Chemical reaction

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Adenosine triphosphate

Glucose

Ch.8 Notes Date Notes Questions 10/12/15 To types of metabolic pathways Catabolic pathways (breaking down, breaking down energy) Anabolic pathways (storing energy, build up) Pathways can be complex and have multiple steps Pathways are the chemical reactions Ex pathways a->b->c-> (a, b and c are chemicals) Living organisms are chemical computers Design like circuit boards Some people working on DNA based computer Also there are works on neuro networks Organisms always share chemicals with everyone Prokaryotes have a much simpler pathways than eukaryotes Metabolic theory that there is a mathematical formula that can explain the interaction of organisms. Energy cannot be created or destroyed Sunlight->Glucose->ATP->Heat Glucose more desired because easiest way to get ATP

Macromolecules worksheet

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Protein

Biomolecular engineering

Macromolecules What are ____________? ____________ are made from thousands or even hundreds of thousands of smaller molecules. Macromolecules are formed by a process known as ____________ in which large compounds are built by joining smaller ones together. Made up ____________, which form ____________. ____________ Groups of Macromolecules There are four groups of macromolecules that make up living things: ____________, ____________, ____________and ____________. Carbohydrates Made up of ____________. Subunit: mono____________ Use for a sources of ____________ Use for ____________ in plants (____________), animals (____________), fungi (____________) and bacteria (____________). Examples: monomers- ____________ ____________- lactose Polymers ?____________

Macromolecules review

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Protein

Biomolecular engineering

Macromolecules What are ____________? ____________ are made from thousands or even hundreds of thousands of smaller molecules. Macromolecules are formed by a process known as ____________ in which large compounds are built by joining smaller ones together. Made up ____________, which form ____________. ____________ Groups of Macromolecules There are four groups of macromolecules that make up living things: ____________, ____________, ____________and ____________. Carbohydrates Made up of ____________. Subunit: mono____________ Use for a sources of ____________ Use for ____________ in plants (____________), animals (____________), fungi (____________) and bacteria (____________). Examples: monomers- ____________ ____________- lactose Polymers ?____________

AP Chemistry MIDTERM review D

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salt

When water evaporates at constant pressure, the sign of the change in enthalpy: a. is negative b. is positive c. depends on the temperature d. depends on the volume of water e. does not exist because the enthalpy change is zero D 100 When water evaporates, the forces holding one water molecule to another water molecule (hydrogen bonds) must be broken. To break these connections, heat energy needs to be added. Therefore this is an endothermic process with a positive delta H. 1 D 200 D 300 2H2S + O2 ? 2S + 2H2O If 102 g of H2S are combined with 64 g of O2, what is the maximum mass of elemental sulfur that could be produced by the reaction? D 400 Fe2O3 + 3CO ? 2Fe + 3CO2

AP Chemistry Zumdahl 7E Chapter 16 Notes

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State functions

Thermodynamic entropy

Chemical thermodynamics

Entropy

Standard molar entropy

gibbs free energy

Enthalpy

Chemical reaction

1 Chapter 16 - Spontaneity, Entropy, and Free Energy 16.1 Spontaneous Processes and Entropy A. First Law 1. "Energy can neither be created nor destroyed" 2. The energy of the universe is constant B. Spontaneous Processes 1. Processes that occur without outside intervention 2. Spontaneous processes may be fast or slow a. Many forms of combustion are fast b. Conversion of diamond to graphite is slow C. Entropy (S) 1. A measure of the randomness or disorder 2. The driving force for a spontaneous process is an increase in the entropy of the universe 3. Entropy is a thermodynamic function describing the number of arrangements that are available to a system a. Nature proceeds toward the states that have the highest probabilities of existing D. Positional Entropy

AP Chemistry Zumdahl 7E Chapter 13 Notes

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Thermodynamic equilibrium

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Equilibrium chemistry

Le Chatelier's principle

Reversible reaction

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 12 Notes

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Rate-determining step

Yield

1 Chapter 12 - Chemical Kinetics 12.1 Reaction Rates A. Chemical kinetics 1. Study of the speed with which reactants are converted to products B. Reaction Rate 1. The change in concentration of a reactant or product per unit of time [ ] t A tt ttimeatAofionconcentratttimeatAofionconcentratRate D D=- -= 12 12 a. Rates decrease with time b. It is customary to express reaction rates as positive values c. Instantaneous rate can be determined by finding the slope of a line tangent to a point representing a particular time C. Decomposition of NO2 2NO2(g) ? 2NO(g) + O2(g) Rate of consumption of NO2 = rate of production of NO = 2(rate of production of O2) [ ]t NO D D- 2 = [ ] t NO D D = [ ] ? ?

Matter - Notes

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Homogeneity and heterogeneity

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Mixture

Separation process

Boiling point

Properties of water

Notes ? Matter Describing Matter Definition - Anything that has mass and takes up space. Matter can be in three states (plasma is another state but exists at high energy that we will not deal with) Solid ? definite shape, definite volume, particles packed closely together Liquid ? indefinite shape, definite volume, particles can flow easily Gas/Vapor ? indefinite shape, indefinite volume, particles are spaced far apart Similar terms but not interchangeable Gases exist as gases at room temperature Vapors are in a gaseous state but generally exist as solids or liquids Characteristic/Physical Properties Physical Properties ? characteristics that are observed but never change for a substance Boiling point (condensation) - temperature at which a liquid turns to a vapor

Raven Biology Chapter 6 Notes

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Adenosine triphosphate

Gavin Morgan 10/28/2015 Chapter 6 2-Point Notes Energy can take many forms: 1. Energy is defined as the capacity to do work. 2. Energy can take many forms: mechanical energy, heat, sound, electric current, light, or radioactivity. The sun provides energy for living organisms: 1. Energy flows into the biological world from the Sun. 2. Breaking the bonds between atoms requires energy. Oxidation-reduction reactions transfer electrons while bonds are made or broken: 1. During a chemical reaction, the energy stored in chemical bonds may be used to make new bonds.

Raven Biology Chapter 2 Notes

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