GBIO 106 1st EditionExam # 1 Study Guide Lectures: 1 - 7LECTURE 1-Francesco Redi: came up with biogenisis, disproved the idea that living things come from dead things (spontaneous generation). -Characteristics of living things: composed of cells, metabolism, homeostasis (maintaining conditions within an organism), growth, reproduction potential, evolution-Processes of life: movement, ingestion, respiration, excretion and secretion-Hierarchy of life: Cells->tissues->organs->systems->organisms->populations->species-Scientific method: observation, hypothesis WETLANDS SAMPLE EXPERIMENT:Independent Variable: NutriaDependent Variable: Cypress SurvivalNull Hypothesis: Nutria do not influence the survival rate of bald cypress saplings. Alternative Hypothesis: Nutria do influence the survival rate of bald cypress saplings.Two enclosures: One with only plants and nutria, one with everything BUT nutria (control). Conclusion: There is a significant difference in survival between the nutria-influenced trees and the trees in the control batch. LECTURE 2CHEMISTRY: -the study of the composition and reactions of matter-elements: a pure substance that cannot be broken down or converted to other substances by ordinary chemical means-most common elements: carbon, hydrogen, oxygen, nitrogen, phosphorous and sulfur. -atoms: smallest unit of matter --> protons, neutrons and electrons. -atomic number: number of protons in an atom. -atoms are neutral-atomic mass: protons+neutrons-isotopes: type of atom of the same element with the same atomic number but different atomic mass. -radioactive isotopes: isotopes with unstable nuclei that decay and emit radiation. -electron configuration: formation of molecules and compounds-molecule: assembly of two or more atoms. -compound: two or more atoms of different atoms bonded in fixed proportions.-chemical bonds: attractive force that arises between two atoms when their electrons interact. -three types of bonds: ionic, covalent, hydrogen. -ion: has a charge, either positive or negative. -cations: positive, anions: negative. -types of covalent bonds: non-polar and polar-non-polar covalent bonds: results in the equal sharing of electrons-polar covalent bonds: unequal sharing of electrons-electronegative: measure of an atoms tendency to attract electrons from other atoms-hydrogen bonds: weak electrical attractions between "H" and negatively charged atoms of a different molecule. WATER: -cohesion: group effort, water sticks to itself-adhesion: sticky to others, sticks to other substances-surface tension makes it hardLECTURE 3MORE WATER:-High specific heat: Heat that has to be gained or lost to change the temperature of something by one degree. Water is reluctant to gain heat. This is because the hydrogen bonds absorb the heat. Its a heat sink. Also reluctant to lose heat. -High heat of vaporization: When water evaporates it pulls heat away with it. -High heat of fusion: Most solids sink in liquid, since most solids are denser. Water is different because of hydrogen bonding. These bonds do not break when water freezes. There is space though between the water and the bonds. The molecules expand and make the ice less dense than water, which is why ice floats in water. -Water is a universal solvent. Hydrophilic molecules are attracted to water and can be dissolved by water. When salt dissolves in water there is no chemical reaction and can be reverted to its original state. -Hydrophobic molecules repel water and therefore cannot be dissolved by water. Water does not mix with oil, wax, or steroids; these are all lipids. -Ionization of water: breaking apart water. Water breaks apart into ions. Pure water breaks into equal numbers of these ions. Some substances don't release equal numbers of H+ and OH-. These are...ACIDS AND BASES:-Acids: substances that release H ions into solutions when they disassociate.Example: HCL ----> (H+) + (Cl-)-Acids are good for cleaning. But highly dangerous. Acids taste sour, like lemon and vinegar. -Acids release hydrogen ions. -Bases accept hydrogen ions. Example: NaOH ----> (Na+) + (OH-)Example 2: (NH3) + (H+) -----> NH4-Antacids: Stuff like tums, pepto-bismol; all contain a base to counteract the effects of acid. Bases neutralize acids, but you shouldn't take too many antacids because we need acid in our stomachs. -pH measures the number of hydrogen ions in a substance. Something on the pH scale is ten times more acidic than the item below it. 7 is neutral. 6.9-0 are acids, 7.1-14 are bases. -Pure water is neutral because there are equal numbers of hydrogen and hydroxide. -pH is something that organisms need to maintain at safe levels. -Buffers can act like acids when you need an acid, and can act like a base when you need a base. We constantly introduce new things through what we eat, so bufferskeep our pH where we need it to be. Carbonic Acid is an acid that occurs in our blood and acts as a buffer. ORGANIC CHEMISTRY: -Organic molecules are way bigger than inorganic molecules and have to be handled differently. Organic molecules contain carbon, the backbone of life. Carbon can hook up to four other molecules, which is unique. It cannot give or take electrons. So it shares its electrons. -The difference between organic molecules is that the carbons are just accessorized differently from one another. Carbon is just the frame upon which other moleculesare added. -Hydroxyl groups (OH) are polar. They are mainly characterized as alcohol and carbohydrates.-Taking Ethane, and adding a hydroxyl group makes it into Ethanol, an alcohol. -Carboxyl groups (COOH) are mainly characterized as organic acids. Take Ethane and add a carboxyl which makes it into acetic acid, or vinegar. LECTURE 4:Functional Groups: A group of atoms that help determine the characteristics and chemical reactivity of organic molecules.-Hydroxyl groups: (OH) (Polar) Mainly characterizes alcohol and carbs-Carboxyl groups: (COOH) Mainly characterizes organic acids-Methyl groups: (CH3) (Non-polar) Makes molecules hydrophobic (lipids). Classes of Organic Molecules: -Carbohydrates: Organic compounds that may provide energy and structural support. -Monosaccharides: simple sugars with 3-7 carbons. (glucose, fructose).-Glucose: animal blood sugar. Most common monosaccharides in living things. -Isomers: molecules that have the same type and number of atoms, but different structures. -Disaccharides: two monosaccharides covalently bonded together.Glucose+Fructose=Sucrose