redox

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cellular respiration

Oxidative phosphorylation

Adenosine triphosphate

mitochondrion

ATP synthase

Nicotinamide adenine dinucleotide

Citric acid cycle

Oxygen

Electrochemical gradient

Intermembrane space

OXIDATIVE PHOSPHORYLATION AND ELECTRON TRANSPORT Adenisine Triphosphate (ATP)??-? The molecule from which cells derive energy. Comprised of an adenisine molecule bonded to three phosphates. Each phosphate bond contains energy, especially the third bond. By breaking that one bond and reducing ATP to adenisine?diphosphate (ADP), the cell can get the energy to carry out its various processes. Electron transport chain??-? Term used to describe the flow of electrons generated by the oxidation of NADH and FADH2. Responsible for establishing an electrochemical gradient across the inner mitochondrial membrane that powers the synthesis of ATP in oxidative phosphorylation.

Cellular Respiration

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cellular respiration

Nicotinamide adenine dinucleotide

Adenosine triphosphate

Carbohydrate catabolism

Glycolysis

Citric acid cycle

Cellular Respiration Cellular respiration can be described as a chemical process that breaks bonds in food molecules or transforms chemical energy from organic molecules into ATP. - Only 40% of food energy is extracted and used for cellular work where the other 60% leaves in the form of heat energy ATP= Provides chemical energy for cellular work/processes in the cell. Structure= Composed of complex organic molecule called adenosine with a tail of three phosphate groups and a ribose sugar- pentose (ADP+P=ATP) (ADP is a diphosphate with an adenosine) ATP is recycled from ADP and phosphate through cellular respiration, ADP and P are connected to create ATP to be used for cell processes, ATP is used for cellular work and ADP and P are extracted from food molecules to create ATP again.

AP Chemistry MIDTERM review C

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Gaseous signaling molecules

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Chemical reactions

Refrigerants

Chemical nomenclature

Coordination chemistry

Oxidation state

Hydrogen

Zn + N O 3- + H+ ?Zn2+ + N H 4+ + H 2O Which statement about this reaction is correct? The oxidation number of H changes from +1 to 0 The oxidation number of H changes from +1 to -1 The oxidation number of N changes from +5 to -3 The oxidation number of N changes from +5 to +3 The oxidation number of N changes from +6 to +4 Assign oxidation numbers to each element Zinc goes from 0 to +2 (lost 2 electrons) N goes from +5 to -3 (gained 8 electrons) C 100 0 +5 -2 -3 +1 +1 -2 2H2O2(g) + S(s) ? SO2(g) + 2H2O(g) What is the enthalpy change in the reaction? C 200 Substance ?Hf (kJ/mol) H2O2(g) -150 S(s) 0 SO2(g) -300 H2O(g) -250 -500 kJ -200 kJ 200 kJ 400 kJ 600 kJ [2(-250) + (-300) ] ? [2(-150) + 0] = -500 C 300 CH3CH2OH(g) + ___O2(g) ? ___CO2(g) + ___H2O(g)

AP Chemistry Zumdahl 7E Chapter 17 Notes

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Standard electrode potential

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Electrochemistry

Galvanic cell

Anode

Electrolysis

Cathode

1 Chapter 17 ? Electrochemistry 17.1 Galvanic Cells A. Oxidation-Reduction Reactions (Redox Rxns) 1. Oxidation = loss of electrons a. the substance oxidized is the reducing agent 2. Reduction = gain of electrons a. the subtance reduced is the oxidizing agent B. Redox energy 1. Heat is produced 2. Electricity can be produced if the reactants are separated a. Reactants can be separated by a salt bridge b. Reactants can be separated by a porous partition c. Electrons travel through a wire C. Galvanic Cell 1. A device in which chemical energy is changed to electrical energy a. Oxidation occurs at the anode b. Reduction occurs at the cathode D. Cell Potential (?cell) 1. The driving force (electromotive force, emf) on the electrons 2. Potential is measured in volts

Reactivity of Nuclear Muons

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Chemical reactions

Oxoanions

Oxidizing agents

Equilibrium chemistry

Reducing agents

Chemical equation

Salt metathesis reaction

Carbonate

Sulfuric acid

Aqueous solution

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,

Cellular Respiration

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Oxidative phosphorylation

Chapter 9: Cellular Respiration?Harvesting Chemical Energy Concept 9.6 (176 ? 178) is not required knowledge for the AP? exam and is omitted. Overview: Life Is Work living cells require transfusions of energy from outside sources to perform their tasks energy enters into an ecosystem as sunlight and leaves as heat Concept 9.1: Catabolic pathways yield energy by oxidizing organic fuels Catabolic Pathways and Production of ATP breakdown of organic molecules is exergonic fermentation is a partial degradation of sugars that occurs without oxygen cellular respiration is the most prevalent and efficient catabolic pathway consumes oxygen and organic molecules (i.e. glucose) yields ATP to keep working, cells must regenerate ATP Redox Reactions: Oxidation and Reduction

Chapter 6

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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 11 October 2012 Jespersen, Brady and Hyslop Chapter 6 Oxidation-Reduction Reactions Reactions that involve the transfer of electrons are called oxidation-reduction or redox reactions. Oxidation is the loss of electrons by a reactant. Reduction is the gain of electrons by a reactant LEO the lion goes GER! LEO: Losing Electrons during Oxidation GER: Gaining Electrons during Reduction Redox Reactions Redox Reactions In a balanced redox reaction, the total number of electrons lost by one substance is the same as the total number of electrons gained by the other. Oxidizing agent ? the substance that accepts the electrons. Reducing agent ? the substance that gives up the electrons.

Bob Jones PPT Notes -- Chapter 8c

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Element-reactant-product table

Thermochemical equation

education

Writing Equations Chemical Equations Math equations show equalities. Chemical equations show processes (one chemical changes to another chemical). A Chemical Equation Must: Identify all the substances involved. Show the composition of the substances (use formulas). A Chemical Equation Must: Account for all the atoms. (There must be the same number of atoms of every element on both sides of the equation.) Parts of an Equation Reactants Products Coefficients Arrow Example reactants Ca(HCO3)2 + Ca(OH)2 2 H2O + 2 CaCO3 products The ?2? is a coefficient to tell how many molecules of each compound are present. What tells you how many atoms of an element are in a molecule? Symbol Subscript Coefficient Catalyst Question 7 Special Symbols in Equations g?: A gas was produced.

Bob Jones PPT Notes -- Chapter 8a

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Chemical reactions

Coordination chemistry

ion

Oxide

Chemical Composition &Reactions Oxidation Numbers Keep track of electrons during bonding Tell how many electrons are involved in the bond Tell whether electrons are gained, lost, or unequally shared Oxidation Numbers Help in predicting formulas The more electronegative element gains electrons. The oxidation number of atoms and elements is zero. (free-element) Rule 1 Oxidation Numbers Examples: He ? no bonds O2 ? equal sharing (free-element) Rule 1 Oxidation Numbers The oxidation number of a monatomic ion is equal to the charge of the ion. (ions) Rule 2 Oxidation Numbers Example: Mg loses two electrons, so its charge is +2; therefore, its oxidation number is also +2. (ions) Rule 2 Oxidation Numbers Example: Cl gains one electron, so its charge and oxidation number are ?1. (ions)

Mitochondria Lab

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cellular respiration

Oxidative phosphorylation

biochemistry

Citric acid cycle

Nicotinamide adenine dinucleotide

Chemiosmosis

mitochondrion

Oxygen