BIOM 121 1nd EditionExam # 1 Study Guide Lectures: 1 - 14Lecture 1 (August 27)I. Chemistrya. Rooted in Alchemyi. Alchemy: an ancient practice focused on changing lead into goldb. Scientific Methodi. The Scientific Method: an experimental method for testing based on observation.ii. Theory: a well tested, unifying principle that explains a body of facts.c. It is an observational science.II. Sates of Mattera. Solidi. Are well understoodii. Have a rigid shapeiii. Particles are tightly packed and cannot move past each otherb. Liquidi. Not well understoodii. Are fluid, and do not have a definite shapeiii. Particles can move past each othera. Gas i. Good theoretical understandingii. Takes the shape and volume of its containeriii. Particles move past each other very rapidlyc. All matter is in constant motion, and as temperature increases, speed increases.III. Classification of Mattera. Compound: contains 2 or more elementsb. Molecule: an aggregate of at least 2 atoms in a definite arrangement, smallest form of a compoundc. Elements: substances that cannot be decomposed into other substances, 118 known in 2011d. Atom: the smallest form of an elementIV. Formulasa. Empirical: what is present in what ratios, OHb. Molecular: most common formula, shows the elements and number of each present, H2O2b. Structural: most useful, shows how the elements are bonded together, H – O – O – HLecture 2 (August 29) I. Classifying Matter – Compounds a. Figure out whether you have a pure substance or a mixture.b. Mixtures arei. Homogenous – Uniformed Compositionii. Heterogeneous – Ununiformed CompositionII. Physical Properties of Mattera. Can be measured or observed without changing the composition or identity of the substance. i. Color, state of matter, melting point, boiling point, density, solubility, conductivity, malleability, ductility, and viscosityb. Used for identification of substaces.c. Densityi. Is equal to Mass (g) / Volume (cm3)ii. Most substances get denser as they go from gas to liquid, except water.d. Intensive and Extensive Propertiesi. Intensive: does not depend of quantity of matter (density of a flake of gold, and a gold ring are the same).ii. Extensive: depends on quantity of matter (mass and volume of a flake of gold, are different that the mass and volume of a gold ring).III. Chemical Propertiesa. Describes the ways a substance may change, or react to create new substances.i. Flammability, corrosively, and reactivity.b. Chemical reactions should be balanced.c. These reactions involve changes in energy.IV. Units of Measurementa. There is a metric unit for every quantity that can be measured.i. Mass = Kilogram (kg)ii. Length = Meter (m)iii. Time = Second (sec)iv. Temperature = Kelvin (K)v. Amount of Substance = Mole (mol)vi. Electric Current = Ampere (A)1. Focus on using not memorizing, list will be given.b. Common Prefixesi. Kilo – k – x103ii. Deca – da – x101iii. Deci – d – x10-1iv. Cenit – c – x10-2v. Milli – m – x10-3vi. Micro – μ – x10-6vii. Nano – n – x10-9viii. Pico – p – x10-121. MEMORIZEc. Temperaturei. Celsius and Kelvin1. K = 273.15 + Degrees in Celsius2. 1 Kelvin = 1 Celsiusd. Additional Measurementsi. Volume = 1 cubic centimeter (cm3) = 1 mLii. Mass: measure of quantity of matter contained, grams (g).iii. Weight: a measure of gravitational attraction for the body1. Force = Mass x Gravitational Acceleration iv. Mass is fixed, weight is relative (you weigh less on the moon than on earth, but still have the same mass).e.V. Units of Energya. The primary measurement is the Jouleb. 1 Calorie = the heat required to raise the temperature of 1g of water by 1 degree Celsiusi. 1 kcal = 1 food calorie = 1000 caloriesc. Food and Caloriesi. An average caloric measurement was determined using calorimetry1. 1 g protein = 4 kcal2. 1 g carbohydrate = 4 kcal3. 1 g fat = 9 kcal4. 1 g alcohol = 7 kcalii. Calorimetry: the food is burned and the energy transferred into heat is measuredd. Dimensional Analysis: using conversions to simplify the units the problem is measured in.i. 1 serving of Cheerios has 110 food calories. How many degrees will this amount of energy heat 1 gallon of water?1. 110000 cal x 1 g H2O 1.0 o C x 1 gallon x 1 liter = ?a. 1 gallon 1 cal 3.78 liter 1000 gii. When set up correctly, dimensional analysis eliminates all extra units. VI. Precision and Accuracya. Accuracy: refers to how closely a measured value agrees with the correct value.i. Error in Measure = Experimental Value – Accepted Valueii. Percent Error = (Error in Measure / Accepted Value) x 100b. Precision: refers to how closely individual measurements agree with one anotherc. Standard Deviation = to the square root of: the sum of the squares of the deviation for each measurement from the average, divided by one less that the number of measurements1.a. X = each measurementb. xI = the mean or averagec. n = the number of valuesd. Σ = means we sum across the valuesLecture 3 (August 30)I. The 2 Kinds of Numbersa. Exact: no more, no less, perfectly.i. There are 12 eggs in a dozenb. Inexact: any measurementII. Rules for Significant Figuresa. Leading zeros are never significantb. Imbedded zeros are always significantc. Trailing zeros are only significant if the decimal point is specifiedd. With Scientific Notatione. Adding or subtracting, the last digit retained is set by the digit with fewest digits after decimal (doubtful digit)f. Multiplication or division: answer contains no more significant figures than the least accurately known numberIII. Dimensional Analysis: a problem-solving method that uses the fact that any number or expression can be multiplied by 1 without changing its value.a. Unit Factors: X units / 1 unit or 1 unit/ X units i. May be made from any two terms that describe the same or equivalent "amounts." b. One continuous calculationc. If just 1, number in a calculation has fewer significant figures than every other number in the problem; the answer must have that few significant figures. d. Conversion factors are exact numberse. Look and read instructions carefully for whether it asks for scientific notation or not.Lecture 4 (September 2)I. Radio Activitya. Marie Curiei. Able to show that the atom was charged by deflecting a tight bean with negative and positive plates.b. Sir Joseph John Thomsoni. In an experiment similar to Curies, he was able to determine