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Equilibrium chemistry

AP Chemistry Zumdahl 7E Chapter 14 Notes

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1 Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry Model 1. Acids are proton donors 2. Bases are proton acceptors 3. H3O+ is called the hydronium ion C. Conjugate Acid-Base Pairs 1. A conjugate base is what remains after an acid has donated a proton a. Cl- is the conjugate base of HCl 2. A conjugate acid is what is formed when a base accepts a proton base acid acid base 3. HCl is a stronger base than H3O+ (H+) so the equilibrium lies far to the right D. Acid Dissociation Constant 1. ][ ]][[ HCl ClHKa -+ = a. water is not included because, in dilute solution, the concentration of

AP Chemistry Zumdahl 7E Chapter 13 Notes

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1 Chapter 13 - Chemical Equilibrium Intro A. Chemical Equilibrium 1. The state where the concentrations of all reactants and products remain constant with time 2. All reactions carried out in a closed vessel will reach equilibrium a. If little product is formed, equilibrium lies far to the left b. If little reactant remains, equilibrium lies far to the right 13.1 The Equilibrium Condition A. Static Equilibrium does not occur in chemical systems 1. No reaction is taking place 2. All product molecules will remain product 3. All unused reactant molecules will remain unreacted B. Dynamic Equilibrium 1. Reactions continue to take place 2. Reactant molecules continue to be converted to product 3. Product continues to be converted to reactant (reverse reaction)

AP Chemistry Zumdahl 7E Chapter 4 Notes

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AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's is low (2.1) 2. Water is a bent molecule 3. Water is a polar molecule B. Hydration of Ionic Solute Molecules 1. Positive ions attracted to the oxygen end of water 2. Negative ions attracted to the hydrogen end of water C. Hydration of Polar Solute Molecules 1. Negative end of polar solute molecules are attracted to water's hydrogen 2. Positive end of polar solute molecules are attracted to water's oxygen D. "Like Dissolves Like" 1. Polar and ionic compounds dissolve in polar solvents like water 2. Nonpolar compounds like fats dissolve in nonpolar solvents like ____ ?_____

Campell9EdChapter3WaterandLife

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Water and Life Chapter 3 Overview: The Molecule That Supports All of Life Water is the biological medium on Earth All living organisms require water more than any other substance Most cells are surrounded by water, and cells themselves are about 70?95% water The abundance of water is the main reason the Earth is habitable ? 2011 Pearson Education, Inc. Figure 3.1 Polar covalent bonds in water molecules result in hydrogen bonding The water molecule is a polar molecule: the opposite ends have opposite charges Polarity allows water molecules to form hydrogen bonds with each other ? 2011 Pearson Education, Inc. Figure 3.2 Hydrogen bond Polar covalent bonds ? ? ? + ? + ? ? ? ? ? + ? + ? ? Four emergent properties of water contribute to Earth?s suitability for life

Bio Inquiry Lab on Enzymes

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Meredith Robbins Inquiry Lab (PH) 10/27/14 Research Question: What conditions would affect the rate of an enzymatic reaction? Null Hypothesis: The Ph and the temperature will not have an effect on the rate of enzymatic reactions. #1 Alternative Hypothesis: The Ph and temperature will have an effect on the rate of enzymatic reactions. #2 Alternative Hypothesis: The Ph and temperature will not have an effect on the rate of enzymatic reactions. Control group: The Ph level of 7 (neutral) Experimental group: Ph- 3, 5, 7, 9, 11 (I will get data for Ph 5 and 7) IV: the Ph level DV: the rate of the enzyme reactions

AP Bio Chp 3

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AP Biology Reading Guide Chapter 3: Water and the Fitness of the Environment Fred and Theresa Holtzclaw Copyright ? 2010 Pearson Education, Inc. - 1 - Name_______________________Period___________ Chapter 3: Water and the Fitness of the Environment Concept 3.1 The polarity of water molecules results in hydrogen bonding 1. Study the water molecules at the right. On the central molecule, label oxygen (O) and hydrogen (H). 2. What is a polar molecule? Why is water considered polar? 3. Now, add + and ? signs to indicate the charged regions of each molecule. Then, indicate the hydrogen bonds. 4. Explain hydrogen bonding. How many hydrogen bonds can a single water molecule form?

Principles of Chemistry Chapter 3

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Chapter 3: Molecules and Chem Equations Section 3.2: Chemical Formulas and Equations Monday, September 8, 2014 2:44 PM Chemical Equations: symbolic representation of a chemical reaction Left side: reactants (original materials) Right side: products (compounds formed from reaction) ? Notation: Reaction w/ heat is indicated by delta Reaction w/ light energy is indicated by hv (called a photochemical reaction) ? Hints: Balance elements that occur in only one compound on each side first Balance free elements last Balance polyatomic ions as groups ? Balancing Chemical Equations Remember LAW OF CONSERVATION OF MATTER Stoichiometry: study of relationships between reactants and products in a chemical reaction (numbers in chem equations are stoichiometric coefficients) ?

Reactivity of Nuclear Muons

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preAP Chem 2013-2014 1 Name ________________________________ Note: It is very important that you note that some elements do not occur as single atoms when by themselves. If they are not combined with another element, they will bond with themselves, forming a _________________ molecule. In any chemical reaction, when you see these elements alone, they must be shown with a diatomic formula. Diatomic elements: H2, N2, O2, F2, Cl2, Br2, I2 I. Describing Chemical Change A. Writing Equations ? words can be used to describe _____________________________, but that can become long and ______________________. ? chemists use ___________________________ to describe reactions. In chemical equations,

Organic Chapter 1 ppt

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Chapter 1 Introduction and Review Organic Chemistry, 6th Edition L. G. Wade, Jr. Chapter 1 * Definitions Old: ?derived from living organisms? New: ?chemistry of carbon compounds? From inorganic to organic, vitalism and W?hler, 1828 => Chapter 1 Chapter 1 * Atomic Structure Atoms: protons, neutrons, and electrons. The number of protons determines the identity of the element. Some atoms of the same element have a different number of neutrons. These are called isotopes. Example: 12C, 13C, and 14C => Chapter 1 Chapter 1 * Electronic Structure Electrons: outside the nucleus, in orbitals. Electrons have wave properties. Electron density is the probability of finding the electron in a particular part of an orbital.

Cell bio chapter 4/5

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Substances found in living tissues Water, macromolecules, proteins, nucleic acids, carbs Concept 4.3 Functional groups Components of organic molecules Involved in chemical reactions Give molecules unique properties Functional groups important in chemistry of life Hydroxyl group, carbonyl group, amino group, carboxyl group Functional groups of sex hormones Functional groups give each molecule unique properties Phosphate group Nucleic acids Adenosine triphosphate (ATP) Concept 4.2 Isomers- compounds with same molecular formula, but different structures and properties Dif shape dif biological abilities Structural isomers- different covalent arrangements of atoms Enantiomers- mirror images of each other Even subtle differences can have different biological response

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