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Chemistry

Chapter 4 Notes

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BIOL 1020 ? CHAPTER 4 LECTURE NOTES Chapter 4: Carbon and the molecular diversity of life Organic Compounds Organic compounds: any compound of carbon and another element or radical Inorganic: any compound that does not contain carbon. Carbon skeletons: the skeletal formula of an organic compound is a shorthand representation of its molecular structure Wide diversity in organic compounds Carbon has diverse bonding patterns. Carbon atomic structure How many valence electrons in a carbon atom? 4 How many covalent bonds can a carbon atom maximum form? 4 Bonding patterns Valence = 4 electrons Different molecular shape: chains, branches, ring, etc. Length difference. Hydrocarbons ? organic molecules consisting of only carbon and hydrogen e.g. propane

Evolution of the Atomic Theory

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Abderites
Ancient Greek philosophers
Amount of substance
Democritus
Atomic theory
Leucippus
Law of definite proportions
Conservation of mass
Antoine Lavoisier
Oxygen
Atomism
Technology

Evolution of the Atomic Theory Democritus and Leucippus 442 BC Stated that: Between atoms lies empty space Atoms are indestructible Atoms have always been and always will be in motion Atoms differ in shape and size ?The more any indivisible exceeds, the heavier it is.? Aristotle 355 BC Came up with the idea that everything was made up of earth, air, fire, and/or water. Antoine Lavoisier 1785 Discovered the Law of Conservation of Mass J. L. Proust 1794 Discovered the law of definite proportions Thomas Young 1801 - 1817 Proved Isaac Newton?s theory, that light is a wave of particles, incorrect and discovered how there was a variation in rays of light due to the size of wavelengths John Dalton 1803 Came up with his own atomic theory that said:

Biology top ten

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Nutrition
Molecular biology
Nitrogen metabolism
Proteins
Proteomics
Amino acid
Peptide
Properties of water
Enzyme
Active transport

Biology Top Ten Elizabeth Kim Natural selection acts on individuals; evolution acts on populations. Water?s polarity contributes to its properties of cohesion and adhesion. Functional groups determine a molecule?s properties ? acidity, baseness. Active transport requires input of free energy while passive transport does not. Each enzyme has a specific function due to distinct shapes of active sites and the substrates that fit into it. Protein is formed from polypeptide chains of their monomers ? amino acids. In early life, as organisms became exposed to a new environment with oxygen, they were able to use photosynthesis to acquire and use energy more efficiently for gaining resources.

Biology Notes

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Cellular respiration
Metabolism
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Integral membrane proteins
Redox
Electron transport chain
Nicotinamide adenine dinucleotide
Oxygen
Chemical bond
Technology

Biology Chapter 6 notes During cellular respirations: electrons are transferred to oxygen as carbon-hydrogen bonds of gloces are broken & hydrogen-oxygen bonds of water form Glucose loses hydrogen atoms as it is converted to carbon dioxide Oxygen gains hydrogen atoms in being converted to water Redox reaction: Electron transfer requires redox reactions for electrons to lose potential energy + release energy Oxidizing glucose: NAD+, dehygrenase Electron transport chain: electrons falling from glucose to oxygen, the transfer of electrons from an organic molecule to NADH Cellular respiration: Glycolysis (cytosol): break glucose into two molecules of pyruvate net product: NADH + ATP

Gas Laws

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Gas laws
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Volume
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Joseph Louis Gay-Lussac
Charles's law

Gas Laws -study the relationships that exist between pressure, volume, temperature and amount (moles) of gas. Boyle?s Law Pressure-volume relationship At constant temperature and amount, the pressure and volume of a gas are inversely proportional. As pressure increases, volume decreases. P1V1=P2V2 Charles? Law Temperature-volume relationship At constant pressure and amount, the temperature and volume of a gas are directly proportional. V1/T1=V2/T2 Gay Lussac?s Law Pressure-temperature relationship Under conditions of constant volume and amount, the temperature and pressure of a gas are directly proportional. P1/T1=P2/T2

Unit 4 Study List: Aqueous Solutions

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Aqueous solution
Solubility
Hydroxide
Acid

AP Chemistry Unit Four: Aqueous Solutions S T U D Y L I S T Properties of Aqueous Solutions ?? Define solute, solvent, and solution. Give examples. ?? Define electrolytes. Give operational and theoretical definitions of electrolytes. ?? Know that soluble ionic compounds and strong acids are strong electrolytes. Ionic compounds of low solubility [e.g. Mg(OH) 2 ] and weak acids/bases are weak electrolytes. ?? Know that molecular compounds (except acids) are non-electrolytes. ?? Know that alcohols (e.g. CH 3 OH )are not ionic hydroxides. Bases are usually metallic hydroxides. ?? Know the solubility rules. State whether an ionic compound is soluble in water. Precipitation Reactions ?? Know that ppt reactions are double

AP Chemistry learning exercise

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Nuclear technology
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Nuclear fuels
Actinides
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Heavy water
Uranium
Deuterium
Properties of water
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Learning exercise

Energy Calculation Problems Problem #1: A cubic block of uranium metal (specific heat = 0.117 J g?1 ?C?1) at 200.0 ?C is dropped into 1.00 L of deuterium oxide of "heavy water" (specific heat = 4.211 J g?1 ?C?1) at 25.5 ?C. The final temperature of the uranium and the deuterium oxide mixture is 28.5 ?C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL) what is the length of the side of the uranium cube? Problem #2: 175.0 g pure H2O was placed in a constant-pressure calorimeter and chilled to 10.0 ?C. 9.80 g pure H2SO4 (also at 10.0 ?C) was added, stirred and the temperature rose to 19.8 ?C. (a) What mass increased in temperature? (b) What was ?t? (c) What was the chemical reaction? (d) What do we assume about the specific heat?

Hydrates Lab

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Evaporating dish
Laboratory glassware
Gauze
Copper
Hydrate
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chemistry hydrates lab

Pre-Lab Title: Hydrates Lab Purpose: This investigation should aid in the understanding of the composition of hydrates and simple decomposition reactions. The purpose is to determine the percent of water in a hydrate. Materials: 1. Evaporating dish 5. Iron Ring 8. Crucible tongs 2. Wire gauze 6. Microspatula 9. Bunsen burner 3. Laboratory balance 7. Safety glasses 10. Ring stand 4. Copper (II) sulfate hydrate Procedure: 1. Prepare the set up shown in figure. 2. Heat the dish with the hottest part of the flames for 3 minutes. 3. Leave the evaporation dish on the gauze and let it cool for 3 minutes.

Bonding General concepts

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bonding
AP Chemistry

Bonding ? General Concepts Electronegativity: The ability of anatom in a molecule to attract shared electrons to itself. Ionic Bonds Electrons are transferred Electronegativity differences are generally greater than 1.7 The formation of ionic bonds is always exothermic! Determination of Ionic Character Compounds are ionic if they conduct electricity in their molten state Electronegativity difference is not the final determination of ionic character Coulomb?s Law ?The energy of interaction between a pair of ions is proportional to the product of their charges, divided by the distance between their centers? There will be a negative sign on the Energy once calculated?it indicates an attractive force so that the ion pair has lower energy than the separated ions.

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