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Chapter 3 Slides
Page 1: Introductory Chemistry
Title: Introductory Chemistry, Second Edition, Chapter 3 Lecture Slides
Author: Kevin Revell
©2021 Macmillan Learning
Page 2: Atoms
Atoms are the fundamental building blocks of matter.
Reference to Revell's Introductory Chemistry (2e, 2021).
Page 3: Law of Conservation of Mass
Matter is neither created nor destroyed in chemical reactions.
Key example:
Hydrogen + Oxygen = Water
4.0 g + 32.0 g = 36.0 g
Antoine Lavoisier (1743-1794) is credited with establishing this principle.
Page 4: Example of the Law of Conservation of Mass
When 16.0 grams of methane react with 64.0 grams of oxygen, they yield:
36.0 grams of water and carbon dioxide
Reaction equation: methane + oxygen = carbon dioxide + water
16.0 g + 64.0 g = 44.0 g + 36.0 g
Page 5: Origins of Atomic Theory
John Dalton (1766-1844) proposed key ideas:
Elements consist of tiny indivisible particles called atoms.
Atoms of each element are unique.
Atoms combine in whole-number ratios to form compounds.
Atoms remain unchanged in chemical reactions.
Page 6: Understanding Atomic Theory
Atoms consist of elements that can combine chemically.
Page 7: Three Foundational Ideas
All matter consists of atoms.
Each element's atoms have distinct properties.
Atoms remain unchanged but can form compounds.
Page 8: Can We See Atoms?
Inquiry into the visibility of atoms.
Page 9: Visualizing Atoms
Scientists use X-ray crystallography to visualize atomic arrangements.
Page 10: Periodic Table of Elements
Displays elements arranged by atomic number and properties.
Example elements: F (Fluorine), Cl (Chlorine), Br (Bromine)
Page 11: Continued Periodic Table of Elements
Classification of elements into groups and periods.
Groups: Elements with similar properties.
Periods: Across rows; represent energy levels.
Page 12: Meaning of Periodic
Explanation of the term 'periodic' with reference to calendars.
Page 13: Groups and Periods
Further classification of elements by family groups (e.g., Metals, Nonmetals).
Page 14: Abbreviations for Elements
Symbols for common elements:
Carbon (C), Hydrogen (H), Magnesium (Mg), Calcium (Ca), Sodium (Na), Iron (Fe), Copper (Cu), Lead (Pb).
Page 15: Blocks of Elements
Main groups, transition metals, and inner transition elements are identified.
Page 16: Metals
Metals are located to the left of the periodic table.
Transition metals are highlighted.
Page 17: Nonmetals
Characteristics of nonmetals: located on the upper right of the periodic table.
Page 18: Metalloids
Metalloids are positioned between metals and nonmetals, exhibiting intermediate properties.
Page 19: Group 1A: Alkali Metals
Alkali metals are soft and react violently with water.
Page 20: Group 2A: Alkaline Earth Metals
Less reactive compared to group 1A and burn brightly.
Page 21: Group 7A: Halogens
Halogens exist as diatomic molecules and form various compounds.
Page 22: Group 8A: Noble Gases
Noble gases are stable, rarely form compounds, and are gases at room temperature.
Page 23: Uncovering Atomic Structure
Each element's atoms are unique, and they combine in whole-number ratios.
Page 24: Describing Particles
Particle characteristics:
Mass: atomic mass unit (u) 1 u = 1.66 × 10−27 kg.
Opposite charges attract; like charges repel.
Page 25: Mendeleev's Periodic Table
Historical perspective on the creation of the periodic table.
Page 26: Identification of Charged Particles
Electron: negatively charged particle.
Page 27: Plum Pudding Model
Proposed by Thomson; depicts negative electrons within positively charged material.
Page 28: Alpha Particle Source
Reference to Ernest Rutherford's experiments with alpha particles.
Page 29: Rutherford’s Conclusions
The atom is primarily empty space with a dense nucleus.
Page 30: Model of an Atom
Illustration of atomic structure with a nucleus and electrons.
Page 31: Volume of an Atom
Discussion regarding the spatial volume of atoms.
Page 32: Atomic Particles
Summary of atomic particles:
Proton: mass 1.0073, charge +1
Neutron: mass 1.0087, no charge
Electron: mass 0.0005, charge -1
Page 33: Atomic Particles Continued
Similar information reiterated for clarity.
Page 34: Atomic Identity
The identity of an atom is determined by the number of protons present.
Page 35: Atomic Number and Mass Number
Atomic number: number of protons.
Mass number: total number of protons and neutrons.
Page 36: Isotopes
Isotopes have the same atomic number but varying mass numbers.
Page 37: Writing Atomic Symbols
Methodology for writing atomic symbols based on protons, neutrons, and mass number.
Page 38: Example of Writing Atomic Symbols
Example using uranium's isotope.
Page 39: Average Atomic Mass
Calculation based on the weighted average of isotopes.
Page 40: Example of Weighted Average
Concept of calculating averages illustrated through poker chips analogy.
Page 41: Example of Average Atomic Mass of Carbon
Average atomic mass example utilizing isotopic abundance of carbon.
Page 42: Summary of Atoms and Elements
Key points about atomic identity, atomic number, and isotopes.
Page 43: Ions (Part 1)
Definition of ions: atoms with overall charge due to electron gain/loss.
Page 44: Ions (Part 2)
Definition and characteristics of lithium and its ion.
Page 45: Ions (Part 3)
Description and comparison of fluorine atom and fluoride ion.
Page 46: Example of Ions
Case study on sulfur atom and its sulfide ion formation.
