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AP Biology

AP Biology. The Study of Life…. AP Biology Framework. Big Idea 1: The process of evolution drives the diversity and unity of life. Big Idea 2: Biological systems utilize free energy and molecular building blocks to grow, to reproduce, and to maintain dynamic homeostasis.

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AP Biology

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  1. AP Biology The Study of Life…

  2. AP Biology Framework • Big Idea 1: The process of evolution drives the diversity and unity of life. • Big Idea 2: Biological systems utilize free energy and molecular building blocks to grow, to reproduce, and to maintain dynamic homeostasis. • Big Idea 3: Living systems store, retrieve, transmit, and respond to information essential to life processes. • Big Idea 4: Biological systems interact, and these systems and their interactions possess complex properties.

  3. Ch. 1 and 2 Recap Summer Homework

  4. Exploring Life CHAPTER 1

  5. OBJECTIVES – YOU MUST KNOW • List (in the correct order) the levels of biological organization. • Determine relationships between organisms using the levels of biological organization. • Describe the characteristics of living things.

  6. 1 The biosphere Figure 1.3 Levels of Biological Organization 2. Ecosystems 3. Communities 4. Populations 5. Organisms

  7. 9Organelles 1 µm Cell 8Cells Atoms 10Molecules 10 µm 7Tissues 50 µm 6Organs and organ systems Figure 1.3

  8. EASY WAY TO REMEMBER… BEC POOT COM

  9. What are the characteristics of living things?

  10. Properties of Life Evolutionary adaptation Order Response to the environment Energy processing Regulation Growth & development Reproduction

  11. the cell theory • All living things are composed of 1 or more cells • Cells are organisms’ basic units of structure and function. • Cells come only from existing cells

  12. How are prokaryotes and Eukaryotes different?

  13. Prokaryotic cell

  14. Eukaryotes

  15. How are proteins made?

  16. DNA and Heritable information • DNA is made of bases that code for Protiens • mRNA is copied from the DNA where is leaves the cell attaches to a ribosome. • tRNA brings amino acids to the site to assemble a protien

  17. What are the taxonomic categories?

  18. GROUPING SPECIES:“HORIZONTAL” DIMENSION OF ORGANIZING LIFE • Domain • Kingdom • Phylum • Class • Order • Family • Genus • Species most inclusive Dumb Kids Playing Chase On Freeways Go Splat OR Dear King Phillip Came Over For Green Soup least inclusive

  19. Species Genus Family Order Class Phylum Kingdom Domain Ursusameri- canus (American black bear) Ursus Ursidae Carnivora Mammalia Chordata Animalia Eukarya Figure 1.14 Classification within Kingdoms

  20. Kingdom Plantae consists of multicellula eukaryotes that carry out photosynthesis, the conversion of light energy to food. 4 µm Bacteria are the most diverse and widespread prokaryotes and are now divided among multiple kingdoms. Each of the rod-shapedstructures in this photo is a bacterial cell. Protists (multiple kingdoms) are unicellular eukaryotes and their relatively simple multicellular relatives.Pictured here is an assortment of protists inhabiting pond water. Scientists are currently debating how to split the protistsinto several kingdoms that better represent evolution and diversity. 100 µm DOMAIN ARCHAEA Kindom Animalia consists of multicellular eukaryotes thatingest other organisms. Kindom Fungi is defined in part by thenutritional mode of its members, suchas this mushroom, which absorb nutrientsafter decomposing organic material. Many of the prokaryotes known as archaea live in Earth‘s extreme environments, such as salty lakes and boiling hot springs. Domain Archaea includes multiple kingdoms. The photoshows a colony composed of many cells. 0.5 µm Figure 1.15 the 3 Domains & their Kingdoms

  21. Figure 1.19 Evolution • accounts for life’s unity and diversity • unity: all species descended from a common ancestor • diversity: modifications that evolved as species branched from their common ancestors • Darwin: “descent with modification”

  22. Chapter 2 The Chemical Context of Life

  23. Objectives- You must Know • The three subatomic particles and their significance • The types of bonds, how they form, and their relative strength

  24. Concept 2.1: Matter consists of chemical elements in pure form and in combinations called compounds • Organisms are composed of matter • Matter is anything that takes up space and has mass • Matter is made up of elements

  25. What are elements? • An element is a substance that cannot be broken down to other substances by chemical reactions • A compound is a substance consisting of two or more elements in a fixed ratio

  26. Sodium Chlorine Sodium chloride

  27. Essential Elements of Life • About 25 of the 92 elements are essential to life • Carbon, hydrogen, oxygen, and nitrogen make up 96% of living matter • Most of the remaining 4% consists of calcium, phosphorus, potassium, and sulfur • Trace elements are those required by an organism in minute quantities

  28. LE 2-3 Nitrogen deficiency Iodine deficiency

  29. Atoms • Atoms are composed of subatomic particles • Relevant subatomic particles include: • Neutrons (no electrical charge) • Protons (positive charge) • Electrons (negative charge) • Neutrons and protons form theatomic nucleus • Electrons form a cloud around the nucleus

  30. Cloud of negative charge (2 electrons) Electrons Nucleus

  31. Atomic Number and Atomic Mass • An element’s atomic number is the number of protons • An element’s mass number is the sum of protons plus neutrons in the nucleus

  32. Isotopes • Isotopes are two atoms of an element that differ in number of neutrons • Most isotopes are stable, but some are radioactive, giving off particles and energy

  33. LE 2-6 Cancerous throat tissue

  34. Valence electrons- those in the outermost shell Helium 2He Hydrogen 1H 2 He 4.00 Atomic number Atomic mass Element symbol First shell Electron-shell diagram Lithium 3Li Beryllium 4Be Boron 5B Carbon 6C Nitrogen 7N Oxygen 8O Fluorine 9F Neon 10Ne Second shell Sodium 11Na Magnesium 12Mg Aluminum 12Al Silicon 14Si Phosphorus 15P Sulfur 16S Chlorine 17Cl Argon 18Ar Third shell

  35. Key Concept: The formation and function of molecules depend on chemical bonding between atoms • Incomplete valence shells allow for shared or transfered valence electrons: Chemical bonds Chemical Bonding

  36. Covalent Bonds • A covalent bond is the sharing of a pair of valence electrons by two atoms

  37. Covalent Bonds • A molecule consists of two or more atoms held together by covalent bonds • A single covalent bond, or single bond, is the sharing of one pair of valence electrons • A double covalent bond, or double bond, is the sharing of two pairs of valence electrons

  38. Name (molecular formula) Electron- shell diagram Structural formula Space- filling model Oxygen (O2)

  39. Name (molecular formula) Electron- shell diagram Structural formula Space- filling model LE 2-11c Water (H2O)

  40. Name (molecular formula) Electron- shell diagram Structural formula Space- filling model LE 2-11d Methane (CH4)

  41. Electronegativity is an atom’s attraction for the electrons in a covalent bond • The more electronegative an atom, the more strongly it pulls shared electrons toward itself

  42. In a nonpolar covalent bond, the atoms share the electron equally • In a polar covalent bond, one atom is more electronegative, and the atoms do not share the electron equally

  43. Ionic Bonds • An ionic bond is an attraction between an anion and a cation • A charged atom (or molecule) is called an ion • An anion is a negatively charged ion • A cation is a positively charged ion

  44. Ionic Bonds Na Cl Na+ Cl– Sodium atom (an uncharged atom) Chlorine atom (an uncharged atom) Sodium ion (a cation) Chlorine ion (an anion) Sodium chloride (NaCl)

  45. Hydrogen Bonds • A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom

  46. Van der Waals Interactions • Molecules or atoms that are very close together can be attracted by fleeting charge differences • Collectively, such interactions can be strong, as between molecules of a gecko’s toe hairs and a wall surface Natural endorphin Morphine Endorphin receptors Brain cell Binding to endorphin receptors

  47. Bond Strength • Between ATOMS • Ionic = strongest • Covalent = weakest • Between COMPOUNDS (dissolving) • Hydrogen Bonds = strongest (created by several covalent) • Ionic = weakest • Salt will dissolve in water • The H and O bonds in water don’t break

  48. Chemical reactions • Chemical reactions lead to new arrangements of atoms • Reactants = The starting molecules • Products = The final molecules

  49. 2 H2 O2 2 H2O Reactants Reaction Products

  50. Some chemical reactions go to completion: All reactants are converted to products • Most chemical reactions are reversible: Products of the forward reaction become reactants for the reverse reaction • Chemical equilibrium is reached when the forward and reverse reaction rates are equal

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