Periodic Trends Notes

Page 1: Intro to the Atom

• Basic introduction to atomic theory and structure is presented.

Page 2: Our Plan

• Have you completed the Intro to Atom Review on pages 1-4?

  • Review of Intro to Atom (Atoms & Isotopes Quizizz)

  • Notes on Introduction to the Atom

  • Complete Practice Problems 1-6 on pages 6 & 7.

Page 3: Our Plan Continued

• Reiterate completion of the Intro to Atom Review on pages 1-4.

  • Analyze Test Results.

  • Perform Test Corrections.

  • Watch videos and take notes from the presentation on Google Classroom.

Page 4: Test Results

• Overview of student test results.

Page 5: Introductory Activity Quizizz!

• Engaging quiz regarding the introduction to atoms.

Page 6: Essential Question

• What evidence exists in your everyday life for the existence of atoms?

Page 7: Main Idea/Question

• How has evidence led to the current model of the atom?

Page 8: The Model of the Atom

• Description of how scientists use experimental results to test scientific models.

• If experimental results deviate from the model's predictions, the model needs revision or replacement.

Page 9: The Model of the Atom Expanded

• Further elaboration on the concept of the atomic model and its evolution.

Page 10: Robust Models

• A robust scientific model can explain/predict numerous results across various experimental circumstances.

Page 11: Main Idea/Question

• How does Coulomb's law help explain atomic structure?

Page 12: Coulomb’s Law

• States that the force between two charged particles is proportional to the product of their charges and inversely proportional to the square of the distance between them.

• Forces can be attractive (opposite charges) or repulsive (same charges).

Page 13: Application of Coulomb's Law

• Relevant throughout the unit because it helps explain periodic trends (e.g., ionization energy, atomic size) and overall atomic structure.

Page 14: Coulomb's Law Explained

• Video resource referenced for explanation of Coulomb’s Law (first 2 minutes recommended).

Page 15: Main Idea/Question

• How does light behave as both a particle and a wave?

Page 16: The Nature of Light

• Light exhibits properties of both particles and waves, presenting a duality.

• Explains how this dual behavior contradicts ordinary physical intuition.

Page 17: Duality: The Double Slit Experiment

• The experiment that illustrates the dual wave-particle nature of light.

Page 18: Light's Mysteries

• Ongoing questions regarding how light exhibits both wave-like spreading and particle-like localization.

Page 19: The Wave Nature of Light

• Light travels at a constant speed in a specific medium (speed of light in a vacuum is c = 2.998 x 10^8 m/s).

Page 20: Wavelength & Frequency

• Wavelength (λ): the distance between identical points in consecutive cycles (units: m or nm).

• Frequency (ν): number of wave cycles passing a point in a unit of time (units: s–1 or hertz).

Page 21: Wavelength and Frequency Visualization

• Differences in amplitude and frequency illustrated with varying wavelengths.

Page 22: Relationship Between Wavelength and Frequency

• Formula c = λν where c is the speed of light, λ is wavelength, and ν is frequency.

Page 23: Conversion Factor

• Insists that 1 m = 1 x 10^9 nm is essential for calculations.

Page 24: Calculating Frequency

• Simple instructions on how to calculate frequency from given wavelength data.

Page 25: Example 1

• Solve for the frequency of an X-ray with a wavelength of 8.21 nm.

Page 26: Example 2 - Try It Out!

• Wavelength calculation for infrared radiation with a frequency of 9.76 x 10^13 Hz yields a result of 3.07 x 10^3 nm.

Page 27: The Particle Nature of Light

• Light exists as particles known as photons; energy of a photon is given by E = hν, where h is Planck's constant (6.626 x 10^-34 J·s).

Page 28: Light Joke

• A humorous anecdote about a photon checking into a hotel.

Page 29: Example 3

• Calculate the energy of a photon of violet light with a frequency of 6.15 x 10^14 s–1.

Page 30: Example 4

• Calculate the energy in kilojoules of 1 mol of photons of red light at a wavelength of 632.8 nm.

Page 31: Example 5 - Try It Out!

• Determine the energy in joules per photon for ultraviolet light at a wavelength of 235 nm (8.48 x 10^-19 J/photon).

Page 32: The Photoelectric Effect

• Light on a metal surface can eject electrons; frequency must exceed a threshold.

Page 33: Kinetic Energy of Electrons

• Kinetic energy is proportional to light’s frequency and independent of light intensity, contradicting wave theory.

Page 34: The Electromagnetic Spectrum

• Ranked by increasing wavelength and decreasing frequency: Gamma Rays, X-Rays, UV Light, Infrared, Microwaves, Radio Waves.

Page 35: Frequency Range of Elements

• Approximate Hz frequencies for different categories including cellular, AM radio etc.

Page 36: Visible Light

• The visible spectrum and mnemonic ROYGBIV for color recognition.

Page 37: Visible Light Properties

• Discussion of the characteristics of visible light; wavelengths and corresponding energies.

Page 38: Conceptual Example

• Compare frequencies of two light sources: faint green vs bright red light.

Page 39: Problem Reminder

• Reminder to complete practice problems on pages 6 & 7.

Page 40: Orbitals

• Initiation into concepts of atomic orbitals and their significance.

Page 41: Our Plan

• Overview of tasks including review, quizzes, notes on orbitals, and practice problems on page 12.

Page 42: Quick Review

• Review of the atom on pages 1-4 and completion of associated review work.

Page 43: Atomic Information Summary

• Breakdown of atomic structure (name, symbol, atomic and mass numbers, neutrons, electrons).

Page 44: Math Review Answers

• Solutions to example problems presented earlier.

Page 45: Essential Question

• Inquiry loop back to earlier essential question regarding existence of atoms.

Page 46: Main Idea/Question

• How is spectroscopy utilized to determine chemical structure?

Page 47: Spectroscopy Definition

• General term describing methods of instrumental analysis based on electromagnetic radiation interacting with matter.

Page 48: Types of Transitions in Spectroscopy

• Associated electromagnetic spectrum types to molecular transitions (microwave, infrared, UV/Visible).

Page 49: Microwave Spectroscopy

• Description of microwave spectroscopy and its relation to molecular rotation.

Page 50: Homonuclear vs. Heteronuclear Molecules

• Distinction between molecular types in context of microwave activity.

Page 51: Infrared Spectroscopy Importance

• Application of infrared spectroscopy in organic chemistry and functional group identification.

Page 52: Summary of Spectroscopic Techniques

• Comparison of energy abilities of UV, Visible, Infrared, and Microwave spectroscopy.

Page 53: UV/Vis Spectroscopy

• Examples of elements and compounds used in UV/Vis spectroscopic assessments.

Page 54: Continuous Spectrum

• Definition of a continuous spectrum as produced from passing white light through a prism.

Page 55: Line Spectra and Elements

• Explanation of line spectra generated from pure elements and their significance to atomic energy levels.

Page 56: Line Spectra Characterization

• Visual representation of line spectra produced from gaseous element discharges.

Page 57: Unique Element Fingerprints

• The unique identification of elements through their specific line emission spectra.

Page 58: Bohr’s Model Development

• Transition from historical atomic understanding to Bohr’s model.

Page 59: Electron Orbit Assumptions

• Electrons assumed to have quantized orbits around the nucleus in Bohr's model.

Page 60: Ground State vs. Excited State

• Distinction mentioned between electron states in atomic structure.

Page 61: Energy Level Representation

• Visualization of energy levels in relation to electron transitions.

Page 62: Quantized Electronic Energy Levels

• Explanation of quantized nature and transitions leading to line spectra.

Page 63: Hamburger Energy Levels Joke

• Anecdotal humor regarding energy levels in food analogy.

Page 64: Activity and Worksheets

• Hands-on activities or assignments referring back to electron configuration.

Page 65: Example of Electron Filling

• Demonstrative example of arranging electrons within orbital diagrams.

Page 66: Essential Question Repeat

• Reiterating earlier essential question.

Page 67: Main Idea/Question

• Inquiry about quantum mechanical model of the atom.

Page 68: Quantum Mechanical Model

• Distinguishing modern quantum mechanics from previous atomic models.

Page 69: Application of Mathematics

• Use of mathematical descriptions in quantum mechanics to assess electron positions.

Page 70: Adaptations of Quantum Model

• Contemporary software used to apply quantum mechanical models.

Page 71: Heisenberg Uncertainty Principle

• Description of limitation in measuring microscopic position and momentum simultaneously.

Page 72: Measurement Consequences

• Impacts of measuring particles, such as photons, affecting their behavior.

Page 73: Uncertainty Principle Analogy

• Simplifying analogy regarding measuring particles.

Page 74: Probability Analogy

• Analogy to capture the uncertainty of electron positions.

Page 75: Electron Humor

• Light-hearted electron exchange joke.

Page 76: Joke Time

• Another humorous anecdote around Heisenberg's and Schrodinger's principles.

Page 77: Our Plan

• Detailed breakdown of tasks to complete regarding atom reviews and practice problems.

Page 78: Quantum Numbers in Orbitals

• Introduction and importance of quantum numbers.

Page 79: Orbitals and Density Analogy

• Using trees and apples to represent electron density distribution.

Page 80: Electron Density Distribution

• Explaining the spatial distribution of electrons.

Page 81: Defining Quantum Numbers

• Explanation of parameters used to quantify electron location.

Page 82: Principal Quantum Number (n)

• Details on energy levels represented by the principal quantum number.

Page 83: Periodic Table Representation

• Overview of elements and their electron configurations by energy level.

Page 84: Angular Momentum Quantum Number (l)

• Description of shapes indicated by quantum numbers.

Page 85: Continuation of Periodic Table Representation

• Further detailing of orbital representation in periodic classification.

Page 86: Magnetic Quantum Number (m1)

• Overview of orientations specific to orbital types and sublevels.

Page 87: S Sublevel Representation

• Visual studies of s orbitals.

Page 88: P Orbitals Representation

• Spatial representation of three p orbitals.

Page 89: D Orbitals Overview

• Discussion of five distinct d orbitals.

Page 90: F Orbitals Overview

• Summary of the seven types of f orbitals in chemistry.

Page 91: Periodic Table Overview

• Reinforcement of the periodic table structure.

Page 92: Quantum Numbers Summary

• Recap of quantum numbers key to understanding atomic structure.

Page 93: Spin Quantum Number (ms)

• Description of electron spin description within quantum terms.

Page 94: Visual Summary Resource

• Link to a visual summary on quantum theory application.

Page 95: Further Learning Resource

• Link to an interactive educational periodic system.

Page 96: Understanding Check Reminder

• Check for comprehension through assigned problems.

Page 97: Electron Configurations Introduction

• Overview of electron configurations and their significance.

Page 98: Our Plan Adjustments

• Outline of modified tasks, including video review and practice work.

Page 99: Video Resource

• External link provided for video studying on electron configurations.

Page 100: Essential Question Recap

• Returning focus to atoms' existence evidence in daily life.

Page 101: Main Idea/Question

• Inquiry into chemists' communication methods for electron location.

Page 102: Quick Review

• Brief summary with key points regarding orbitals and quantum numbers.

Page 103: Quick Review of Quantum Numbers

• Symbol representations and their values listed.

Page 104: Extended Quick Review

• Visual overview of orbitals and their configurations.

Page 105: Pauli Exclusion Principle

• Explanation of electron sharing restrictions and their significance.

Page 106: Aufbau Principle Basics

• Overview of electron filling from lowest to highest energy levels.

Page 107: Aufbau Principle Examples

• Illustrative examples of Aufbau principle in action for elements.

Page 108: Hund’s Rule Exploration

• Explanation of orbital filling behavior according to Hund's rule.

Page 109: Orbital Diagrams

• Visual representation of electron configurations in orbital diagrams.

Page 110: Electron Configuration Overview

• Description of electron configuration explanations and representations.

Page 111: Periodic Table Configuration Example

• Listing of periodic table elements and their configurations.

Page 112: Group Overview

• Summary of electron configurations across the periodic table.

Page 113: Orbital Notation Description

• Explanation of how to write orbital notation for elements.

Page 114: Configuration for Sulfur

• Comparative configurations for element sulfur using spdf notation and orbital diagrams.

Page 115: Configuration for Calcium

• Instructions to determine configurations for calcium.

Page 116: Electron Configuration Simulation Link

• Interactive simulation link for visual learning of electron configurations.

Page 117: Noble-Gas Core Notation

• Introduction to condensed electron configuration notation using noble gases.

Page 118: Periodic Table Notation Overview

• Discussing configurations and transformations in periodic table context.

Page 119: Simplifying Orbital Notation

• Approach to writing configurations in noble gas notation.

Page 120: Ground-State Configuration Example

• Guided configuration writing for strontium in both notations.

Page 121: Main Group vs. Transition Elements

• Difference in filling orbitals for main group vs transition elements.

Page 122: Exceptions to Aufbau Principle

• Analysis of elements that deviate from expected filling patterns.

Page 123: Noble Gas Notation for Silver

• Practice on identifying noble gas notation for silver.

Page 124: Valence and Core Electrons Overview

• Clarification on definitions and distributions of valence vs core electrons.

Page 125: Valence and Core Electrons Practice Examples

• Practice questions based on identifying valence and core electrons of compounds.

Page 126: Electron Configuration of Anions

• Overview of process for anion configurations, completing electron shells.

Page 127: Electron Configuration of Cations

• Process for determining configurations for metal cations post-electron removal.

Page 128: Exemplifying Electron Configurations

• Breakdown of configurations for multiple atom types.

Page 129: Co3+ Configuration Example

• Calculate configuration for Co3+ illustrating noble-gas shorthand notation.

Page 130: More Practice on Configuration Notation

• Prompt to provide noble gas notation examples for nonmetals and transition metals.

Page 131: Isoelectronic Definition and Examples

• Explanation of isoelectronic series and their significance.

Page 132: Isoelectronic Species Practice

• Engage with isoelectronic examples and comparisons.

Page 133: Final Practice Reminder

• Completion reminder for practice problems from pages 14-16.

Page 134: Beer’s Law & Vibrational Spectroscopy

• Introduction to Beer’s Law and its relationship to spectroscopic analysis.

Page 135: Our Plan Recap

• Summary of session plans including quizzes and notes.

Page 136: Quantum Numbers Review

• Comprehensive points regarding quantum number implications and examples.

Page 137: Answer Key Overview

• Key to answers related to earlier questions about quantum numbers.

Page 138: Essential Question Reminder

• Recap of ongoing essential question surrounding atom existence in real life.

Page 139: Main Idea/Question Exploration

• Inquiry into the functions of electronic and vibrational spectra.

Page 140: Utilizing Electronic & Vibrational Spectra

• Explains how spectra identify elements and compounds through spectra utilization.

Page 141: Color Absorption Dynamics

• Describe the color absorption characteristics based on light interactions.

Page 142: Wavelength Absorption Analysis

• Discuss implications for color and absorption within transition metals like Chromium.

Page 143: Spectrophotometer Device Overview

• Introduced to the spectrophotometer's function and utility in analysis.

Page 144: Colorimeter Functionality

• Description of colorimetric devices and their purpose.

Page 145: Measuring Absorbance

• Detailed viewpoints on how photonic measures take place through absorption metrics.

Page 146: Absorbance Definition

• Definition explaining how absorbance measures light interaction with samples.

Page 147: Visible Light Spectrum Handling

• Engage in how instruments operate within visible light spectrum ranges.

Page 148: Spectrophotometer Control Overview

• Controls for wavelength and absorbance adjustments.

Page 149: Interactive Beer’s Law Simulation

• Link provided for activities in Beer’s Law experimentation.

Page 150: Beer’s Law Formula Introduction

• Breakdown detailing Beer’s Law and how it relates to concentration measurement.

Page 151: Proportions in Beer’s Law

• Explanation on direct relationships between absorbance and concentration.

Page 152: Example Application of Beer’s Law

• Example regarding understanding of wavelength absorption principles.

Page 153: Fe+3 Determination Example

• Practical application for concentration determination involving absorbance.

Page 154: Cr3+ Calibration Example

• Showcases how calibration curves function in absorbance analysis.

Page 155: Summary Resource Link

• Directing towards Bozeman science summary resource for causative theories.

Page 156: Food Dye Configuration Table

• Overview of food dye sample absorption analysis for concentration understanding.

Page 157: Food Dye Molarity Calculate

• Detailed observation of molarities across dilutions and their implications.

Page 158: Wrap Up with Quizizz

• Final tasks involving assessments through Quizizz.

Page 159: Investigation 4 Announcement

• Keeps track of pre-lab activities in conjunction with investigative tasks.

Page 160: Classroom Setup Overview

• Classroom expectations are established for organization and procedural flow.

Page 161: Lesson Plan Preview

• Roadmap for planning out investigation activities and report due dates.

Page 162: Investigation Overview

• Breaks down investigation expectations concerning teaching procedures.

Page 163: Food Dye Absorbance Analysis

• Sample results related to food dye absorbance leading to inference generation.

Page 164: Laboratory Protocol Tips

• Guidelines for effective lab work preparation and safe procedures.

Page 165: Measuring Mass Percent in Brass

• Contextualize understanding measurement and value confidence in results.

Page 166: Periodic Trends Introduction

• Engaging summary regarding trends across the periodic table.

Page 167: Trends Assessment Overview

• Detailing steps in the assessment of periodic trends.

Page 168: Periodic Evidence Reminder

• Return focus to atom existence evidence with periodic trends related.

Page 169: Trends in Periodic Table

• Outline of observational trends in atomic details reflected in periodic table.

Page 170: Families in the Periodic Table

• Overview of major elemental families found in the periodic table framework.

Page 171: Periodic Structure Overview

• Evaluate the structure and respective families that are equivalent.

Page 172: Shielding and Trends

• Explanation of shielding effects on atomic characteristics and their resultant trends.

Page 173: General Properties Trends

• Discussions on repetitive chemical and physical properties as elements categorized.

Page 174: Understanding Atomic Radius

• Clarifies definitions concerning atomic measurements and relationships.

Page 175: Periodic Trends in Atomic Radius

• Explains reasons for atomic radius variations across the periodic table.

Page 176: Nuclear Charge Impact

• Discusses effective nuclear charges on atom sizes based on arrangement.

Page 177: Period Element Sequence

• Listing of elements across various periods of the periodic table.

Page 178: Group Trends in Atomic Radius

• Explanation of atomic radius increase down groups across the periodic table.

Page 179: Atomic Radii Examples

• Specific examples showcasing atomic radii trends for visual verification.

Page 180: Listed Period Elements Again

• Renote to engage understanding of specific elemental trends.

Page 181: Atomic Radius Comparisons

• Engage with a specific task of sorting elements based on atomic radius.

Page 182: Ionic Radius Dimensions

• Defines ionic radius with comparisons between cations and anions.

Page 183: Cation Characteristics

• Discusses why cations appear smaller than their atomic counterpoints due to electronic change.

Page 184: Anionic Characteristics

• Anions compared to neutral atoms that lead to notable size increases.

Page 185: Ionic Radius Properties and Data

• Data presented on ionic radii for various elements for reference.

Page 186: Ionic Size Ordering Task

• Engage with an exercise to compare sizes of ionic species.

Page 187: Ionization Energy Introduction

• Foundations based on energy required to remove electrons from their atom.

Page 188: First Ionization Energy Description

• Clarification of requirements and assessments necessary for removing electrons.

Page 189: Trends in Ionization Energy

• Discussion on general ionization energy trends and their influential factors.

Page 190: Energy Jumps in Ionization

• Notable jumps in energy levels after removing a specific number of electrons.

Page 191: Ionization Energy Explaining Patterns

• Compare ionization energy aspects of periodic table elements utilizing trends.

Page 192: Quantitative Ionization Energy Inquiry

• Engage with energy values to calculate valence electrons based on energy statistics.

Page 193: AP Exam Readiness Testing

• Question presented to understand ionization energy trends across elements.

Page 194: Ionization Energy Trends Across Period

• Increases across periods due to additional protons enhancing attraction.

Page 195: Broad Visual Introduction to Elements

• Overall atomic representation in terms of their structural elements and energy.

Page 196: Ionization Energy Group Trends

• General decreases in ionization energy as electron shielding increases down groups.

Page 197: General IE Trends Clarified

• Review surrounding jumps within ionization energy and comparative measurements.

Page 198: Analogies for Ionization Energy Understanding

• Comparative thoughts between major elements to appreciate underlying energy configurations.

Page 199: Understanding Larger Trends

• Connections made between periodic table elements and ionization levels.

Page 200: Ionization Energy Values Structure

• Explaining exceptions to ionization predictions based on energy additions and arrangements.

Page 201: Electron Repulsion Factor

• Discusses electron pair repulsions within orbitals and their role in energy behavior.

Page 202: Detailed Ionization Insights

• Follow-through to concepts concerning attraction versus repulsion and their interdependencies.

Page 203: Ionization Energy Order Comparisons

• Engage with tasks requiring ordering of elements on the basis of input energy.

Page 204: Electron Affinity Basics

• Understanding the change in energy via electron acquisition.

Page 205: Period Trends in Electron Affinity

• Increases across periods as protons ultimately draw more electrons.

Page 206: Group Trends Summary

• Emphasizes decreases in electron affinity as areas increase across the periodic table.

Page 207: Graphical Representation of Trends

• Visual representations of periodic trends capturing proton attraction dynamics.

Page 208: Summary and Departure of Electronegativity

• Offers summary observations compared to electron energy and properties.

Page 209: Electronegativity Essentials

• Discuss ability of different atoms to attract electrons in compounds.

Page 210: Electronegativity Period Trends

• Noted increases across periods, capturing attraction powers of atoms.

Page 211: Generalized Trends and Gaps

• Compile notes on general patterns, reflecting on roll models and atomic relationships across fields.

Page 212: Electronegativity Group Trends

• Explore how properties diminish down groups, impacting compound formation.

Page 213: Electronegativity vs. Electron Affinity

• Compare and contrast definitions crystallizing their individual characteristics.

Page 214: Utility of Periodicity

• Discuss practical usages of periodicity in new materials' design and elemental replacements.

Page 215: Periodicity Judgement

• Observational evaluations aiding predictability in experimental outcomes.

Page 216: Comparative Values Table

• Table representing key atomic properties and their respective values across periodic table.

Page 217: Summary Resource Link

• Connects to additional study resources reinforcing key principles present in discussions.

Page 218: Periodic Review Material

• Additional links offered for further diving into periodic characteristics.

Page 219: Practice Recap

• Developed practice materials deployed in dynamic assessments within elements' properties.

Page 220: Addressed Wrap- Up Material

• Closure with understanding tracking concepts alongside digital evaluation forms to check for knowledge retention.

Page 221: Mass Spectrometry & PES Overview

• Initial overview of mass spectrometry concepts tied to isotopes and compound analysis.

Page 222: Continued Lesson Plans

• Laying out steps for further exploration within mass spectrometry and assessments thereof.

Page 223: Video Resource for Introductory Material

• External video link intended for enhancing student understanding.

Page 224: Post-Assessment Steps

• Clarifying next steps within laboratory preparations including analytical calculations.

Page 225: Essential Question Recapture

• Return to the examination of atom existence in real-life applications.

Page 226: Main Idea on Mass Spectrometry

• Core focus on implications mass spectrometry has in chemical structure determination.

Page 227: Cited Work

• Documentation attributions to documents and scientific work referenced throughout modules.

Page 228: Analytical Capability of Mass Spectrometry

• Definition of mass spectrometry now depicted as a powerful analytical tool.

Page 229: Fundamental Mass Spectrometer Mechanics

• Breakdown of how mass spectrometers function to identify compounds.

Page 230: Design Overview

• Depiction with visual aids of fundamental mass spectrometer components.

Page 231: Example Analysis of Silicon Spectrum

• Inquiry into isotopes presented through mass spectrum analysis of silicon.

Page 232: Copper Isotope Analysis

• Evaluation of the mixtures and their isotopes observed through mass spectrometry.

Page 233: Further Average Atomic Mass Calculations

• Example showcasing weighted averages in atomic mass concerning isotope populations.

Page 234: Mass Spectrum Analysis of Unknown Elements

• Engages in analytical thinking around unknown elements and their carbon structure extraction.

Page 235: PES Analysis Inquiry

• Questions around the understanding of chemical structures via photoelectron spectroscopy.

Page 236: Photoelectron Spectroscopy Mechanics

• Description of PES and its significance in understanding electron energies.

Page 237: Historical Context of PES

• Reference back to origins regarding the photoelectric effect and its developments.

Page 238: Instrument Mechanics of PES

• Basic look at PES instruments that perform investigative electric structures.

Page 239: Schematic of a PES Device

• Visual depiction of major system components that comprise photoelectron spectrometry.

Page 240: Electron Ejection Explanation

• Electron ejection probability narrative linked to varying energetic emissions.

Page 241: Spectrum Analysis Discussion

• Spectrum valuation and derivation of numerical data from energy levels.

Page 242: PES Lambda Example

• Example cases of electron configurations determined from photoelectron spectroscopy.

Page 243: Li Structure Analysis via PES

• Evaluate acceptance for electronic orbital matching with PES peak identification.

Page 244: PES Identification Challenge

• Inquiry into visual phenomena of PES representations leading to chemical species identification.

Page 245: Comparative Spectroscopy Labeling

• Discussion of unknown spectral structures and how to determine elemental characteristics.

Page 246: Pre-Lab Question Support

• Group pre-lab related inquiry, focusing on computational assistance.

Page 247: Detailed Pre-Lab Analysis

• Application of Beer’s Law in sample assessments in lab-related investigations.

Page 248: Exit Ticket Focus for Understanding Assessment

• End with key reflective summary and exit rationale for gauging understanding.

Page 249: Investigation Focus

• Referencing ongoing assessment indicators and tracking for forthcoming investigations.

Page 250: System for Learning Outcomes

• Detailing course management and planned learning modules focused on assessments and covers. 1