Transcript Chapter 2

Chapter 2
• Law of Conservation of Mass
• Law of Definite Proportions
• Law of Multiple Proportions
• Dalton’s Atomic Theory
– Small atoms
– Identical
– Atoms go together to make compounds
– Reactions reorganize atoms
• Avogadro’s hypothesis
– Equal volumes contain equal moles
• Early atom
• Thomson
– CRT
– Electron
– Proton
• Millikan
• Radioactivity
• Rutherford
– Gold Foil Experiment
• Nuclear model
• Modern atomic model
– Electron, Proton, Neutron
– Isotopes
– Atomic symbol
• Molecules and Ions
– Polyatomic ions
• Periodic Table
– Layout
– Families to remember
• Nomenclature
• Binary Ionics
– Type 1 NaCl, MgF2, (NH4)2S
– Type 2 FeO, Fe2O3, AuS
• Polyatomic Ions
• X = Family 17
– XO4- = per _ ate
– XO3- = _ ate
– XO2- = _ ite
– XO- = hypo _ ite
• Sulfate family
– SO42- _ ate
– SO32- _ ite
• Phospate family
– PO43- _ ate
– PO33- _ ite
• Others
– CN - OH - NO3- NO2– MnO4 - CrO4 - Cr2O7 – CO3 - C2O4 - C2H3O2 – NCS- O2 - NH4+ Hg22+
2
2
2
2
2
• Binary Covalents
– 1 mono
– 2 di
– 3 tri
– 4 tetra
– 5 penta
– 6 hexa
– 7 hepta
– 8 octa
– 9 nona
– 10 deca
• CO2, SO3, N2S4
• Acids
– Without oxygen
– Hydro_ic acid
– HCl – hydrochloric acid
– With oxygen
– No hydro and if the polyatomic ends in ate
change to ic if ite change to ous
– HClO3 chloric acid
– H2SO3 sulfurous acid or sulfous acid