Biochemistry Task 5 Shannon Alford Lipid Storage Molecule Conversion to ATP Lipids (also known as fats) are nonpolar‚ insoluble molecules gained within the body trough digestion of food. Triglycerides‚ a type of lipid that serve as storage units for energy have 3 fatty acid chain tails made up of carboxylic acid and a fatty carbon chain attached to a glycerol backbone. These molecules can be saturated or unsaturated contingent on the bond types and hydrogen number in the molecule. Anytime a fatty
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N10/4/CHEMI/SP2/ENG/TZ0/XX 88106105 CHEMISTRY STANDARD LEVEL PAPER 2 Thursday 11 November 2010 (afternoon) Candidate session number 0 1 hour 15 minutes 0 INSTRUCTIONS TO CANDIDATES • • • • Write your session number in the boxes above. Do not open this examination paper until instructed to do so. Section A: answer all of Section A in the spaces provided. Section B: answer one question from Section B. Write your answers on answer sheets. Write your session number
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Affinity - ability to accept an electron alkaline earth elements have low electron affinities halogens have high electron affinities noble gases have electron affinities near zero other element groups tend to have low electron affinities Electronegativity - measure of the attraction to form a chemical bond increases moving left to right decreases moving top to bottom Stoichiometry: Balance the equation. Convert units of a given substance to moles. Using the mole ratio‚ calculate the moles
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Binary Solutions Composition as a thermodynamic variable Gibbs free energy of binary solutions Entropy of formation and Gibbs free energy of an ideal solution Chemical potential of an ideal solution Regular solutions: Heat of formation of a solution Activity of a component‚ Henry’s and Raoult’s laws Real solutions: interstitial solid solutions‚ ordered phases‚ intermediate phases‚ compounds Equilibrium in heterogeneous systems Reading: Chapter 1.3 of Porter and Easterling‚ Chapters 9.5‚ 9.6‚ 9.9
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HOW DOES THE SOLUBILITY OF POTASSIUM CHLORIDE (KCL) AND POTASSIUM IODIDE (KI) IN WATER VARY WITH TEMPERATURE? AIM To observe solubilities of KCl and KI with water at different temperatures To compare the two solubility curves and discuss what might vary the solubility of different ionic compounds. THE VARIABLES DEPENDENT VARIABLE Temperature INDEPENDENT VARIABLE Amount of solute (KCl‚ KI) CONSTANTS Amount of the solvent (water)‚ pressure APPARATUS 100G OF POTASSIUM CHLORIDE 100G
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Biology Midterm Review Chapter 2- The Chemical Basis of Life 1: Atoms - The smallest functional units of matter that form all chemical substances - Cannot be further broken down into other substances by ordinary chemical or physical means - Each specific type of atom is a chemical element Three Subatomic Particles: - Protons – Positive (+1)‚ found in nucleus‚ same number as electrons - Neutrons – Neutral (0)‚ found in nucleus‚ number can vary - Electrons – Negative (-1)‚ found
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IRON (METAL) Iron is a chemical element with the symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal in the first transition series. It is the most common element (by mass) forming the planet Earth as a whole‚ forming much of Earth’s outer and inner core. It is the fourth most common element in the Earth’s crust. Iron’s very common presence in rocky planets like Earth is due to its abundant production as a result of fusion in high-mass stars‚ Like other group 8 elements‚ iron
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Gas chromatography (GC) is a chromatography technique where the separation of individual components (analytes) from a sample relies on their differing distribution between a mobile and stationary phase. The mobile phase carries the analytes through the stationary phase. In GC‚ it’s an inert gas (usually helium or nitrogen). The gas must be inert‚ so it won’t react with the sample to give a false reading. The stationary phase is a substance fixed in place to which the sample adsorbs because
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DIVISION OF CHEMISTRY :MODULE: GENERAL CHEMISTRY (CHY2021) TUTORIAL # 2 DATE: September 2013 1. Define the following terms: mass number‚ atomic number and the atomic mass unit (amu). 2. With the help of The Periodic Table‚ complete the table below. Symbol Atomic # Proton # Neutron # # of Electrons Mass Number Charge Ar 19 31 17 18 35 20 18 3+ 40 3. In your own words‚ explain Thomson’s and Rutherford’s contribution to the atomic theory. Give sketches to substantiate your answer. 4. Explain
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elements. Some substances are more combustible‚ or able to be burned‚ than other substances. Oxidation state: The difference in the number of electrons associated with an atom as a pure element as compared with that atom in a compound. An element’s electronegativity value and other properties affect its oxidation state in different compounds. Decomposition: Some compounds decompose into more than one different element or compound as bonds are broken. Hydrogen peroxide (H2O2)‚ a chemical you may have around
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