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Chemat3_LPPT_Ch01
Chapter 1: Matter and Energy - An Atomic Perspective
Page 1
Title: Chemistry: An Atoms-Focused Approach
Authors: Gilbert, Kirss, Bretz, Foster
Edition: Third Edition
Copyright: © 2020 W. W. Norton & Company
Page 2: Particulate Nature of Matter
Atoms: Smallest particle of an element, cannot be chemically or mechanically divided into smaller particles.
Page 3: Elements
Element: A pure substance that cannot be separated into simpler substances.
Page 4: Compounds
Compound: A pure substance composed of two or more elements chemically bonded in fixed proportions.
Page 5: Law of Definite Proportions
Each compound always contains the same proportion of its component elements.
Examples: (a) Solid (b) Liquid (c) Gas
Page 6: Classification of Matter
Pure Substance:
Can it be decomposed by a chemical reaction? No
Can it be separated by a physical process? Yes
Types:
Element: Example - Pure gold,
Mixture: Example - Salad dressing
Mixtures:
Homogeneous: Uniform throughout (Example - Ice)
Heterogeneous: Distinct regions (Example - Vinegar)
Page 7: Scientific Method
Steps:
Observe natural phenomena
Propose a hypothesis
Generate predictions
Design and carry out experiments
Analyze results and refine the hypothesis
Establish a theory and communicate to peers
Page 8: Law of Multiple Proportions
When different masses of one element react with a fixed mass of another, they must be in a small, whole-number ratio.
Page 9: Types of Pure Substances
Examples:
Element: Pure gold (1 Kilo Fine Gold)
Compound: Ice (water)
Page 10: Properties of Pure Substances
Intensive Properties: Independent of the amount of substance.
Extensive Properties: Dependent on the amount of substance.
Physical Properties: Measured without changing the substance.
Chemical Properties: Observable only when reacting with other substances.
Page 11: Density
Formula: Density = mass (m) / volume (V)
Page 12: COAST: A Framework for Solving Problems
Collect & Organize: Identify key concepts; assemble information.
Analyze: Evaluate information; relationships.
Solve: Perform calculations, check units.
Think About It: Consider reasonableness of answer; check units.
Page 13: Sample Exercise 1.1 - Distinguishing Physical and Chemical Properties
Properties of Gold:
(a) Insoluble in water but reacts with aqua regia (chemical)
(b) Melting point 1064°C (physical)
(c) Hammered into sheets (physical)
(d) Reacts with cyanide (chemical)
Page 14: Sample Exercise 1.1 - Continued
Chemical Properties: These indicate how substances react.
Physical Properties: Observable without changing the substance's identity.
Summary of Gold's properties - (a) and (d) are chemical; (b) and (c) are physical.
Page 15: Sample Exercise 1.1 - Solve
Chemical (a, d) and Physical (b, c) properties are identified.
Page 16: Sample Exercise 1.1 - Think About It
Gold jewelry is not soluble in water; alteration of chemical identity is necessary for solubility.
Page 17: Sample Exercise 1.1 - Summary
Chemical properties indicate reactions; physical properties indicate states of matter.
Page 18: Types of Mixtures
Homogeneous Mixture: Uniform composition.
Heterogeneous Mixture: Distinct regions.
Page 19: Separation of Mixtures
Methods include: Distillation, Filtration, Chromatography.
Page 20: Sample Exercise 1.2 - Classifying Classes of Matter
Examples:
(a) Fruit salad - heterogeneous mixture
(b) Filtered air in a scuba tank - homogeneous mixture
(c) Helium gas - element
(d) Dry ice - compound
Page 21: Sample Exercise 1.2 - Organize and Analyze
Classifications based on provided examples.
Page 22: Sample Exercise 1.2 - Solve
Classifications confirmed: Fruit salad (heterogeneous), Filtered air (homogeneous), Helium (element), Dry ice (compound).
Page 23: Sample Exercise 1.2 - Think About It
Distinguishing homogeneous from heterogeneous can be challenging.
Page 24: Sample Exercise 1.2 - Summary
Reinforced classifications based on mixtures and their properties.
Page 25: States of Matter
Solid: Definite shape and volume.
Liquid: Definite volume, shape of container.
Gas: Neither definite volume nor shape.
Page 26: Atomic Color Palette
Color representation of atoms throughout the text.
Page 27: Phase Transformations
Diagrams of sub-processes: Sublimation, Melting, Vaporization.
Page 28: Sample Exercise 1.3 - Distinguishing States of Matter
Identify states and phase changes using diagrams.
Page 29: Sample Exercise 1.3 - Analyze
Space arrangement determines physical states: solid, liquid, gas.
Page 30: Sample Exercise 1.3 - Solve
Solid, liquid, and gas states identified; freezing and sublimation processes explained.
Page 31: Sample Exercise 1.3 - Think About It
Differences in behavior of particles in the three states.
Page 32: Sample Exercise 1.3 - Summary
Summary of particle arrangements and states of matter.
Page 33: Forms of Energy
Energy: Capacity to do work (Work = Force × Distance).
Law of Conservation of Energy: Energy cannot be created or destroyed, only transformed.
Types of Energy:
Potential energy (stored)
Kinetic energy (motion)
Page 34: Formulas and Models
Types of formulas to represent compounds and elements.
Molecular, structural, condensed structural, ball-and-stick, and space-filling models discussed.
Page 35: Ionic Compounds
Contain ions, examples include sodium chloride (table salt).
Page 36: Expressing Experimental Results
Use of SI units for consistency in measurements.
Examples and their SI unit equivalents provided for mass, length, temperature, etc.
Page 37: Metric System Prefixes
Comprehensive table of metric prefixes, conversions, and examples.
Page 38: Temperature Scales
Common scales: Fahrenheit, Celsius, Kelvin.
Page 39: Measurements
Measurement examples illustrating uncertainty in values.
Page 40: Exact Numbers
Definitions and examples of exact numbers, their significance.
Page 41: Precision and Accuracy
Definitions and distinctions between precision (reproducibility) and accuracy (truth to value).
Page 42: Significant Figures
Importance of significant figures in measurements and calculations explained.
Page 43: Rules for Determining Significant Figures
Guidelines on which digits are considered significant.
Page 44: Significant Numbers in Calculations
Guidelines for maintaining significant figures through calculations.
Page 45: Sample Exercise 1.6 - Density Calculation
Density derived from measurements of a gold nugget's mass and displacement in water.
Page 46: Sample Exercise 1.6 - Collect and Organize
Explanation of how density relates to mass and volume.
Page 47: Sample Exercise 1.6 - Analyze
Methodology of calculating density using mass and volume.
Page 48: Sample Exercise 1.6 - Solve
Step-by-step process on calculating density for the gold nugget example.
Page 49: Sample Exercise 1.6 - Think About It
Discusses reasoning regarding gold's density and identity.
Page 50: Sample Exercise 1.6 - Summary
A thorough recap of density calculation and interpretation.
Page 51: Unit Conversions
Importance and application of conversion factors.
Page 52: Dimensional Analysis
Utilization of dimensional analysis for conversions.
Page 53: Sample Exercise 1.7 - Amoxicillin Dosage Calculation
Application of unit conversions to determine dosage.
Page 54: Sample Exercise 1.7 - Collect and Organize
Discusses necessary conversions for amoxicillin dosage.
Page 55: Sample Exercise 1.7 - Analyze
Review of conversion factors and calculations.
Page 56: Sample Exercise 1.7 - Solve
Final calculation for determining dosage in mL.
Page 57: Sample Exercise 1.7 - Think About It
Justification for rounding based on significant digits.
Page 58: Sample Exercise 1.7 - Summary
Collect and summarize the dosing calculation process.
Page 59: Sample Exercise 1.9 - Temperature Conversion
Problem scenario dealing with interstellar space temperature.
Page 60: Sample Exercise 1.9 - Collect and Organize
Preparation for temperature conversion task.
Page 61: Sample Exercise 1.9 - Analyze
Expectations for calculated results based on common knowledge.
Page 62: Sample Exercise 1.9 - Solve
Mathematical steps for converting K to °C and °F.
Page 63: Sample Exercise 1.9 - Think About It
Reasoning for conversion results.
Page 64: Sample Exercise 1.9 - Summary
Summary of temperature conversion task explained clearly.
Page 65: Analyzing Experimental Results: Standard Deviation
Standard deviation as a measure of variation among values; formula provided.
Page 66: Analyzing Experimental Results: Confidence Interval
Definition and parameters for creating confidence intervals.
Page 67: Analyzing Experimental Results: Outliers
Explanation of Grubbs’ test and its application in identifying outliers.
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