Chemistry 1A (PEM 1100) Course Notes

Introduction

  • Instructor: Glenn Loring, coordinator of PEM 1100 alongside Yanina Ladwig.

  • Chaotic start of the semester with technical issues noted.

    • Changes in systems have caused audio issues for lectures.

  • Purpose of video introductions in the course: engagement and context, not mere gimmick.

Course Overview

  • Chemistry at university focuses on understanding the "why" rather than just formulas and calculations.

  • Key question posed: "Why are you here in this chemistry class?"

    • Common response: Required core or gateway course.

Enrollment in Programs

  • Overview of students from various programs enrolled in the course:

    • Bachelor of Science (various tracks)

    • Bachelor of Biomedical Science

    • Bachelor of Engineering

    • Bachelor of Biotechnology

    • Human Movement, Nutrition, Health Sciences, Computing, Economics, Business, etc.

  • PEM 1100 serves as foundational chemistry for these diverse programs.

Goals of Course

  • Aim to foster joy and appreciation of chemistry among students.

  • Feedback from students encouraged to improve course experience.

Understanding Chemistry and Chemical Change

  • Emphasis on observing chemical changes like:

    • Energy transfer

    • Heat and light release

    • Color changes and gas release

  • Understanding chemical reactions begins with atoms and substances involved.

Indigenous Acknowledgment and Cultural Context

  • Recognition of traditional custodians of the land during the course sessions.

  • Emphasis on cultural capability as a graduate attribute and connection to knowledge transfer and learning.

Course Attendance and Participation

  • Attendance not mandatory, but active participation encouraged.

  • Flexibility in combining lecture streams if conflicts arise.

  • Lab sessions require sign-in to manage over 1000 students effectively.

  • Instruction on checking program and timetable adjustments.

Course Management through Blackboard

  • Blackboard as essential hub for course management and resources.

  • Important areas in Blackboard:

    • Orientation folder: Contains critical information.

    • Weekly folders: Organization of all lecture notes and resources by week.

  • Mid-semester exam will cover material up to week four; structured to aid learning.

  • Assessment folder contains schedule and requirements for tasks contributing to 15% of course marks.

Expectations and Communication

  • Course's expectation for adult learning and self-management.

  • Encouragement to post questions on discussion forums (Ed) monitored by teaching staff.

Introduction to Atom and Atomic Structure

  • Start with basic concepts of atom:

    • Composition of atoms: protons, neutrons, electrons (subatomic particles).

    • Importance of perceptible and measurable properties in science.

  • Introduction of atomic theory:

    • Classical views from Greeks (Democritus, Lucretius).

    • Development and evolution of atomic models:

    • Dalton's sphere model.

    • Plum pudding model (Thomson).

    • Rutherford’s nuclear model.

    • Bohr model.

    • Quantum mechanical model (Schrodinger).

Understanding of Atoms in Chemistry

  • Definition of atoms: Discrete chemical species with subatomic particles.

  • Molecules defined as atoms bonded together (intricacies of bonding discussed).

Atomic Number and Mass

  • Atomic notation:

    • Atomic number (ine character Z): number of protons.

    • Mass number (A): total protons + neutrons.

  • Example of sodium (Na) and copper (Cu) symbols emphasizing historical naming significance from Latin, Greek origins.

Learning Application: Trends in the Periodic Table

  • Approach to finding neutrons in an atom:

    • Example done with sulfur (atomic number 16, mass number 32).

  • Importance of linking atomic structure to chemical properties and behaviors.

    • Recognition of trends observed in periodic table educating chemistry behavior patterns.

Energy and Light Fundamentals in Chemistry

  • Introduction to concepts of energy in relation to atomic structure and bonding.

  • Equations introduced:

    • Energy relation to Planck's constant and frequency (E = h\nu).

    • Speed of light as a variable link to energy and wavelength (c = BB\nu).

    • Synthesis of relationships (E = hc/λ).

  • Practical examples illustrating these principles using experimental demonstrations of sodium and chlorine interactions.

Experimental Visualization of Atomic Structures

  • Discussion of atomic force microscopy providing visualization of atoms, bonding arrangements, and advancements in measurement techniques.

  • Historical acknowledgment of significant scientists contributing to atomic theory.

Importance of Active Participation and Regular Updates

  • Encouragement to check announcements, manage time effectively throughout the semester.

  • Critical takeaway: Stay updated with course dynamics and possible changes in the schedule and assessment due dates.