CHEM 1000 Lecture Notes - Lecture 3: Atomic Theory

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17 Nov 2017
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Chapter 2: Atoms
Sections 2.1-2.6 (Law of: Conservation of Mass, Definite Proportions, Multiple
Proportions; Mole & Avogadro’s number)
Atoms: Greek “Cannot be divided”
Ideas of the atom has changed over time.
Law of Conservation of Mass: Matter is neither created nor destroyed during a chemical
change.
Mass of the products = mass of the reactants
Law of Definite Proportions: A compound always contains the SAME elements in certain
definite proportions
Constant composition
Law of Multiple Proportions: Elements may combine in more than one set of
proportions, with each set corresponding to a different compound (H2O; H2O2)
John Dalton & The Atomic theory of Matter:
1) All matter is composed of extremely small particles called atoms
2) All atoms of a given element are alike and differ from the atoms of any other
element
3) Compounds are formed when atoms of different elements combine in fixed
proportions
4) A chemical reaction involves the rearrangement of atoms
Avogadro’s # (6.022 x 1023) = 1 Mole
6.022 x 1023 atoms of Carbon = 1 mole of carbon
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