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.