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- Principles of Chemistry I
- University of Miami
- Verified Notes
Browse the full collection of course materials, past exams, study guides and class notes for CHM 111 - Principles of Chemistry I at University of Miami verified by our community.
PROFESSORS
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Amy Scott
fall
24Valentine St. Hilaire
fall
2Verified Documents for Amy Scott
Class Notes
Taken by our most diligent verified note takers in class covering the entire semester.
CHM 111 Lecture Notes - Lecture 1: Microsoft Powerpoint, International System Of Units, Filter Paper
Matter: anything that takes up space and has mass. Separation of matter: distillation: to separate a homogeneous mixture of liquids, it is boiled to a
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CHM 111 Lecture Notes - Lecture 2: Decimal Mark, Scientific Notation, Negative Number
Sig figs stands for significant figures: rules: Zeros in front of the first nonzero number are not significant. For numbers greater than 1, all zeros a
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CHM 111 Lecture Notes - Lecture 3: Unified Atomic Mass Unit, Microsoft Powerpoint
Law of conservation of mass: aka dalton"s atomic theory, states that matter is neither created nor destroyed in chemical reactions, total mass of react
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CHM 111 Lecture Notes - Lecture 4: Polyatomic Ion, Molar Mass, Periodic Trends
Atoms at start of reaction will be there at end of reaction (balanced) Electrons can transfer from one atom to the other. Ion: atom(s) with a positive
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CHM 111 Lecture Notes - Lecture 5: Microsoft Powerpoint, Ionic Compound, Sulfite
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CHM 111 Lecture Notes - Lecture 6: Nitrogen Trifluoride, Molar Mass, Chemical Formula
Chapter 3: molecules, compounds, and chemical equations (cont. ) Can be only nonmetals or a nonmetal with a metalloid. Prefixes must be used if multipl
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CHM 111 Lecture Notes - Lecture 7: Chemical Formula, Reagent, Chemical Equation
Chapter 3 (reviewed)/ chapter 4: chemical quantities and aqueous reactions. The relationship between the # of molecules and the # of atoms is used for
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CHM 111 Lecture Notes - Lecture 8: Microsoft Powerpoint, Reagent
Chapter 4: chemical quantities and aqueous reactions (continued) What would result (product) if the limiting reagent reacted: actual yield. The results
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CHM 111 Lecture Notes - Fall 2018 Lecture 10 - Spectator ion, Chemical equation, Precipitation (chemistry)
Chapter 4: chemical quantities and aqueous reactions (continued) Precipitation reactions and predicting precipitation reactions: precipitation reaction
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CHM 111 Lecture 11: CHM 111 lecture #11
Chapter 4 (continued)/ chapter 5: gases: definition: the of an atom if the electrons were completely transported, equation: valence electrons nonbondin
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CHM 111 Lecture Notes - Lecture 12: Van Der Waals Equation, Ideal Gas Law, Kinetic Theory Of Gases
Definition: volume of 1 mole at stp (ideal gas equation results in 22. 4 l) Density at standard conditions: density calculation: d=m/v or d=pmm/rt. Mm=
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CHM 111 Lecture Notes - Lecture 13: Valence Electron, Lewis Acids And Bases, Nonmetal
Chapter 9: chemical bonding (first half of lecture was spent going over exam 1) Lewis model: lewis theory: a simple bonding theory that looks closely a
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CHM 111 Lecture Notes - Lecture 14: Microsoft Powerpoint, Covalent Bond, Formal Charge
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CHM 111 Lecture Notes - Lecture 15: Intermolecular Force, Atomic Orbital, Chemical Polarity
Three states of matter: solid: particles are packed tightly together and cannot move but can vibrate, liquid: particles are closely packed and have som
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CHM 111 Lecture Notes - Lecture 16: Intermolecular Force, Miscibility, Pentane
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CHM 111 Lecture Notes - Lecture 19: Bravais Lattice, Coordination Number, Crystal Structure
Diffraction from a crystal: crystal lattice: the regular arrangements in a crystalline solid. X-ray diffraction analysis: unit cell: smallest unit that
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CHM 111 Lecture Notes - Lecture 20: Intermolecular Force, Microsoft Powerpoint, Dynamic Equilibrium
Chapter 13: solutions: you will get dehydrated if you drink seawater, dehygration will be the result because there will be a higher concentration of sa
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CHM 111 Lecture Notes - Lecture 21: Mole Fraction, Boiling-Point Elevation, Boiling Point
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CHM 111 Lecture Notes - Lecture 22: Equilibrium Constant, Spectrophotometry, Hemoglobin
Hemoglobin equilibrium system: hemoglobin: protein in red blood cells that reacts with o2. Dynamic equilibrium: a reaction that goes both ways. Hb, o2
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CHM 111 Lecture Notes - Lecture 24: Dimensionless Quantity, Equilibrium Constant, Exothermic Process
Chapter 15: chemical equilibrium (review) and practice problems. Reactions where the reactant and product are in different phases. Finding equilibrium
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CHM 111 Lecture 25: Chm111
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CHM 111 Lecture Notes - Lecture 29: Nitric Acid, Acetic Acid, Trioxidane
Hydronium ion: h+ ions react with h2o to create h3o, h+ ions are protons. The reaction: ha (aq) + h2o (l) a- (aq) + h3o+ (aq) The larger the constant,
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CHM 111 Lecture Notes - Lecture 30: Hydrolysis, Lone Pair, Ethylamine
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CHM 111 Lecture Notes - Lecture 31: Titration Curve, Equivalence Point, Titration
Equation: ph = pka + log ([conjugate base] / [acid]) Calculating a new ph: use a stoichiometry calculation, use an equilibrium calulation. Endpoint: th
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