'2 br 2' presentation slideshows

Chemical Bonding: Putting it Together 1. chemical bond: -ionic bond: -covalent bond:

Chemical Bonding: Putting it Together 1. chemical bond: -ionic bond: -covalent bond: -Electronegativity: -Polar Covalent: 2. octet rule: EXCEPTIONS 3. Lewis dot structure Formal Charge: Resonance: Isomers:. 4. Types of Bonds: -Single vs. double vs.triple bonds:

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Unit 9: Kinetics and Equilibrium

Unit 9: Kinetics and Equilibrium. Chapter 13 Pre-AP Chemistry I Edmond North High School. Collision Theory. The following three statements summarize the collision theory . 1. Particles must colli de in order to react. 2. The particles must collide with the correct orientation .

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Alkenes, Reactions

Alkenes, Reactions. R-H R-X R-OH R-O-R Alkenes. Acids Bases Metals Oxidation Reduction Halogens. Alkenes, reactions . Addition ionic free radical Reduction Oxidation Substitution. Reactions, alkenes: Addition of hydrogen (reduction).

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Nash Equilibrium: Illustrations

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Chemical Kinetics: Rate Laws ORDER OF REACTION

Chemical Kinetics: Rate Laws ORDER OF REACTION. rate (= ? d [A ] / d t ) = k[A] x [B] y Overall order of reaction = x + y Example: rate = k[A] 2 [B] The reaction is second order in A first order in B overall reaction order = 1+ 2= 3 (sum of the exponents).

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Instructor: Dr. Marinella Sandros

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Kinetics Follow-up

Kinetics Follow-up. Average Rate. Instantaneous rate of reactant disappearance. Instantaneous rate of product formation. Mechanisms. Reactions take place over the course of several steps.

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The balanced chemical equation provides information about the beginning and end of reaction.

Reaction Mechanisms. The balanced chemical equation provides information about the beginning and end of reaction. The reaction mechanism gives the path of the reaction. Mechanisms provide a very detailed picture of which bonds are broken and formed during the course of a reaction.

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Chapter 14 Chemical Kinetics

Chapter 14 Chemical Kinetics. Reaction Coordinate Diagrams. It is helpful to visualize energy changes throughout a process on a reaction coordinate diagram like this one for the rearrangement of methyl isonitrile. Reaction Coordinate Diagrams.

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Reaction Rate

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Lecture 16.1

Lecture 16.1. Chapter 16: Chemical Equilibria. All chemical reactions are reversible, at least in principle.

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Balancing Equations

Balancing Equations. Chemical equation must obey the law of conservation of mass. According to the Law, mass cannot be created or destroyed BALANCED OR NOT BALANCED? Mass of reactants: molar mass of Fe + 2(molar mass of O)= 55.85 g + 2X 16 g = 56 g + 32 g= 88 g

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Balancing Equations

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Reaction Mechanisms

Reaction Mechanisms. Chapter 14. Reaction Mechanisms. The sequence of events that describes the actual process by which reactants become products is called the reaction mechanism. Reaction Mechanisms. Reactions may occur all at once or through several discrete steps.

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Homework

Homework. Chapter 2 Read pages 43-44 WS: Naming molecules Quiz: Next Time! Test Dates: Jan. 17, 18, 19. Acid Worksheet 1. perchloric acid 2. HI 3. phosphoric acid 4. H 2 CO 3 5. hydrocyanic acid 6. HClO 7. HNO 3 8. hydrochloric acid 9. H 3 PO 3 10. HClO 2 11. nitrous acid 12. HBr

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EMPIRICAL FORMULA

EMPIRICAL FORMULA. ANSWERS. 1. Determine the empirical formula of a compound that contains 2.94 g oxygen and 1.96 g sulfur. 2.94 g oxygen x --------------- = 1.96 g sulfur x ----------------- =. 1 mol. 0.184 mol. 16 g. 1 mol. 0.0613 mol.

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7.5-7.6 Types of Reactions and Combination R eactions

7.5-7.6 Types of Reactions and Combination R eactions. By: Kailyn, Kailey, and Aaditi. 7.5 Types of Reactions. Reaction- A process in which atoms of the same or different elements rearrange themselves to form a new substance. Combination Decomposition Combustion Single Replacement

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Decomposition

Decomposition. By Will and Katelyn. Decomposition. In a decomposition reaction , a single compound is broken down into two or more particles. How Decomposition Reactions Occur.

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Termolecular

Termolecular. Fast Initial Step. 2 NO ( g ) + Br 2 ( g ) ??? 2 NOBr ( g ). The rate law for this reaction is found to be Rate = k [NO] 2 [Br 2 ] Because termolecular processes are rare, this rate law suggests a two-step mechanism. Step 1: NO + Br 2. NOBr 2 (fast).

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