionization energy occur? Background information: Understand the concept of effective nuclear charge
Consider the two waves shown in the diagram below.
The way matter interacts with electromagnetic radiation gives a great deal of information about the electronic structure of atoms. In this section we will look at the electromagnetic spectrum and then
Use the Venn Diagram to compare and contrast the Bohr Model of the atom with the Quantum Mechanical Model of atom
Use the Venn Diagram to compare and contrast the Bohr Model of the atom with the Quantum Mechanical Model of atom Bohr Model Quantum Model Energy level Atomic orbital Quantum Atomic number Quantum mechanical
Chapter 5 Electrons In Atoms
Chapter 5 Electrons In Atoms 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 Copyright Pearson Education, Inc., or its affiliates.
Electron Configuration
Electron Configuration Orbitals Remember that orbitals simply represent an area where the electron is most likely to be found. Formally, orbitals are defined using four quantum numbers Orbitals have particular
Section 3 Electron Configurations. Chapter 4. Preview
Preview Lesson Starter Objectives Electron Configurations Rules Governing Electron Configurations Representing Electron Configurations Elements of the Second Period Elements of the Third Period Elements
Student Exploration: Electron Configuration
Name: Date: Student Exploration: Electron Configuration Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund s rule, orbital, Pauli exclusion
Unit 4B- Electron Configuration- Guided Notes
Unit 4B- Electron Configuration- Guided Notes Atomic Structure Electrons are arranged in or around the nucleus of an atom o First shell can hold a maximum of electrons o Second shell can hold a maximum
Unit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
Advanced Theories of Atomic Structure: Atomic Orbitals
Advanced Theories of Atomic Structure: Atomic Orbitals What are the more advanced theories of atomic structure? Richard Feynman, 1918 1988. Winner of the 1965 Nobel Prize in Physics. The modern scientific
An Electron s Address: Orbital Diagrams and Electron Configuration
AP Chemistry Ms. Ye Name Date Block An Electron s Address: Orbital Diagrams and Electron Configuration Information: Energy Levels and Sublevels As you know, in his solar system model Bohr proposed that
An Electron s Address
Honors Chemistry Name Date Block An Electron s Address Information: Energy Levels and Sublevels As you know, in his solar system model Bohr proposed that electrons are located in energy levels. The current
Questions: Use the information above to answer the following questions 1. How many sublevels exist in the 1 st energy level?
Honors Chemistry Ms. Ye Name Date Block An Electron s Address Information: Energy Levels and Sublevels As you know, in his solar system model Bohr proposed that electrons are located in energy levels.
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
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,
= proton (positive charge) = electron (negative charge) = neutron (no charge) A Z. ,, and are notations that represent isotopes of carbon.
ChemQuest 8 Name: Date: Hour: Information: Structure of the Atom Note the following symbols: (they are not to scale) = proton (positive charge) = electron (negative charge) = neutron (no charge) The following
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
Orbital Diagram Rules: 1. The Aufbau Principle: Under normal condition, each electron occupies the
Honors Chemistry Ms. Ye Name Date Block Orbital Diagram Rules: 1. The Aufbau Principle: Under normal condition, each electron occupies the 2. The Pauli Exclusion Principle: a maximum of can occupy an orbital
Electron Configurations
Why? Electron Configurations What is the electron structure in an atom? The electron structure of an atom is very important. Scientists use the electronic structure of atoms to predict bonding in molecules,
General Chemistry 1 CHM201 Unit 4 Practice Test. 4. What is the orbital designation for an electron with the quantum numbers n 4, 3?
General Chemistry 1 CHM201 Unit 4 Practice Test 1. An orbital s orientation in space is determined by a. the quantum number. d. the n quantum number. b. the m l quantum number. e. both the and m l quantum
Electron Configurations
Why? Electron Configurations What is the electron structure in an atom? The electron structure of an atom is very important. Scientists use the electronic structure of atoms to predict bonding in molecules,
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
UNIT 1 ATOMIC STRUCTURE NOTES #4
CH40S UNIT 1 ATOMIC STRUCTURE NOTES #4 Name H O W E L E C T R O N S A R E A R R A N G E D I N A T O M S The arrangement of electrons among the orbitals of an atom is called the electron configuration of
Early Chemistry. Early Chemists only believed in 1 element: Dirt. Later Chemists believed in 4 elements:
Early Chemistry Early Chemists only believed in 1 element: Dirt Later Chemists believed in 4 elements: Air Earth Fire Water Various combinations of these produced various compounds Atomic Structure All
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:
5.2 Electron Arrangement in Atoms > Happy Thursday!
Happy Thursday! Please take out your homework problems for me to check for a grade. Keep them out since we will be going over them. Also, take out your notes packet! 1 Chapter 5 Electrons In Atoms 5.1
Unit 8 Building Atoms with Quantum Leaps
Oh boy... Sam Beckett (from Quantum Leap) Unit 8 Building Atoms with Quantum Leaps Physicists Put Atom in Two Places at Once This was the headline in the science section of the New York Times on May 28,
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,
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
Wave-Mechanical Model of the Atom. Aim: To write orbital notation and electron configurations representing the wave mechanical model of the atom.
Wave-Mechanical Model of the Atom Aim: To write orbital notation and electron configurations representing the wave mechanical model of the atom. Wave-Mechanical Model of the Atom Atoms contain protons,
Terms to Know. 10.Angular quantum number 11.Magnetic quantum number 12.Spin quantum number
Terms to Know 1. Photon 2. Atomic emission spectrum 3. Ground state 4. Atomic orbital 5. Aufbau principle 6. Pauli exclusion principle 7. Hunds rule 8. Electron configuration 9. Principle quantum number
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
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
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
Model 1 The Boarding House
NS D4 Electron Configurations Name What is the electron structure in an atom? The electron structure of an atom is very important. Scientists use the electronic structure of atoms to predict bonding in
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
Chemistry 11. Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms
Chemistry 11 Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms 2 1. Atomic number and atomic mass In the previous section, we have seen that from 50 to 100 years after Dalton proposed
CHAPTER 3: Electrons in Atoms
CHAPTER 3: Electrons in Atoms 3.1 Sub-shells and Atomic Orbitals 3.2 Electronic Configuration 3.3 Ionisation Energy Learning outcomes: (a) describe the number and relative energies of the s, p and d orbitals
Atomic Structure Atoms are very small ~ metres All atoms are made up of three sub-atomic particles: protons, neutrons and electrons
IB Chemistry (unit ) ATOMIC THEORY Atomic Structure - Recap Questions Define the following words: Atom Element Molecule Compound Atomic Structure Atoms are very small ~ - metres All atoms are made up of
Essential Organic Chemistry. Chapter 1
Essential Organic Chemistry Paula Yurkanis Bruice Chapter 1 Electronic Structure and Covalent Bonding Periodic Table of the Elements 1.1 The Structure of an Atom Atoms have an internal structure consisting
POGIL: Electron Configurations
Name DUE DATE Period Chemistry POGIL: Electron Configurations Why? The electron structure of an atom is very important. Scientists use the electronic structure of atoms to predict bonding in molecules,
Name: Class: Date: ID: A
Name: Class: _ Date: _ ID: A EOC review II Matching Match each item with the correct statement below. a. atomic orbital d. ground state b. aufbau principle e. Pauli exclusion principle c. electron configuration
Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2
Name Date Due Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2 Directions: Write your answers to the following questions in the space provided. For problem solving, all of the
Chapter 4 Arrangement of Electrons in Atoms. 4.1 The Development of a New Atomic Model
Chapter 4 Arrangement of Electrons in Atoms 4.1 The Development of a New Atomic Model Properties of Light Electromagnetic Radiation: EM radiation are forms of energy which move through space as waves There
WP Unit 2 Practice: The Atom
WP Unit 2 Practice: The Atom Name 1. Name, and identify them clearly in your answer, one halogen, one noble gas, one alkali metal, one alkali earth metal, one metalloid, one transition metal and finally
Chapter 7 The Structure of Atoms and Periodic Trends
Chapter 7 The Structure of Atoms and Periodic Trends Jeffrey Mack California State University, Sacramento Arrangement of Electrons in Atoms Electrons in atoms are arranged as SHELLS (n) SUBSHELLS (l) ORBITALS
Goals for Today. Clarify some Rydberg Concepts Absorption vs. emission
Note: Due to recent changes the exam 2 material for these slides ends at Ionization Energy Exceptions. You can omit Lewis Structures through General Formal Charge Rules. CH301 Unit 2 QUANTUM NUMBERS AND
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
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
Atomic Spectroscopy II
Applied Spectroscopy Atomic Spectroscopy II Multielectron Atoms Recommended Reading: Banwell And McCash Chapter 5 The Building-Up (aufbau) Principle How do the electrons in multi-electron atoms get distributed
Chapter 7. DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration
Chapter 7 DeBroglie Waves Heisenberg s Uncertainty Quantum Numbers Electron Configuration Are Electrons Particles or Waves? De Broglie (1892 1987) If electromagnetic radiation behaves as a particle, could
What are molecular orbitals? QUANTUM MODEL. notes 2 Mr.Yeung
What are molecular orbitals? QUANTUM MODEL notes 2 Mr.Yeung Recall, the quantum model is about electrons behaving both a wave and a particle. Electrons are in areas of calculated probability, these are
PHYS 202. Lecture 23 Professor Stephen Thornton April 25, 2005
PHYS 202 Lecture 23 Professor Stephen Thornton April 25, 2005 Reading Quiz The noble gases (He, Ne, Ar, etc.) 1) are very reactive because they lack one electron of being in a closed shell. 2) are very
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
Orbital Diagrams & Electron Configurations for Atoms and Ions
Orbital Diagrams & Electron Configurations for Atoms and Ions Section 3.5 The Periodic Table is like a MAP that describes the arrangement of electrons within their orbitals. Orbital diagrams represent
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
Unit 1. Electronic Structure page 1
Unit 1 Electronic Structure Section 1. Learning Outcomes Practice Questions Answers Electronic Structure Electromagnetic spectrum / calculations Electron configuration / Periodic Table Electronic Structure
Key Equations. Determining the smallest change in an atom's energy.
ATOMIC STRUCTURE AND PERIODICITY Matter and Energy Key Equations λν = c ΔE = hν Relating speed of a wave to its wavelength and frequency. Determining the smallest change in an atom's energy. H( λ =R n
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
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
Many-Electron Atoms. Thornton and Rex, Ch. 8
Many-Electron Atoms Thornton and Rex, Ch. 8 In principle, can now solve Sch. Eqn for any atom. In practice, -> Complicated! Goal-- To explain properties of elements from principles of quantum theory (without
Section 11: Electron Configuration and Periodic Trends
Section 11: Electron Configuration and Periodic Trends The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 11.01 The Bohr Model of the Atom
Chapter 8. Structure of Atom
Chapter 8 Structure of Atom Synopsis Energy propagates as electromagnetic waves and can have a wide variety of wavelengths. The entire range of wavelengths is known as the electromagnetic spectrum. Max
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
Chap 7 Part 2Tc.notebook November 02, 2017
Chapter 7 Section 4 11 Quantum mechanics electrons are organized in atoms in very specific ways energy levels represent distances from the nucleus inside energy levels are orbitals that can hold 2 electrons
Chapter 9. Molecular Geometry and Bonding Theories
Chapter 9. Molecular Geometry and Bonding Theories PART I Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. The shape of a molecule
Quantum theory predicts that an atom s electrons are found in: To account that orbitals hold two electrons, we need:
Quantum theory predicts that an atom s electrons are found in: To account that orbitals hold two electrons, we need: Shells (principle quantum number, n) Subshells (angular momentum, l) Orbitals (magnetic
Chapter 1 Chemical Bonding
Chapter 1 Chemical Bonding 1.1 Atoms, Electrons, and Orbitals Atoms are composed of + Protons positively charged mass = 1.6726 X 10-27 kg Neutrons neutral mass = 1.6750 X 10-27 kg Electrons negatively
Chapter 6. Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms Electronic Structure Electronic structure the arrangement and energy of electrons 1 st lets talk about waves Why? Extremely small particles have properties that
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals. Description A1. Marble Lab. Nailon Isotope Lab A2.
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals Name: Period: Unit 3 Atomic Structure and Periodic Table Unit Goals- As you work through this unit, you should be able to: 1. describe
PAPER No. 7: Inorganic Chemistry - II (Metal-Ligand Bonding, Electronic Spectra and Magnetic Properties of Transition Metal Complexes
Subject Chemistry Paper No and Title Module No and Title Module Tag 7, Inorganic chemistry II (Metal-Ligand Bonding, Electronic Spectra and Magnetic Properties of Transition Metal Complexes) 10, Electronic
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
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
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
Remember Bohr s Explanation: Energy Levels of Hydrogen: The Electronic Structure of the Atom 11/28/2011
The Electronic Structure of the Atom Bohr based his theory on his experiments with hydrogen he found that when energy is added to a sample of hydrogen, energy is absorbed and reemitted as light When passed
Name Class Date. Chapter: Arrangement of Electrons in Atoms
Assessment Chapter Test A Chapter: Arrangement of Electrons in Atoms In the space provided, write the letter of the term that best completes each sentence or best answers each question. 1. Which of the
CHEM 103 Spectroscopy and the Quantum Mechanical Model
CHEM 103 Spectroscopy and the Quantum Mechanical Model Lecture Notes April 6, 2006 Prof. Sevian Agenda Emission spectroscopy How the quantum mechanical model explains it Where quantum mechanics breaks
Many-Electron Atoms. Thornton and Rex, Ch. 8
Many-Electron Atoms Thornton and Rex, Ch. 8 In principle, can now solve Sch. Eqn for any atom. In practice, -> Complicated! Goal-- To explain properties of elements from principles of quantum theory (without
Chapter 11 Prep Test CLASS SET!!!! Matching
CLASS SET!!!! ID: A Chapter 11 Prep Test Matching Match each item with the correct statement below. A electronegativity D period B ionization energy E transition metal C atomic radius F group 1 type of
PHYS 202. Lecture 23 Professor Stephen Thornton April 20, 2006
PHYS 202 Lecture 23 Professor Stephen Thornton April 20, 2006 Reading Quiz The noble gases (He, Ne, Ar, etc.) 1) are very reactive because they lack one electron of being in a closed shell. 2) are very
Unit 1 Part 1 Atomic Structure and The Periodic Table Introduction to Atomic Structure UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE
UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE PART 1 INTRODUCTION TO ATOMIC STRUCTURE Contents 1. Protons, Neutrons and Electrons 2. Early Models of the Atom 3. Isotopes and Atomic Mass 4. Atoms and Ions
Biotech 2: Atoms and Molecules OS Text Reading pp Electron cloud Atoms & Nucleus 2e Subatomic Particles Helium Electron cloud
9/4/017 Biotech : Atoms and Molecules OS Text Reading pp. 34-4 Atoms & Subatomic Particles Nucleus Helium e cloud cloud e Protons Neutrons Mass number = 4 s Nucleus Carbon atomic number = # of protons
Quiz 2/ A/ How many orbitals are possible for n=3? B/ How many orbital nodes do 2S,3P,4d and 5f orbitals exhibit? 11/11/2016 Dr. Mohammed H.
Quiz 2/ A/ How many orbitals are possible for n=3? B/ How many orbital nodes do 2S,3P,4d and 5f orbitals exhibit? 11/11/2016 Dr. Mohammed H. Said 1 lecture 2 Effective nuclear charge The effective nuclear
2.3 Atomic Structure and the Periodic Table
2.3 Atomic Structure and the Periodic Table Although the Bohr theory and subsequent revisions were based on the idea of an electron traveling in some kind of orbit or path, a more modern view is that 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
1.1 Electronic Structure & Spectroscopy
Advanced Higher Chemistry (CfE) Unit 1 Unit 1 - Inorganic & Physical Chemistry 1.1 Electronic Structure & Spectroscopy Electromagnetic Spectra Electron Configuration Spectroscopy Learning Outcomes Pupil
How Electrons Determine Chemical Behavior
The Periodic Table Activity 7 How Electrons Determine Chemical Behavior GOALS In this activity you will: Investigate more patterns electron arrangements of atoms. Relate the positions s on the, their electron
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
Electrons in Atoms. So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding
Electrons in Atoms So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding 12.1 Development of Atomic Models Dalton s Thompson s Rutherford s Bohr s carbon Quantum Model
Test bank chapter (7)
Test bank chapter (7) Choose the most correct answer 1. The lowest energy state of an atom is referred to as its a) bottom state. b) ground state. c) fundamental state. d) original state. 2. All s orbitals
Guide for Reading. Vocabulary electron configurations aufbau principle Pauli exclusion principle Hund s rule. Reading Strategy
5.2 Electron Arrangement in Atoms 5.2 Connecting to Your World Does this scene look natural to you? Surprisingly, it is. Arrangements like this are rare in nature because they are unstable. Unstable arrangements,