SCI 230: Exam 1

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SCI 230: Exam 1
2013-02-07 21:29:52

Chapters 1-3
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  1. Discovery Science
    • Verifiable observations and measurements
    • Describe life in variety of ways
    • "Descriptive science"
  2. Scientific Method
    • Series of steps
    • Observations, hypothesis, experiment, result
  3. Hypothesis
    • A testable statement
    • "If __ occurs, then __ will result."
    • Has to be able to be proven false
  4. Scientific Names
    • Binomial nomenclature
    • Genus = capital letter
    • species = lowercase letter
  5. 3 Domains
    • Domain Bacteria
    • Domain Archaea
    • Domain Eukarya
  6. 4 Kingdoms in Domain Eukarya
    • Plant
    • Fungi
    • Animal
    • Protist
  7. 7 Characteristics of Life
    • Living organisms:
    • 1) Reproduce
    • 2) Grow and develop
    • 3) Process energy
    • 4) Regulation
    • 5) Interact
    • 6) Order
    • 7) Evolutionary Adaptation
  8. Scientific Fact
    An observation that has been repeated confirmed and for all practical purposes is accepted as true.
  9. Scientific Law
    • A descriptive generalization about how some aspect of the natural world behaves under stated circumstances
    • 1st Law of Thermodynamics
  10. Scientific Theory
    • A well-substantiated explanation of some aspect of the natural world that can incorporate facts, laws, inferences, and tested hypothesis.
    • Theory of Evolution
    • Evidence behind it
  11. What is meant by the phrase "science is not set in stone"?
    • The body of knowledge grows and science adapts to this new knowledge
    • Science can change (planets)
    • Body of science tends to be self-correcting
  12. Correlation
    An apparent statistical relationship between variables
  13. Causation
    Established relationship between variables
  14. Protons
    • In nucleus
    • 1 unit of positive charge
  15. Electrons
    • Revolve around nucleus
    • 1 unit of negative charge
  16. Neutrons
    • In nucleus
    • 0 charge
  17. Nucleus
    • Center of atom
    • Made up of protons and neutrons
  18. Electron Shells
    • The number of electrons in the outermost shell determines how the atom reacts
    • with other atoms and molecules
    • If the outermost shell is incomplete, then the atom or molecule is reactive
  19. Isotopes
    Have the same number of protons and electrons, but different number of neutrons
  20. Atomic Number
    Determined by number of protons
  21. Ionic Bonds
    Are ionic compounds that are held together by the attraction of opposite charge
  22. Ions
    Atoms/molecules with a + or – charge
  23. Covalent Bonds
    Share electrons
  24. Hydrogen Bonds
    • Form between water molecules as they align themselves by opposite charges (H +, O -)
    • They stay bonded for only a short time
  25. pH Scale
    • Each pH unit represents a 10-fold change in concentration
    • pH 7 = Neutral
    • pH 2 = Acidic
    • pH 8 = Base
  26. Acid
    • Chemicals that releases H+ to a solution (increase the concentration (relative number) of H+ ions)
    • The more H+ ions, the stronger the acid
  27. Base
    • Chemical bond that accepts H+ ions and removes it from a solution (leaving behind OH- ions)
    • The more OH- ions, the stronger the base
  28. What 4 elements make up 96.3% of our body weight? What 5th element is need in the molecules of life?
    • Oxygen, Carbon, Hydrogen, and Nitrogen
    • Phosphorous
  29. What are the 5 molecules of life given in class?
    • Water
    • Carbohydrates
    • Lipids
    • Proteins
    • Nucleic Acids
  30. Why can isotopes be dangerous?
    • Some are radioactive = Nucleus decays, giving off particles and energy
    • Higher isotopes, more dangerous
  31. What are the similarities and differences between ionic and covalent bonds?
    • Similarities = Both have complete outer shells and positive and negative charges hold them together
    • Differences = I bonds gain and lose electrons, but C bonds don't / I bonds form ionic compounds, but C bonds form molecules
  32. What percentage of Earth is freshwater? What percentage is available to us?
    • Less than 3%
    • Only about 0.5%
  33. What causes water to be a polar molecule?
    • Covalent bond
    • The oxygen atom pulls all the electrons (water = 10e-) much more strongly to them than the hydrogen atoms, so they don’t share the electrons equally.
    • Electrons are mostly on the oxygen, so it shifts to the negative pole
  34. How are hydrogen bonds differ from ionic bonds and covalent bonds?
    • Hydrogen bonds take place between water molecules by opposite charges
    • Ionic = Stronger charge
    • Covalent = Share electrons
  35. Discuss the 4 unique qualities of water that make life possible on Earth with examples.
    • Liquid water is cohesive - H bonds cause water molecules to stick together and pull each other up (Surface tension, moving water in trees)
    • Ice is less dense than liquid water - Water molecules are spread apart, so there are less water molecules in a large space.
    • Water moderates temperature - Water heats up and cools down slowly. (Evaporative cooling - sweating, Coastal Areas)
    • Water is the universal solvent - Many things dissolve in water (H bonds pull Na and Cl into water.)
  36. At what temperature is water most dense?
    Most dense at 4C (39.2F)
  37. What does pH measure?
    The acidity or alkalinity of a solution on a scale in which 7 is neutral, lower values are more acidic and higher values are more basic.
  38. What does each unit of pH represent?
    • It represents a tenfold change in concentration.
    • Lemon juice (pH-2) is 10 times more acidic than grapefruit juice (pH-3)
    • Multiply by 10 for each
  39. What is the "biological range" on a pH scale?
    pH 6.5 - 8.2
  40. What is acid precipitation?
    Rain, snow, or fog has a pH below 5.6.
  41. What causes acid precipitation?
    Caused by sulfur and nitrogen oxides, mostly from burning fossil fuels.
  42. Hydrocarbons
    • Most simple carbon molecules
    • Hydrogen and carbon only4 bonds for each carbon
  43. Monomers
    Subunits of polymers
  44. Polymers
    Molecules built by linking together a large number of subunits
  45. Dehydration Synthesis
    • “To form by removing water”
    • -OH and –H are removed
    • Making water H2O
  46. Hydrolysis
    • Monomers are broken off of polymers using a process
    • Water is added to break the polymer
    • Split into –OH and –H
  47. 3 Types of Carbohydrates
    • Monosaccharides
    • Disaccharides
    • Polysaccharides
  48. Hydrophilic
    • "Water loving"
    • Hydrogen bonds form between oxygen atoms on water or carbohydrate molecules and hydrogen atoms on the other
    • Large molecules attract water, small molecules dissolve in water
  49. Hydrophobic
    • "Fear of water"
    • Molecules are repelled from water
  50. Type of Lipid
  51. Triglyceride
    • 3 fatty acids chains linked to glycerol
    • Main function = Energy storage
  52. How many amino acids are in proteins?
    20 Amino Acids monomers
  53. What are the 4 classes of proteins?
    • Structural – Hair, tendons, silk (spiders)
    • Contractile – Provide movement (muscles)
    • Signaling – Messages within cells and from one cell to another
    • Enzymes – Greatly increase the rate of reactions in cells
  54. Nucleic Acids
    • Information storage in cells
    • Made up of carbon, oxygen, hydrogen,
    • nitrogen, and phosphorus
  55. Nucleotides
  56. How many nitrogenous bases are in proteins?
    There are 5 nitrogenous bases in proteins
  57. 4 Organic Molecules of Life and how each is used in organisms
    • Carbohydrates - Energy and structure
    • Lipids - Energy and structure
    • Proteins - Structure, enzymes, and signaling
    • Nucleic Acids - Storage of genetic information
  58. Why is carbon so important in building these organic molecules?
    • Large amount of energy is stored in the Carbon-Hydrogen bonds
    • This is where most of the energy is stored in macromolecules
  59. 2 differences between hydrocarbons and carbohydrates
    • Carbohydrates are made up of carbon (c),
    • hydrogen (H), and oxygen (O) and hydrocarbons which are hydrogen and carbon only
    • Carbohydrates are our primary source of energy and hydrocarbons is where energy is stored, but can't use the energy
  60. How are dehydration synthesis and hydrolysis used in cells to build and break down polymers? How is water used in each?
    • Polymers are built from monomers through
    • the process of dehydration synthesis.
    •  - “To form by removing water”
    •  - Making water H2O
    • Monomers are broken off of polymers using a process called hydrolysis
    •  - Water is added to break the polymer
  61. Where is most of the energy stored in both hydrocarbons and carbohydrates and fats?
    Hydrocarbons store the most energy
  62. 3 Monosaccharides
    • Glucose
    • Fructose
    • Galatose
  63. 3 Disaccharides and 1 place you might find each
    • Sucrose = Table sugar
    • Maltose = Beer
    • Lactose = Milk sugar
  64. 3 Polysaccharides and how each are used
    • Starch - Storage in plant roots and seeds, found in food (potatoes)
    • Glycogen - Stored in muscle cells for quick energy
    • Celluose - Plant cell walls, wood
  65. What are fatty acids? How do they relate to fats and triglycerides?
    • C=O group plus a hyrdocarbon chain (about 15-18 carbons long)
    • 3 fatty acids chains linked to glycerol - triglycerides (another name for fat)
  66. What is the difference between saturated and unsatured fats?
    • Saturated - Fatty acids filled with the maximum number of hydrogen atoms on the carbon chain
    • Unsaturated - Fatty acid with less than the maximum number of hydrogen atoms on the carbon chain
  67. Why are some fats solid at room temperature and others liquid?
    • Solid - Packed tightly because they are straight lined (saturated)
    • Liquid - Can't pack tightly because they are bent (unsaturated)
  68. What are trans fat? Where do they come from? Why have they gotten so much attention recently?
    • Unsaturated fats that have been partially hydrogenated (H atoms added)
    • Adding H atoms often makes double bonds
    • in the trans configuration (across the bond)
    • Nutrition labels lie about having trans fats or “partially hydrogenated oils or hydrogenated oils.”
  69. What are the 4 levels of structure in protein information?
    • Primary Structure -Unique sequence of amino acids / Different sequence for each protein
    • Secondary Structure - Interactions caused by hydrogen bonds
    • Tertiary Structure - Proteins automatically go into its 3D shape as they are being formed in water
  70. What are the 2 forces that causes proteins to self-construct into their 3D shape?
    • Hydrogen bonds
    • Hydrophobic / hydrophilic interactions
    • Hydrophobic = Inside protein (get away from water), Hydrophilic = Outside protein (attract water)
  71. Why is the 3D shape of a protein so important?
    3-D shape determines the function of the proteins
  72. What are the 3 components of DNA?
    • Sugar
    • Phosphate Group
    • Nitrogenous Base
  73. Which 2 components form the "backbone" of the molecule?
    Sugar and phosphate groups
  74. Which components form bonds across the helix?
    Sugar and phosphate groups
  75. What are the monomers and polymers for carbohydrates, lipids, proteins, and nucleic acids?