Lec 1 Chemistry essential ideas

GERMAN-MONGOLIAN - INSTITUTE FOR RESOURCES AND TECHNOLOGY

Chemistry: essential ideas

Lecture 1

Module Description

  • Module Title: Chemistry

  • Module Code: CHEM101

  • Duration: 1 semester

  • Semester: Fall

  • Module Start:

  • Credit Points: 5 CP

  • Workload: 180 h

    • Contact hours: 72 h

    • Individual study: 108 h

  • Module Coordinator: Prof. Dr. B. Battsengel

  • Language: English

Syllabus Content

  • Introduction to basic principles and concepts of:

    • Organic, inorganic, and physical chemistry

    • Components of matter and atomic theory

    • Compounds, formulas, names & mass of compounds

    • The mole, formula determination, writing & balancing chemical equations

    • Quantities of reactants & products, solution stoichiometry fundamentals

    • Nature of light, atomic spectra, quantum-mechanical model of the atom

    • Electron configuration and chemical periodicity

Assessment Criteria

  • Grade Total Score:

    • Performance: 30 points

    • Final Exam: 70 points

    • Write Essay, Teamwork: 10 points

    • Midterm: 10 points

    • Seminar: 10 points

Important Dates

  • Task Given: 3rd week

  • Checking Essay/Presentation: 7th week

  • Midterm Participation: 9th week

Participation & Exams

  • Individual Participation: Oral, mini-tests (4 times)

Final Exam Regulations

  • Attendance Requirement: 80% minimum; otherwise, failure

  • Cheating Policy: Zero tolerance; failure

  • Mobile Phones: No usage allowed

  • Restroom Policy: No breaks during the 2-hour exam duration

  • Retakes: 2 allowed in following semester; written application required for 2nd retake

Recommended Textbooks

  • Silberberg, Chemical Chemistry for Engineering Students

  • Principles: Reinforced Second Edition

  • Atkins: The Quest for Insight, Seventh Edition

  • Authors: Peter Atkins, Loretta Jones, Leroy Laverman

Course Content Overview

1.1 Fundamental Definitions

1.2 Chemical Arts and the Origins of Modern Chemistry

1.3 The Scientific Approach: Developing a Model

1.4 Chemical Problem Solving

1.5 Measurement in Scientific Study

1.6 Uncertainty in Measurement: Significant Figures

Why Study Chemistry?

  • Essential Role in Life:

    • Metabolism involves chemical reactions for breaking down/building up vital molecules.

    • Understanding Biology through chemical principles.

  • Chemistry is crucial in food, clothing, and everyday materials.

Definitions in Chemistry

  • Matter: Anything with mass and volume; includes all physical substances.

  • Composition: Types and amounts of substances making up matter.

  • Properties: Unique characteristics defining substances.

Detailed Understanding of Matter

  • Matter Types:

    • (a) Atoms of an element

    • (b) Molecules

    • (c) Mixtures

    • Any element has one kind of atom; compounds contain at least two types.

Properties of Matter

Physical Properties

  • Characteristics displayed independently:

    • Examples: color, melting point, boiling point, density.

Chemical Properties

  • Observable as substances interact:

    • Examples: flammability, corrosiveness.

Changes in Matter

Physical Change

  • Composition unchanged, involves state alterations (e.g. ice melting).

Chemical Change

  • Composition changes, new substances formed (e.g. combustion).

Characteristics of Changes

  • Physical Changes:

    • Do not change substance composition.

    • Examples: changes of state, volume adjustments.

  • Chemical Changes:

    • Result in new substances being created.

    • Examples: combustion, oxidation, decomposition.

Chemistry: The Central Science

  • Understanding chemistry helps connect various scientific fields.

Scientific Methodology

  • Observations: Initial data collection guiding hypotheses.

  • Hypothesis: Proposed explanation of observations.

  • Experiment: Testing hypotheses by studying variables.

  • Model Development: Adjusting theories based on experimental outcomes.

Domains of Chemistry

  • Macroscopic Domain: Everyday observable materials.

  • Microscopic Domain: Particles and atoms not visible to the naked eye.

  • Symbolic Domain: Language of chemistry; symbols, formulas, equations.

Classifying Matter

  • Matter Classification:

    • Constant properties & composition: Purity vs. Mixtures.

    • Mixtures: Can be heterogeneous (non-uniform) or homogeneous (uniform).

    • Compounds can be broken down; elements cannot.

Atoms and Molecules

  • Atom: Smallest particle of an element with its properties.

  • Molecule: Composed of multiple atoms bonded together.

Elements and Compounds

  • Elements: Pure substances, cannot be chemically broken down.

  • Compounds: Can be broken down chemically into elements or substances.

Measurement in Chemistry

  • Base Units for length, mass, time, temperature, etc.:

    • Length: meter (m)

    • Mass: kilogram (kg)

    • Time: second (s)

    • Temperature: kelvin (K)

  • Measurement is critical for hypothesis testing and scientific laws.

Density and Volume Calculations

  • Density: Ratio of mass to volume; SI unit: kg/m³.

  • Volume Relationships: Conversions among units like L and m³.

Temperature Scales

  • Kelvin: Absolute scale starting from zero.

  • Celsius: Used globally based on water's freezing/boiling points.

  • Fahrenheit: Common in the USA; differs in degree definition.

Learning Checks and Sample Problems

  • Example problems illustrate applications of chemistry concepts.

Note: The output should be adjusted for clarity, detail, and coherence based on the needs of the student.