Che 113

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Chapter 2

• Che 113
• Dr. McGoldricks lecture notes

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Chapter Two Overview

• Classification of Matter
• Fundamental Particles
• Atomic Theory
• Periodic Table
• Lewis Diagrams
• Chart Trends

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Classification

• Impure matter mixtures
• Pure matter -compounds and elements
• Atoms of Life C, H, O, and N

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Daltons Atomic Theory

• Atom is smallest sample of element
• Atoms are indivisible
• Atoms of same element are the same
• Atoms of diff. element are diff.
• Che rxn is a reshuffling of atomic combinations

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Che Laws Revisited

• Conservation Law
• Contstant Composition Law
• Multiple Proportion Law

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Elemental Forms

• Monoatomic ( ex. He, Na)
• Diatomic (ex. H2, O2)
• Triatomic (ex. O3)
• Polyatomic (ex. S8 )

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Fundamental Particles
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Isotopes

• Mass number p n
• Atomic number p
• Isotope Notation
• charge X
• Examples

mass
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Atomic Weight

• Carbon- 12 standard(relative mass)
• Avg. based on abundancy

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The Periodic Table

• Periodicity ( periods, groups)
• Metals, nonmetals, metalloids
• A elements representative
• B elements transition metals
• Group names, main inner transition
  (lanthanides and actinides)memorize A elements

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Development of Modern Atomic Theory

• 1913 Bohr Trilogy- Bohr orbits- Quantization
• 1921 Quantum Mechanics- the probablility picture
• Shells, subshells, orbitals

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Electron Filling

• Electron Configurations
• Orbital Box Diagrams
• Examples all A elements 1st transition (note
  exceptions Cu and Cr)
• USE THE CHART!!

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Lewis Diagrams

• For atoms
• For ions ( cations, anions)
• To be continued with bonding

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Periodic Trends

• Atomic Size Z effective nuclear charge
• Ionization Energy
• Electron Affinity

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End Chapter 2

• Homework
• Test I on Ch 1 and 2

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