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CHEM 111 (69)
Lecture

Mixtures and compounds, chemical formulae, molar mass, mass percent

4 Pages
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Department
Chemistry
Course Code
CHEM 111
Professor
Dana Johnson

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Description
6 October Announcements ALEKS stuff Exam tonight Check room list (A103) Only pencil, calculator, and ID at your desk So, no sunglasses, hats, water bottles, backpacks, etc. Recitation tomorrow B202 only Starting every hour from 9 am to 3 pm To go over the exam Mixtures and compounds Mixtures – groups of substances that are physically intermingled, can be separated by physical means, can vary in composition Compounds – type of matter composed of elements that are chemically bonded together, cannot be separated by physical means, do not vary in composition Chemical formulae Give information about the identity and number of atoms in a compound Empirical formula – gives the relative number of atoms, such as the ionic formula unit Empirical formula for hydrogen peroxide → HO, showing a one-to-one ratio of atoms Molecular formula – gives the actual number of atoms in a molecule, excludes ionic compounds Molecular formula for hydrogen peroxide → H O2 2 From Monday Mass of compounds given in terms of formula units or molecules Basic formula: Formula / molecular mass = Σ of all atomic masses in the formula unit or molecule The mole revisited “The amount of substance with the same number of entities as there are in 12 g of carbon – 12” The number = Avogadro’s number or 6.022 x 10 23 Weight component essential: One atom of carbon – 12 → 12 amu One mole of carbon – 12 → 12 grams Molar mass The weight of a molecule or formula mass in amu = the weight of one mole of the substanc
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