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