blb15_chem_ch01_lecture_ppt_accessible

Page 1: Introduction to Chemistry

• Welcome to Chemistry 1210.

• Course content includes synthetic and organic chemistry.

• Reference link for chemistry outline: https://www.thoughtco.com/what-is-chemistry-p2-604135

Page 2: Office Hours

• Location: SC 020B

• Office Hours:

  • Monday: 3:00-4:20

  • Tuesday: 3:00-4:00

  • Wednesday: 3:00-4:20

  • Friday: 10:00-11:00

Page 3: Textbook Information

• Book Title: Chemistry: The Central Science, Fifteenth Edition

• Available Resources:

  • Inclusive Access for homework and eText available through Canvas

  • Authors: Brown, LeMay, Bursten, Murphy, Woodward, Stoltzfus

Page 4: ACS Exam Preparation

• Title: Preparing for Your ACS Examination in General Chemistry Study Guide, Second Edition

• ISBN: 978-1-7327764-0-1

• Sold through Chem Club ACS. See Dr. Prater in SC 013A for more information.

Page 5: Recommended Calculator

• A scientific calculator is required for the course.

• Graphing calculators are not allowed in exams.

• Final exam requires a department-issued calculator model.

Page 6: Grading Structure

• Homework and Quizzes: 25%

• Midterms: 50%

• Final Exam: 25%

Page 7: Grading Scale

• A: 100-93

• A-: 92.9-90

• B+: 89.9-87

• B: 86.9-83

• B-: 82.9-80

• C+: 79.9-77

• C: 76.9-73

• C-: 72.9-70

• D+: 69.9-67

• D: 66.9-63

• D-: 62.9-60

• F: 0-59.9

Page 8: Homework Guidelines

• Mastering Chemistry available via Canvas.

• It is recommended to work on homework daily; resources include TA, Tutor Center, PAL groups, and office hours.

Page 9: Exams Procedure

• Exams will be administered in the Testing Center located on the 2nd floor of the Electronic Learning Center (ELC).

• Dates for exams must be adhered to, barring university excused absences. Exam accommodations require earlier completion.

Page 10: Mastery Quizzes Data

• Comparison of Mastery Quiz percentages to Exam Scores for Exam 3:

  • Quiz Range: 0-40%: Avg Score 45.7

  • Quiz Range: 40-55%: Avg Score 66.1

  • Quiz Range: 55-70%: Avg Score 79.6

  • Quiz Range: 70-85%: Avg Score 84.5

  • Quiz Range: 85-100%: Avg Score 88.8

Page 11: Final Exam Information

• Location: Same as classroom

• Date and Time: Tuesday, April 22nd, 11:00 – 1:00 pm

• Type: Cumulative multiple choice, standardized exam from the American Chemistry Society (ACS)

Page 12: ACS Study Manual

• ACS study manual available on campus at a lower cost than online.

• Available in SC 013A with Dr. Prater.

Page 13: Final Grades Curving Policy

• Individual exams will not be curved.

• Must complete assignments with at least a 75% average and not have more than 1 missing quiz/assignment.

• Must score above 75% on mastery quizzes and take every exam.

Page 14: Laboratory Information

• Labs commence next week.

• Ensure to take the attendance quiz (deadline on Canvas).

• Purchase lab manual and goggles at the bookstore; lab coats are optional.

• Read and sign safety contract in the lab manual.

• First lab topic: Safety in the Laboratory.

Page 15: Attendance Policy

• Attendance is not mandatory.

• Occasional pop quizzes may be administered.

Page 16: Notifications

• All course notifications will be sent via Canvas.

• Students are responsible for checking announcements.

Page 17: Late Work Policy

• Most submissions will be through Mastering Chemistry.

• A 20% penalty will apply for late submissions per day.

• Other late work requires official documentation from a university official.

Page 18: Extra Credit Policy

• Extra credit isn't expected during the course; if offered, all students will have an equal opportunity to participate.

Page 19: Introduction to Matter, Energy, and Measurement

• Chemistry is the central science.

Page 20: Definition of Chemistry

• Chemistry explores matter, its properties, and the changes it undergoes.

• It fundamentally connects numerous science fields.

Page 21: Classifications of Matter

• Matter: anything with mass and occupies space.

• States of Matter: Solid, Liquid, Gas.

Page 22: Properties of States of Matter

• States Example: Ice (solid), Water (liquid), Water vapor (gas).

• Properties:

  • Volume: Present in all states.

  • Shape: Fixed in solids, variable in liquids and gases.

Page 23: Atoms as Building Blocks

• Atoms are fundamental components of matter; different types represent different elements.

Page 24: Substances and Their Properties

• Substance: Composed of atoms with distinct properties; composition remains consistent across samples.

Page 25: Types of Substances

• Element: Cannot be decomposed into simpler substances.

• Compound: Composed of two or more elements; can be decomposed into simpler substances.

Page 26: Atom and Molecule Composition

• Elements composed solely of one type of atom.

• Compounds consist of at least two different types of atoms.

Page 27: Definition of Molecule

• A molecule consists of two or more covalently bonded atoms.

Page 28: Representation of Atoms and Molecules

• Different colored balls represent different elements; their connections signify molecules.

Page 29: Common Chemical Elements

• Chemists use symbols to represent elements:

  • Carbon (C), Aluminum (Al), Copper (Cu), Iron (Fe), etc.

  • Symbols typically have one or two letters.

Page 30: Element Composition

• 118 named elements exist; five elements constitute 90% of Earth's crust by mass.

• Three elements represent 90% of the human body's mass.

Page 31: Composition of Compounds

• Compounds exhibit definite composition—consistent atom ratios (Law of Constant Composition).

Page 32: Substance Classifications

• Substances categorized as:

  • Pure substances: Made of one type of substance.

  • Mixtures: Composed of two or more substances.

Page 33: Mixtures

• Mixtures show properties of constituent substances; can be homogeneous (uniform) or heterogeneous (varying composition).

Page 34: Classifying Matter

• Decision scheme to classify matter:

  • Element, Compound, Homogeneous Mixture, Heterogeneous Mixture.

Page 35: Practice Problem on Classification

• Classify the following:

  • Silver, an orange, brass, salt water.

Page 36: Distinguishing Matter Classification

• Sample classifications:

  • (a) Molten Iron: Element

  • (b) Chocolate Chip Cookie: Heterogeneous Mixture

  • (c) Ethylene Glycol: Compound

  • (d) Sugar Water: Homogeneous Mixture.

Page 38: Properties of Matter

• Key types of properties:

  • Physical Properties

  • Chemical Properties

Page 39: Physical Properties

• Observable without changing substance.

• Includes color, odor, density, etc.

Page 40: Chemical Properties

• Observed upon altering the substance's composition.

• Examples: flammability, corrosiveness.

Page 41: Physical vs. Chemical Properties

• Intensive Properties: Independent of substance quantity (e.g. density).

• Extensive Properties: Dependent on amount (e.g. mass).

Page 42: Changes in Matter

• Physical Changes: No composition change in substances (e.g. melting, evaporation).

• Chemical Changes: Produce new substances (e.g. combustion).

Page 43: Examples of Physical Change

• State conversions (e.g. melting of ice). Chemical composition remains unchanged.

Page 44: Chemical Reaction Example

• Reaction example: Copper penny reacts with nitric acid to yield a blue solution and nitrogen dioxide.

Page 45: Separation Methods for Mixtures

• Methods: filtration, distillation, chromatography.

Page 46: Filtration Method

• Technique to separate solid substances from liquids or solutions.

Page 47: Distillation Method

• Separates homogeneous liquid mixtures based on differing boiling points.

Page 48: Chromatography Method

• Separates substances by their interaction with a porous solid: a liquid mixture's components adhere differently.

Page 49: Energy Concept

• Energy: Capacity for work or heat transfer.

• Work: energy transfer enforcing displacement.

Page 50: Energy Forms

• Kinetic Energy: Energy of motion (KE = 1/2 mv^2).

• Potential Energy: Stored energy based on object position.

Page 51: Kinetic Energy Calculation

• Kinetic energy formula and understanding units.

Page 52: Importance of Measurement in Chemistry

• The quantitative nature of many chemistry topics necessitates accurate measurement, including:

  • Units of measurement

  • Measured quantities

  • Uncertainty measures

  • Significant figures

  • Dimensional analysis.

Page 53: SI Units Overview

• SI Units (Système International d’Unités): Different base units for different quantities.

Page 54: Metric System Units

• Common Base Units:

  • Mass: gram (g)

  • Length: meter (m)

  • Time: second (s)

  • Temperature: Celsius (℃) or Kelvin (K)

  • Volume: liter (L) or cubic centimeter (cm³).

Page 55: SI Units vs. Metric System

• Comparison of units between SI and metric systems for various physical quantities.

Page 56: Metric System Prefixes (1)

• Prefixes for conversions:

  • Peta (P): 10^15

  • Tera (T): 10^12

  • Giga (G): 10^9

  • Mega (M): 10^6

  • Kilo (k): 10^3.

Page 57: Metric System Prefixes (2)

• Continued prefix list with usage examples for nanowatt through attowatt (n, p, f, a).

Page 58: SI Prefixes Practice

• Identifying unit names for specific exponent values.

Page 59: SI Prefixes Practice Exercises

• Evaluating unit conversions and expressions.

Page 60: Solutions to Practice Exercises

• Calculate results for assorted units and conversions.

Page 61: Mass and Length Units

• Mass defined in SI as kilograms (kg) with metric equivalent as grams (g).

Page 62: Length Units

• Length measurement in meters (m), equating to yards.

Page 63: Volume Measurement

• Volume is a derived from length; commonly used units include L and mL.

Page 64: Glassware for Measuring Volume

• Various equipment for measuring variable and specific volumes in lab settings.

Page 65: Temperature Concept

• Defines temperature as the measure of heat flow from one object to another.

Page 66: Temperature Scales

• Common scientific temperature scales include Celsius and Kelvin.

• Significant points: Water freeze and boil.

Page 67: Kelvin Temperature Scale

• Kelvin is an SI temperature unit—absolute zero defined as 0 K.

Page 68: Practice with Temperature Conversions

• Exercises on converting between temperature scales.

Page 69: Fahrenheit Scale Limitations

• Not typically used in scientific measurements but common in other contexts.

Page 70: Practice on °C and °F Conversions

• Exercises geared to help understand temperature conversions between scales.

Page 71: Temperature Conversion Practice

• Various scenarios on converting °F to K.

Page 72: Density Definition

• Density is a physical property: D = mass/volume.

Page 73: Density Table

• Table listing the density of varying substances at 25 °C.

Page 74: Density Calculation Questions

• Includes different density calculations and examples to solve.

Page 75: Density Sample Exercise

• Example calculations of density and utilizing density for mass or volume determination.

Page 76: Energy Units

• Unit of Energy: Joule (J)—derived unit with relation to mass, distance, and time.

Page 77: Measurement Uncertainty

• Understanding that all measurements contain some inaccuracy and determining significant characters.

Page 78: Exact Numbers in Science

• Exact numbers are clearly defined or counted, possessing infinite significant figures.

Page 79: Inexact Numbers in Science

• Inexact measurements depend on methodology and equipment, allowing for human errors.

Page 80: Significant Figures in Laboratory Measurements

• Practice on how to take accurate volume readings using proper significant figures.

Page 81: Precision vs. Accuracy

• Precision: How closely measurements align with one another.

• Accuracy: How closely measurements reflect the true value.

Page 82: Significant Figures Definition

• All digits in a measured quantity are significant. Rounding adheres to significant figure rules.

Page 83: Rules for Significant Figures

• Rules governing how to count significant figures within numbers and particularly important digits.

Page 84: Examples of Significant Figures

• Examples illustrate correct significant figure analysis in various number formats.

Page 85: Atlantic Pacific Rule Overview

• The method for identifying significant figures based on decimal presence.

Page 86: Pacific Rule for Significant Figures

• If a decimal is present, start counting from the left at the first non-zero digit.

Page 87: Atlantic Rule for Significant Figures

• If decimal absent, count from the right at the first non-zero.

Page 88: Significant Figures Practice Exercises

• Exercises to engage understanding of significance in various numbers.

Page 89: Significant Figures in Multiplication and Division

• Method for significant figure rounding in operations.

Page 90: Multiplication and Division Significant Figure Review

• Explanation clarified through a worked example of finishing calculations.

Page 91: Steps for Significant Figures in Calculations

• Detailed steps on handling multiplication and division within significant figures rules.

Page 92: Further Calculation Examples

• Examples clarifying how to handle significant figures in multi-step calculations.

Page 93: Significant Figures Practice Repeat

• Additional opportunities to practice significant figure concepts.

Page 94: More Practice with Significant Figures

• Continuation of significant figure practice with more examples relating to calculations.

Page 95: Significant Figures in Addition and Subtraction

• Rounding for addition and subtraction follows least significant decimal place rule.

Page 96: Rules for Addition/Subtraction Significant Figures

• Guidelines for maintaining accuracy based on additive/subtractive calculations.

Page 97: Processes for Calculating Significant Figures

• Steps to ensure accuracy post-calculation adherence to significant figure accuracy rules.

Page 98: More Practice on Addition/Subtraction

• Further exercises with attention to significant figures in addition and subtraction contexts.

Page 99: Practice with Addition/Subtraction Examples

• Engaging examples for students to illustrate the rounding needs.

Page 100: Significant Figures Results for Practice Problems

• Presenting the results of additional exercises based on significant figure principles.

Page 101: Significant Figures in Results

• The least certain measurement limits resultant significant figures in answers.

Page 102: Completing Significant Figures in Calculations

• Steps highlighted towards achieving significant figures in compound calculations.

Page 103: Logarithm and Significant Digits

• Logarithmic entries guide counting significant figures from decimals.

Page 104: Dimensional Analysis Overview

• Tools for unit changes through conversion factors provided for depth learning.

Page 105: Dimensional Analysis Continued

• Usage of ratios for converting between units multiple times.

Page 106: Unit Conversion Exercise

• Various applications for understanding dimensional analysis through unit conversion examples.

Page 107: Practice Unit Conversions

• Engaging practice problems focusing on converting common units entirely.

Page 108: Unit Conversion Practice Exercises

• Given various common conversions for practice scenarios.

Page 109: Multi-step Conversion Examples

• Demonstration of multiple conversions within various applications.

Page 110: Additional Unit Conversion Tasks

• Continuation of practice regarding unit conversions emphasizing accuracy and understanding.

Page 111: Energy Change Calculation Sample

• Problem-solving related to changes in energy during chemical reactions.

Page 112: Derived Conversion Factors

• Exercises determining essential conversion factors, elaborating detailed scenarios.

Page 113: Units of Volume Practice Problem

• Application of conversions in understanding volumes toward practical conclusions.

Page 114: Volume-related Problem Solving

• Situational volume calculations that require unit conversions.

Page 115: Volume Conversion Sample Exercise

• Calculation scenarios transforming volume measures from km³ to liters.

Page 116: Density Conversion Exercises

• Solving mass of water in grams based on a volume derived from density.

Page 117: Copyright Information

• Work protected by copyright laws for educational integrity and instructor usage.