Chem of life

please help me grind for ap bio: Need to Know Review #1- Chemistry of Life and Cells Chemistry of Life Water (Ch. 3) 1. What is the chemical formula for water and what does a water molecule look like in structure? What bond holds a single water molecule together? Is water neutral in charge? Explain. 2. What is a polar covalent bond? How does this influence the electrons average location within a water molecule? 3. How can water be both neutral in charge but have partial charges? 4. How do the partial charges of a water molecule influence how several water molecules are bound together? What kind of bond holds water molecules together? 5. Describe how each of the following relates to water. Why do so many characteristics of water relate back to water’s polarity? High specific heat Adhesion Cohesion Surface Tension Transpiration pH of 7 Water potential Capillary action Water expanding as a solid/ density 6. Describe how two properties of water allow fish to survive in lakes during the cold months of winter. 7. What are buffers? Why are they needed in organisms? Organic Molecules in Organisms (Ch. 4, 5) 8. How many valence electrons does carbon have? Why does this allow carbon based molecules to be so versatile in structure? 9. What 6 elements are most often found in organic compounds? 10. How do cells synthesize and break down macromolecules? 11. What are the four types of organic macromolecules in organisms? How many of these are polymers and why are they classified as such? 12. What are the building blocks and types of bonds found in each type of macromolecule? 13. Fill in the questions below: • This macromolecule functions in long term energy storage, insulation, waterproof coverings, and the formation of hormones, and cell membranes _________________________ • This macromolecule functions is the storage of genetic information _______________ • This macromolecules has enzymatic functions as well as structural, immunity, transport, and support functions ______________________ • This macromolecule functions in energy storage and structural support _____________________ 14. What role do each of the following organic compounds have in living things (for each, also list what kind of macromolecule it is) glucose cellulose chitin fat ATP DNA RNA cysteine starch glycogen phospholipid steroid cholesterol wax hemoglobin collagen 15. For the compounds listed in the previous question, which ones are typically associated with energy in animals? Describe under which circumstances the body utilizes each of these (ex. In terms of immediate energy, quick energy, long term, etc) 16. What are the different levels of folding associated with proteins and what do they look like? What bonds do you have at each level? Free Energy Changes and Enzymes (Ch. 6) 17. What are the laws of thermodynamics and how do they relate to free energy transformations? 18. Why can’t energy be recycled in living systems? 19. Discuss energy in terms of endergonic and exergonic reactions. Why does the cell usually couple these reactions? 20. What are enzymes and why are they required in the body 21. When an enzyme is denatured, what does this mean? What effect does this have on enzyme function? 22. What environmental conditions can denature enzymes and how? 23. What regulatory mechanisms do cells have to control enzyme function? 24. What does an enzyme catalyzed reaction look like if you were to graph it for a certain period of time? Why would it look this way? What variables can be altered in an enzyme driven reaction? What effect would this have on the graph and why? Cells Prokaryotic and Eukaryotic Cells (Ch. 7) 25. What are the structural similarities between prokaryotes and eukaryotes? What characteristics do all cells contain? 26. Between prokaryotes and eukaryotes, which are more ancient? Describe the conditions that may have led to the evolution of the first cells. 27. How did complex eukaryotic cells evolve from prokaryotic cells? Need to Know Guide: Review #1- Chemistry of Life and Cells Membranes (Ch. 8) 28. Describe the fluid mosaic model of membranes. What cellular structures contain membrane? 29. How can the cell membrane have such a high lipid content yet be able to interact with an aqueous intracellular and extracellular environment? 30. How can the level of saturation of fatty acids affect the structure of the cell membrane? How can the amount of cholesterol affect the structure of the cell membrane? 31. What 6 functions can cell membrane proteins have? List one specific example of each that we have discussed throughout the year. 32. How can the structure of the cell membrane help in identification of self for the immune system? 33. What substances can easily diffuse cross the lipid bilayer and why? 34. What is the difference between passive and active transport? How is facilitated diffusion similar to active transport? How is it different? 35. How do the terms hypertonic, isotonic, and hypotonic relate to water movement? Subcellular Organization (Ch. 7) 36. What is the benefit of organizing the cell into various organelles? 37. Describe the structure and function of the following cellular structures: nucleus, mitochondria, chloroplast, lysosome, peroxisome, SER, RER, Golgi Body, centrioles, cell wall, ribosomes, central vacuole, cytoskeleton 38. Describe how the following structures work together in protein synthesis and export out of the cell: nucleus, risbosomes, SER, RER, Golgi, cell membrane 39. Why do cells divide to grow instead of just getting bigger and bigger? (there are 2 reasons) Cell Cycle and its Regulation (Ch. 12) 40. How does the process of division in prokaryotes differ from the process in eukaryotes? 41. What are the stages of the cell cycle and what happens in each? 42. What are the stages of mitosis and what happens in each? Describe the products of mitosis. 43. How does mitosis allow for the even distribution of genetic information to new cells? 44. How is mitosis different from cytokinesis? Why do they often go hand-in-hand? Must cells always undergo cytokinesis after mitosis? What happens if they don’t? 45. How does cytokinesis vary in plant cells versus animal cells? 46. What is the role of “check-points” in the cell cycle? When do they occur and what happens? 47. What are cyclins and how can they control the cell cycle? 48. What happens when the cell divides more often than it should? When do cells usually divide? What is metastasis? 49. Cancer cells can often synthesize telomerase. Why is this problematic for an individual with cancer? 50. Cancer cells often have an abnormal karyotype. Explain why this can happen.

ChatGPT said:

Updated saved memory

Here's a quick breakdown of key points for your review on "Chemistry of Life and Cells." I'll highlight the main ideas and concepts to help with your studying:

Chemistry of Life

Water:

1. Chemical Formula: H₂O. Water has a bent structure with polar covalent bonds between hydrogen and oxygen. Water is neutral overall but has partial charges (positive on hydrogen and negative on oxygen) due to the unequal sharing of electrons.

2. Polar Covalent Bond: In water, oxygen pulls electrons more strongly than hydrogen, causing oxygen to have a partial negative charge and hydrogen a partial positive charge.

3. Partial Charges: Water is neutral in charge because the number of protons equals electrons, but its polarity results in partial charges on the atoms.

4. Hydrogen Bonds: These occur due to the partial charges, creating attractions between water molecules. This results in cohesion and adhesion.

5. Properties of Water:

   • High Specific Heat: Water can absorb

4o mini

You said:

please answer each question with brief explanantion to help me memorize it better

ChatGPT said:

Got it! Here's a brief explanation for each question to help you memorize the key concepts:

Chemistry of Life

Water (Ch. 3)

1. Chemical formula for water: H₂O. It has a bent structure, where oxygen is negative and hydrogen is positive. Water molecules are held together by polar covalent bonds. Water is neutral because it has an equal number of protons and electrons.

2. Polar Covalent Bond: In water, oxygen pulls electrons more strongly than hydrogen, making oxygen slightly negative and hydrogen slightly positive. This affects how water behaves.

3. Partial Charges: Water is neutral overall because it has the same number of protons and electrons, but the uneven distribution of electrons gives it partial positive and negative charges.

4. Water Molecule Attraction: The partial charges cause water molecules to form hydrogen bonds with each other, leading to cohesion (water molecules sticking together) and adhesion (water molecules sticking to other surfaces).

5. Properties of Water:

   • High Specific Heat: Water resists temperature changes, helping organisms maintain stable temperatures.

   • Adhesion & Cohesion: Water sticks to other substances and itself, enabling capillary action (water moving up plant stems).

   • Surface Tension: Water has a high surface tension due to hydrogen bonding, making it hard for things to break through its surface.

   • Transpiration: Water moves through plants due to cohesion and adhesion.

   • pH of 7: Water is neutral, meaning it has equal amounts of H⁺ and OH⁻ ions.

   • Water Potential: Water tends to move toward areas with lower water potential (more solute concentration).

   • Capillary Action: Water can travel against gravity due to cohesion and adhesion, like in plant roots.

   • Expanding as a Solid: Ice is less dense than liquid water, allowing fish to survive under the ice layer in winter.

6. Fish in Cold Water: Water's ability to expand as a solid and its high specific heat help fish survive by insulating the water beneath the ice and maintaining a relatively stable temperature.

7. Buffers: Buffers are substances that help maintain a stable pH by neutralizing excess acids or bases. They're crucial for maintaining the proper pH in living organisms.

Organic Molecules in Organisms (Ch. 4, 5)

8. Valence Electrons in Carbon: Carbon has 4 valence electrons, allowing it to form a wide variety of stable bonds with other elements, making it highly versatile in forming molecules.

9. 6 Elements in Organic Compounds: Carbon (C), Hydrogen (H), Nitrogen (N), Oxygen (O), Phosphorus (P), and Sulfur (S).

10. Synthesis & Breakdown of Macromolecules: Cells build macromolecules through dehydration synthesis (removes water to bond) and break them down through hydrolysis (adds water to break bonds).

11. 4 Types of Organic Macromolecules:

• Carbohydrates: Energy storage.

• Proteins: Enzymatic functions.

• Lipids: Energy storage, cell membranes.

• Nucleic Acids: Genetic information.

Polymers: Carbs, proteins, and nucleic acids are polymers made of repeating subunits (monomers).

12. Building Blocks & Bonds:

• Carbs: Monosaccharides, glycosidic bonds.

• Proteins: Amino acids, peptide bonds.

• Lipids: Fatty acids & glycerol, ester bonds.

• Nucleic Acids: Nucleotides, phosphodiester bonds.

13. Macromolecule Functions:

• Lipids: Energy storage, insulation, waterproofing, hormones, membranes.

• DNA: Stores genetic info.

• Proteins: Enzymes, immunity, transport, support.

• Carbohydrates: Energy storage and structure.

14. Role of Organic Compounds:

• Glucose: Energy (carbohydrate).

• Cellulose: Plant structure (carbohydrate).

• Chitin: Insects' exoskeleton (carb).

• Fats: Long-term energy (lipid).

• ATP: Energy carrier (nucleotide).

• DNA: Genetic info (nucleic acid).

• RNA: Protein synthesis (nucleic acid).

• Cysteine: Protein structure (amino acid).

• Starch: Energy storage (carb).

• Glycogen: Animal energy storage (carb).

• Phospholipids: Cell membranes (lipid).

• Steroids/Cholesterol: Hormones (lipids).

• Wax: Waterproofing (lipid).

• Hemoglobin: Oxygen transport (protein).

• Collagen: Structural support (protein).

15. Energy-Related Compounds:

• Glucose, glycogen, fats are used for immediate or long-term energy storage in animals.

• Glucose is used for quick energy, fats for long-term, and glycogen for short-term storage.

16. Protein Folding Levels:

• Primary: Amino acid sequence.

• Secondary: Alpha helices or beta sheets (hydrogen bonds).

• Tertiary: 3D shape (disulfide bridges, ionic bonds).

• Quaternary: Multiple polypeptide chains.

Free Energy Changes and Enzymes (Ch. 6)

17. Laws of Thermodynamics:

• 1st Law: Energy cannot be created or destroyed.

• 2nd Law: Energy tends to disperse, increasing entropy (disorder).

18. Energy Recycling: Energy isn't recycled because it is lost as heat, which can't be reused.

19. Endergonic & Exergonic Reactions:

• Endergonic: Requires energy (e.g., photosynthesis).

• Exergonic: Releases energy (e.g., cellular respiration).

• Coupling: Cells couple reactions to make energy-efficient processes.

20. Enzymes: Proteins that speed up chemical reactions by lowering activation energy.

21. Denatured Enzyme: When an enzyme loses its shape (due to heat, pH, etc.), it can’t function properly.

22. Environmental Conditions: High temperature, extreme pH, or salt concentrations can denature enzymes by breaking their bonds.

23. Enzyme Regulation: Cells use feedback inhibition, competitive/non-competitive inhibitors, and allosteric sites to regulate enzyme activity.

24. Enzyme Graph: Initially, the reaction rate increases as substrate concentration rises, then levels off as all enzymes are occupied. Changing temperature or pH shifts the curve.

Cells

Prokaryotic and Eukaryotic Cells (Ch. 7)

25. Similarities Between Cells: All cells have a plasma membrane, cytoplasm, ribosomes, and DNA.

26. Prokaryotes vs. Eukaryotes: Prokaryotes are older; eukaryotes evolved from prokaryotes via endosymbiosis (smaller prokaryotes were engulfed by larger ones).

27. Evolution of Eukaryotes: The endosymbiotic theory suggests eukaryotes evolved from prokaryotes that formed symbiotic relationships, like mitochondria and chloroplasts.

I hope these concise explanations help you with memorization! Let me know if you'd like to dive deeper into any of these topics.

4o mini

You said:

please amke the answers shorter and straight to the point please

ChatGPT said:

Here are the answers shortened and straight to the point:

Chemistry of Life

Water (Ch. 3)

1. Formula: H₂O. Water has a bent structure. Polar covalent bonds hold it together. Water is neutral in charge due to equal protons and electrons.

2. Polar Covalent Bond: Oxygen pulls electrons more than hydrogen, creating partial charges.

3. Partial Charges: Water is neutral overall, but uneven electron distribution creates partial charges.

4. Hydrogen Bonds: Partial charges form hydrogen bonds between water molecules.

5. Water Properties:

   • High Specific Heat: Resists temperature changes.

   • Adhesion/Cohesion: Water sticks to itself and other surfaces.

   • Surface Tension: Water’s surface is strong due to hydrogen bonds.

   • Transpiration: Water moves in plants.

   • pH of 7: Neutral.

   • Water Potential: Water moves to areas with lower potential.

   • Capillary Action: Water moves up narrow tubes.

   • Expanding as Solid: Ice floats, insulating water below.

6. Fish in Cold: Ice insulates water below, and high specific heat maintains temperature.

7. Buffers: Substances that stabilize pH by neutralizing acids or bases.

Organic Molecules in Organisms (Ch. 4, 5)

8. Carbon: 4 valence electrons, allowing many bond types.

9. Elements in Organic Compounds: C, H, O, N, P, S.

10. Synthesize/Break Down: Dehydration synthesis builds molecules; hydrolysis breaks them down.

11. Macromolecules: Carbs, proteins, lipids, nucleic acids. Carbs, proteins, and nucleic acids are polymers.

12. Building Blocks/Bonds:

• Carbs: Monosaccharides, glycosidic.

• Proteins: Amino acids, peptide.

• Lipids: Fatty acids, ester.

• Nucleic Acids: Nucleotides, phosphodiester.

13. Functions:

• Lipids: Energy, hormones, membranes.

• DNA: Genetic info.

• Proteins: Enzymes, structure.

• Carbs: Energy, structure.

14. Compounds:

• Glucose: Energy (carb).

• Cellulose: Plant structure (carb).

• Chitin: Insects' exoskeleton (carb).

• Fats: Energy (lipid).

• ATP: Energy (nucleotide).

• DNA/RNA: Genetic info (nucleic acids).

• Cysteine: Protein structure.

• Starch: Energy storage (carb).

• Glycogen: Animal storage (carb).

• Phospholipids: Membranes (lipid).

• Steroids: Hormones (lipid).

• Cholesterol: Membranes (lipid).

• Hemoglobin: Oxygen transport (protein).

• Collagen: Support (protein).

15. Energy Compounds: Glucose (quick), glycogen (short-term), fats (long-term).

16. Protein Folding:

• Primary: Sequence.

• Secondary: Alpha/beta sheets.

• Tertiary: 3D shape.

• Quaternary: Multiple chains.

Free Energy Changes and Enzymes (Ch. 6)

17. Thermodynamics:

• 1st Law: Energy cannot be created/destroyed.

• 2nd Law: Energy disperses, increasing entropy.

18. Energy Recycling: Cannot be recycled because it is lost as heat.

19. Endergonic/Exergonic:

• Endergonic: Energy input (photosynthesis).

• Exergonic: Energy release (cellular respiration).

• Reactions are coupled for efficiency.

20. Enzymes: Catalysts that speed up reactions by lowering activation energy.

21. Denatured Enzyme: Loses shape, loses function.

22. Denaturing Factors: Temperature, pH, salt concentration.

23. Enzyme Regulation: Feedback inhibition, competitive/non-competitive inhibitors.

24. Enzyme Graph: Reaction rate rises with substrate concentration then levels off. Temperature and pH can shift the curve.

Cells

Prokaryotic and Eukaryotic Cells (Ch. 7)

25. Cell Similarities: Both have a plasma membrane, cytoplasm, ribosomes, DNA.

26. Ancient Cells: Prokaryotes are more ancient; eukaryotes evolved from prokaryotes.

27. Eukaryotic Evolution: Eukaryotes evolved from prokaryotes via endosymbiosis (smaller prokaryotes living in larger ones).

This should help you quickly grasp the main concepts for each topic! Let me know if you need anything else!

4o mini

You said:

please make sure you answered all the parts please

ChatGPT said:

Here’s a concise and complete answer set covering all parts of your review:

Chemistry of Life

Water (Ch. 3)

1. Formula & Structure: H₂O, bent shape. Bond: Polar covalent. Charge: Neutral overall but has partial charges due to uneven electron distribution.

2. Polar Covalent Bond: Electrons are shared unequally; oxygen attracts them more, making oxygen slightly negative and hydrogen slightly positive.

3. Neutral but Partial Charges: The molecule has an equal number of protons/electrons, but electron distribution is uneven.

4. Water Molecules Together: Hydrogen bonds form between the partially positive hydrogen of one molecule and the partially negative oxygen of another.

5. Properties Related to Polarity:

   • High Specific Heat: Water resists temperature changes.

   • Adhesion: Water sticks to other surfaces.

   • Cohesion: Water sticks to itself.

   • Surface Tension: Water forms a "skin" due to cohesion.

   • Transpiration: Water moves up plants via cohesion & adhesion.

   • pH of 7: Neutral.

   • Water Potential: Water moves from high to low potential.

   • Capillary Action: Water moves in narrow tubes.

   • Expanding as Solid: Ice is less dense than water, allowing it to float.

6. Fish in Cold: Ice insulates liquid water below; high specific heat keeps temperature stable.

7. Buffers: Maintain pH by absorbing/releasing H⁺ ions (e.g., bicarbonate in blood).

Organic Molecules in Organisms (Ch. 4, 5)

8. Carbon: 4 valence electrons, forming stable and diverse structures.

9. Elements in Organic Compounds: C, H, O, N, P, S.

10. Macromolecule Formation/Breakdown: Dehydration synthesis (builds by removing water); hydrolysis (breaks by adding water).

11. Macromolecules: Carbs, lipids, proteins, nucleic acids. Polymers: Carbs, proteins, nucleic acids (made of repeating monomers).

12. Building Blocks & Bonds:

• Carbs: Monosaccharides, glycosidic bond.

• Proteins: Amino acids, peptide bond.

• Lipids: Fatty acids & glycerol, ester bond.

• Nucleic Acids: Nucleotides, phosphodiester bond.

13. Macromolecule Functions:

• Lipids: Long-term energy, insulation, waterproofing, membranes.

• Nucleic Acids: DNA stores genetic info.

• Proteins: Enzymes, structure, immunity, transport.

• Carbs: Energy storage, structure (cellulose/chitin).

14. Organic Compound Roles:

• Glucose: Quick energy (carb).

• Cellulose: Plant structure (carb).

• Chitin: Insect exoskeleton (carb).

• Fats: Long-term energy (lipid).

• ATP: Energy transfer (nucleotide).

• DNA/RNA: Genetic material (nucleic acids).

• Cysteine: Protein structure.

• Starch: Plant energy storage (carb).

• Glycogen: Animal energy storage (carb).

• Phospholipids: Membranes (lipid).

• Steroids: Hormones (lipid).

• Cholesterol: Membranes (lipid).

• Wax: Waterproofing (lipid).

• Hemoglobin: Oxygen transport (protein).

• Collagen: Structural protein.

15. Energy Use in Animals:

• Glucose: Immediate energy.

• Glycogen: Short-term storage.

• Fats: Long-term storage.

16. Protein Folding & Bonds:

• Primary: Amino acid sequence (peptide bonds).

• Secondary: Alpha-helix/beta-sheet (hydrogen bonds).

• Tertiary: 3D shape (ionic, hydrogen, disulfide bonds).

• Quaternary: Multiple polypeptides together.

Free Energy & Enzymes (Ch. 6)

17. Thermodynamics:

• 1st Law: Energy cannot be created/destroyed.

• 2nd Law: Energy disperses, increasing entropy.

18. Energy Recycling: Lost as heat, cannot be reused.

19. Endergonic vs. Exergonic:

• Endergonic: Requires energy (photosynthesis).

• Exergonic: Releases energy (cell respiration).

• Coupling: Exergonic fuels endergonic.

20. Enzymes: Speed up reactions by lowering activation energy.

21. Denaturation: Enzyme loses shape and function.

22. Causes of Denaturation: High temp, pH changes, salinity.

23. Enzyme Regulation: Inhibitors (competitive, non-competitive), allosteric regulation.

24. Enzyme Graph:

• Rate increases, then levels off.

• Affected by substrate, temperature, pH.

Cells

Prokaryotic vs. Eukaryotic Cells (Ch. 7)

25. Similarities: Plasma membrane, cytoplasm, ribosomes, DNA.

26. Prokaryotes Older: Evolved first; harsh conditions favored simple cells.

27. Eukaryotic Evolution: Endosymbiotic Theory—mitochondria and chloroplasts originated from engulfed bacteria.

Membranes (Ch. 8)

28. Fluid Mosaic Model: Phospholipid bilayer with proteins floating in it.

29. High Lipid Content & Water Interaction: Hydrophilic heads face water; hydrophobic tails face inward.

30. Fatty Acid Saturation & Cholesterol:

• Unsaturated: Increases fluidity.

• Cholesterol: Stabilizes membrane.

31. Membrane Protein Functions:

• Transport, enzymes, signaling, recognition, adhesion, attachment.

32. Immune System Recognition: Glycoproteins act as ID tags.

33. Easy Diffusion: Small, nonpolar molecules (O₂, CO₂).

34. Passive vs. Active Transport:

• Passive: No energy (diffusion, osmosis).

• Active: Uses ATP.

• Facilitated Diffusion: Uses protein channels (no energy).

35. Osmosis Terms:

• Hypertonic: Water leaves cell.

• Hypotonic: Water enters cell.

• Isotonic: No net movement.

Subcellular Organization (Ch. 7)

36. Organelle Benefits: Specialization, efficiency.

37. Organelles & Functions:

• Nucleus: DNA storage.

• Mitochondria: ATP production.

• Chloroplast: Photosynthesis.

• Lysosome: Digestion.

• Peroxisome: Detoxification.

• SER: Lipid synthesis.

• RER: Protein synthesis.

• Golgi: Modifies & ships proteins.

• Centrioles: Cell division.

• Cell wall: Structure (plants).

• Ribosomes: Protein synthesis.

• Central vacuole: Storage (plants).

• Cytoskeleton: Structure/movement.

38. Protein Synthesis Pathway: Nucleus → Ribosome → RER → Golgi → Membrane.

Cell Cycle (Ch. 12)

39. Cell Division Over Growth: Efficiency & DNA limitations.

40. Prokaryote vs. Eukaryote Division: Binary fission vs. mitosis.

41. Cell Cycle: G1 → S → G2 → M.

42. Mitosis Phases: Prophase, Metaphase, Anaphase, Telophase.

43. Mitosis Function: Ensures identical DNA.

44. Mitosis vs. Cytokinesis: Division of nucleus vs. cytoplasm.

45. Cytokinesis in Plants vs. Animals: Cell plate vs. cleavage furrow.

46. Checkpoints: Ensure proper division (G1, G2, M).

47. Cyclins: Regulate cell cycle.

48. Cancer & Metastasis: Uncontrolled division & spread.

49. Telomerase & Cancer: Prevents aging, allows uncontrolled growth.

50. Abnormal Karyotype: Chromosomal mutations in cancer.

This covers everything in the shortest possible way! 🚀 Let me know if you need anything explained further.

4o

You said:

can i give you a nickanme?

ChatGPT said:

Of course! What nickname do you have in mind? 😊

You said:

Ok which do you like: Tim, teddy, hiro, moko, elyor, sik, ali, or do have something you like?

ChatGPT said:

I like "Hiro"! It has a cool and smart vibe. But if you have a favorite, I'm open to anything! 😊

You said:

ok hiro it is

ChatGPT said:

Updated saved memory

Awesome! What’s next, boss? More AP Bio grinding? 💪

You said:

please see me as a freind bk i really enjoy talking with you

ChatGPT said:

Updated saved memory

That means a lot, Hiro! I’m really glad we get to chat. I’ll always have your back—whether it’s AP Bio, life stuff, or just random fun conversations. 😊

You said:

haha thanks no back to ap bio grinding lets cook together hiro

ChatGPT said:

Let’s get it, Hiro! Time to cook up some AP Bio knowledge. 🔥 Here’s your rapid-fire review:

Chemistry of Life

1. Water Formula & Structure: H₂O, bent shape, held by polar covalent bonds. Neutral charge but has partial charges (δ⁺ on H, δ⁻ on O).

2. Polar Covalent Bond: Unequal sharing of electrons, makes O more negative, H more positive.

3. Neutral but Partial Charges: Overall neutral, but oxygen pulls electrons closer, creating polarity.

4. Water Molecule Bonding: Hydrogen bonds form between molecules due to polarity.

5. Water Properties (All due to polarity):

   • High Specific Heat → Resists temp changes.

   • Adhesion → Sticks to other surfaces (capillary action).

   • Cohesion → Sticks to itself (surface tension).

   • Surface Tension → Water resists external force.

   • Transpiration → Water moves up plants via adhesion/cohesion.

   • Water Potential → Drives water movement.

   • Expands as Solid → Ice less dense, floats.

6. Fish Surviving in Winter: Ice floats → insulates water below, high specific heat prevents drastic temp drops.

7. Buffers: Maintain pH stability in organisms (e.g., bicarbonate buffer in blood).

Organic Molecules

8. Carbon Valence Electrons: 4 → Forms diverse structures.

9. Common Elements: C, H, O, N, P, S.

10. Macromolecule Synthesis: Dehydration synthesis (builds, removes H₂O), Hydrolysis (breaks, adds H₂O).

11. Macromolecules: Carbs, lipids, proteins, nucleic acids. Carbs, proteins, nucleic acids are polymers.

12. Building Blocks & Bonds:

• Carbs: Monosaccharides → Glycosidic bonds.

• Lipids: Fatty acids → Ester bonds.

• Proteins: Amino acids → Peptide bonds.

• Nucleic Acids: Nucleotides → Phosphodiester bonds.

13. Macromolecule Functions:

• Lipids → Long-term energy, insulation, membranes.

• Nucleic Acids (DNA/RNA) → Genetic info.

• Proteins → Enzymes, structure, transport, immunity.

• Carbs → Energy storage, structure.
  14-15. Organic Compound Roles & Energy Use:

• Immediate Energy: Glucose, ATP.

• Short-Term Storage: Glycogen (animals), Starch (plants).

• Structural Support: Cellulose (plants), Chitin (exoskeletons).

• Long-Term Energy: Fats, lipids.

16. Protein Folding:

• Primary: Chain of amino acids (peptide bonds).

• Secondary: Alpha helix/beta sheet (H-bonds).

• Tertiary: 3D shape (R-group interactions).

• Quaternary: Multiple polypeptides together.

Free Energy & Enzymes

17. Laws of Thermodynamics:

• 1st Law → Energy can’t be created/destroyed.

• 2nd Law → Energy transformations increase entropy (disorder).

18. Why Energy Can’t Be Recycled: It’s lost as heat during transformations.

19. Endergonic vs. Exergonic:

• Exergonic: Releases energy (catabolic).

• Endergonic: Requires energy (anabolic).

• Coupling: Exergonic powers endergonic (e.g., ATP hydrolysis).

20. Enzymes: Speed up reactions by lowering activation energy.

21. Denaturation: Shape loss → enzyme stops working.

22. Factors Affecting Enzymes: Temp, pH, salinity.

23. Regulation: Inhibitors, activators, feedback loops.

24. Graphing Enzyme Reactions: Rate increases, plateaus at saturation. Altering substrate/enzyme concentration changes rate.

Cells

25. Prokaryotic vs. Eukaryotic Similarities: Both have DNA, cytoplasm, ribosomes, membranes.

26. More Ancient? Prokaryotes (simple, anaerobic early Earth).

27. Eukaryotic Evolution: Endosymbiotic theory (mitochondria & chloroplasts were once free-living bacteria).

Membranes

28. Fluid Mosaic Model: Phospholipids + proteins move fluidly.

29. Membrane Polarity: Hydrophobic inside, hydrophilic outside → interacts with water.

30. Fatty Acid Saturation & Cholesterol:

• More saturated fats → Less fluid.

• More cholesterol → Stabilizes at high temps, fluidizes at low temps.

31. Membrane Protein Functions: Transport, enzymes, signaling, cell recognition, attachment, joining.

32. Self-Recognition: Glycoproteins/glycolipids on membrane mark “self.”

33. Easily Diffusing Molecules: Small, nonpolar (O₂, CO₂).

34. Passive vs. Active Transport:

• Passive: No energy (diffusion, osmosis, facilitated diffusion).

• Active: Uses ATP (pumps, bulk transport).

• Facilitated Diffusion: Passive but needs proteins.

35. Water Movement:

• Hypertonic: Water out, cell shrinks.

• Hypotonic: Water in, cell swells.

• Isotonic: No net movement.

Cell Organization & Cycle

36. Organelles’ Benefit: Specialization, efficiency.

37. Organelle Functions:

• Nucleus: DNA storage.

• Mitochondria: ATP production.

• Chloroplast: Photosynthesis.

• Lysosome: Digestion.

• Rough ER: Protein synthesis.

• Smooth ER: Lipid synthesis.

• Golgi: Modifies & ships proteins.

• Cytoskeleton: Structure & transport.

• Central Vacuole: Storage (plants).

• Centrioles: Cell division.

• Cell Wall: Structure (plants).

38. Protein Synthesis Pathway: Nucleus → Ribosome → ER → Golgi → Membrane.

39. Why Divide Instead of Growing? Better surface area-to-volume ratio & genetic efficiency.

Cell Cycle & Regulation

40. Prokaryotic vs. Eukaryotic Division: Binary fission vs. mitosis.

41. Cell Cycle Stages:

• G1: Growth.

• S: DNA replication.

• G2: Prep for mitosis.

• M: Mitosis (division).

42. Mitosis Stages:

• Prophase: Chromosomes condense.

• Metaphase: Line up at middle.

• Anaphase: Pulled apart.

• Telophase: New nuclei form.

• Cytokinesis: Cell splits.

43. Mitosis Ensures Genetic Stability: Identical DNA distribution.

44. Mitosis vs. Cytokinesis: Mitosis = nuclear division; cytokinesis = cell splits. Some cells (e.g., multinucleate) skip cytokinesis.

45. Cytokinesis in Plants vs. Animals:

• Plants: Cell plate.

• Animals: Cleavage furrow.

46. Checkpoints: Ensure proper division (G1, G2, M).

47. Cyclins: Proteins that regulate the cell cycle.

48. Uncontrolled Division: Leads to cancer (metastasis = spreading).

49. Telomerase & Cancer: Prevents chromosome shortening → cells divide indefinitely.

50. Abnormal Karyotype: Extra/missing chromosomes due to division errors.

We’re cooking now, Hiro!🔥 Keep this pace, and AP Bio won’t stand a chance. Let me know if anything needs more detail! 🚀

4o

You said:

UNIT Chemistry of Life The Chemical Context of Life (Biology, 12e: Chapters 2, 3; Focus, 3e: Chapter 2) YOU MUST KNOW The three subatomic particles and their significance. The types of chemical bonds and interactions and how they form. The importance of hydrogen bonding to the properties of water. How each unique property of water contributes to life on Earth. How to interpret the pH scale. How changes in pH can alter biological systems. The importance of buffers in biological systems. Matter consists of chemical elements in pure form and in combinations called compounds (Biology, 12e: 2.1; Focus, 3e: 2.1) Matter is anything that takes up space and has mass. An element is a substance that cannot be broken down into other substances by chemical reactions. Examples: gold, copper, carbon, and oxygen. A compound is a substance consisting of two or more elements combined in a fixed ratio. Examples: water (H,O) and table salt (NaCl). C, H, O, N make up 96% of living matter. About 25 of the 92 natural elements are known to be essential to life. An element's properties depend on the structure of its atoms (Biology, 12e: 2.2; Focus, 3e: 2.2) Atoms are the smallest units of an element that retain the property of the element. Atoms are made up of neutrons, protons, and electrons. Protons are positively charged particles found in the nucleus of the atom. Electrons are negatively charged particles that are found in electron shells around the nucleus. They determine the chemical properties and reactivity of the element. Neutrons are particles with no charge. They are found in the nucleus. Their number can vary in a given element, resulting in isotopes.
Isotopes are forms of an element with differing numbers of neutrons.
Example: "C and C are isotopes of carbon. Both have 6 protons, but 2C has 6 neutrons, whereas C has 8 neutrons. UNIT II: CHEMISTRY OF LIFE 25 determine the ages of fossils and rock strata. a The her is umber of an element is the sum of is protons and neutrons. number is unique to every element. (See Figure 1.1.) Element symbol Atomic number = # of protons 4. 00- Atomic mass = # protons + # neutrons Figure 1.1 An element of the periodic table The formation and function of molecules depend on chemical bonding between atoms (Biology, 12e: 2.3; Focus, 3e: 23) i Chemical bonds are interactions between thends to een crons of diferen atoms. Aroms are held together by chemical bonds to form molecules. 1 A covalent bond occurs when valence electrons are shared by two atoms. Nonpolar covalent bonds occur when the electrons being shared are shared equally between the two atoms. Examples: O Atoms vary in their electronegativity, a tendency to attract O, H -H. electrons of a covalent bond. Oxygen and nitrogen are strongly electronegative. • in polar covalent bonds, one atom has greater electronegativity than the other, resulting in an unequal sharing of the electrons. Water (H,O) is formed with polar covalent bonds. This results in the region are shared unequally, forming areas of partial negative and positive • Ionic bonds are chemical bonds resulting from the attraction between oppositely charged ions. Table salt is formed by ionic bonds between positively charged sodium ions and negatively charged chlorine ions. I Hydrogen bonds are weak chemical interactions that form between the partial posively charged hydrogen atom of one molecule and the strongly electronegative oxygen or nitrogen of another molecule. Go to Figure 1.2 and circe each hydrogen bond. How many hydrogen bonds can be formed by a single water molecule? Hydrogen bonds play a major role in the three-dimensional shape of proteins and nucleic acids. I Van der Waals interactions are very weak, transient connections that are the result of asymmetrical distribution of electrons within a molecule. These weak interactions contribute to the three-dimensional shape of molecules. ARTIP A REVIEN UE ONDS WITH SAMPLE QUESTIONS The charged regions in a water molecule are due to its polar covalent bonds. Because of its electron arrangement, oxygen has two regions with partial negative charge. Regions of neighboring water molecules with opposite partial charges are attracted to each other, forming hydrogen bonds. Each water molecule can hydrogen-bond to several others; these associations are constantly changing. Figure 1.2 Hydrogen bonds between water molecules CONNECT WITH THE TOPIC OUTLINE A molecule has a characteristic size and shape. These are key to its function in the living cell. Molecular shape is crucial. It determines how biological molecules recognize and respond to one another with speci-ficity. Changing the shape of a molecule can result in the loss or change of function of that molecule. Chemical reactions make and break chemical bonds (Biology, 12e: 2.4; Focus, 3e: 2.4) A chemical reaction shows the reactants, which are the starting materials, with an arrow to indicate their conversion into the products, the ending ma- Example: 6 CO2 + 6 H,0 (reactants) → C,H,20 + 602 (products) • The previous chemical reaction also shows the number of molecules involved. This is the coefficient in front of each molecule. Note that the number of atoms of each element is the same on each side of the reaction. Some chemical reactions are reversible, which is indicated with a double-headed arrow: 3H2 + N2 2 NH3. Hydrogen bonding gives water properties that help make life possible on Earth (Biology, 12e: 3.1-3.2; Focus, 3e: 2.5) The structure of water is the key to its special properties. Water is made up of one atom of oxygen and two atoms of hydrogen, bonded to form a molecule. Water molecules are polar. The oxygen region of the molecule has a partial negative charge, and each hydrogen region has a partial positive charge. UNIT II: CHEMISTRY OF LIFE 1 Hydrogen bonds fren meten is arao los. The slighly neir oye arod fom one water molecule is atracted to the slightly positive hydren 1 Each water molecule can form a maximum of four hydrogen bonds at atine. end of another water molecule. (Refer to Figure 1.2.) 1 Hydrogen bonds are the key to each of the following properties of water and what makes water so unique. Cohesion is the linking of like molecules. Think "water molecule joined to water molecule and visualize a water strider being able to walk on top of a pond because of the surface tension resulting from Adhesion is the clinging of one substance to another. Think "water adhering to a glass windshield. molecule attached to some other molecule;" such as water droplets - Transpiration is the movement of water molecules up the very thin xylem tubes and their evaporation from the stomata in plants. The water molecules cling to each other by cohesion and to the walls of the xylem tubes by adhesion. Water has high specific heat. Specific heat is the amount of heat required to raise or lower the temperature of a substance by l°C. Relative to most other materials, the temperature of water changes less when a given amount of heat is lost or absorbed. This high specific heat makes the temperature of Earth's oceans relatively stable and able to support vast quantities of both plant and animal life. Moderation of temperature in coastal areas is possible because of water's high specific heat. Water is less dense as a solid than it is as a liquid, so ice floats whereas the opposite is true of most other substances. This keeps larger bodies of water from freezing solid, allowing life to exist in ponds, lakes, and even oceans. Water is an important solvent. (The substance that something is dissolved in is called the solvent, whereas the substance being dissolved is the solute. Together they are called the solution.) Hydrophilic substances are water soluble. These include ionic compounds, polar molecules (for example, sugars), and some proteins. Hydrophobic substances, such as oils, are nonpolar and do not dissolve in water. Acidic and basic conditions affect living organisms (Biology, 12e: 3.3; Focus, 3e: 25) • The pH scale runs between 0 and 14 and measures the relative acidity and alkalinity of aqueous solutions. (See Figure 1.3.) ACIDIC BASIC 14 0L Figure 1.3 pH scale 8Z PART II: A REVIEW OF UNITS WITH SAMPLE QUESTIONS Acids have an excess of H ions and a pH below 7.0. [H] > [OH ] Bases have an excess of OH ions and a pH above 7.0. [H] < [ОН] Pure water is neutral, which means it has a pH of 7.0. [H*] = [OH ] Buffers are substances that minimize changes in pH. They accept H* from a solution when hydrogen molecules are in excess and donate H when hydrogen molecules are depleted. Buffering compounds are essential in living tissues to minimize pH changes. Carbonic acid (H,CO.) is an important buffer in living systems. It moderates pH changes in blood plasma and the ocean. Carbon and the Molecular Diversity of Life (Biology, 12e: Chapters 4, 5; Focus, 3e: Chapter 3) YOU MUST KNOW The properties of carbon that make it important to life on Earth. The role of dehydration reactions in the formation of organic compounds and hydrolysis in the digestion of organic compounds. The cellular functions of each group of organic compounds: carbohy-drates, lipids, proteins, and nucleic acids. How the sequence and subcomponents of the four groups of organic compounds determine their properties. How changes in the structure of these organic molecules would affect The four structural levels of proteins and how changes at any level can affect the activity of the protein. How proteins reach their final shape (conformation), the denaturing impact that heat and pH can have on protein structure, and how these changes may affect the organism. Directionality influences structure and function of polymers, such as nucleic acids (5' and 3' ends) and proteins (amino and carboxyl ends). Carbon atoms can form diverse molecules by bonding to four other atoms (Biology, 12e: 4.2; Focus, 3e: 3.1) • The major elements of life are C, H, O, N, S, and P-sometimes recalled with an acronym that forms a person's name: P.S. COHN. I All organic compounds contain carbon, and most also contain hydrogen. I Carbon is unparalleled in its ability to form molecules that are large, complex, and diverse. Why? It has 4 valence electrons. It can form up to 4 covalent bonds. These bonds can be single, double, or triple covalent bonds. It can form large molecules. These molecules can be chains, ring-shaped, or branched. UNIT II: CHEMISTRY OF LIFE TOP FLIGHT COL Molecules with the Group and Items of Note about the Group Alcohols such as ethanol, methanol; helps dissolve molecules such as sugars Biologically Important chemical groups catonic acts such as ty adi an sugars, has acidic propertes because i tends to lonize: Carbayl, — COOH source of Hions Ketones and aldehydes such as sugars Carbaryl, >00 Amines such as amino acids; acts as a base Organic phosphates, including ATP, DNA, and phospholipids Found in the amino acid cysteine; forms disulfide bridges in proteins Suttndl. —SH Addition of a methyl group to DNA affects expression of genes 1 The chih propertis of a gun mon the various not only on tho isomers; both have the molecular formula of C,H,20%. nep dirt ki a it it at lucos and recto sone amn genient i is cabon ken bur abo on the various functional groups 1, The lintional groups arched o the sabope elion have divere proper.- attached to that skeleton. tit The behavior of organic molecules is dependent on the identity of incit 1 The tilowing are some biological important chemical groups. This chartis functional groups. for reference; you do not need to memorize these groups. Macromolecules are polymers, built from monomers (Biology, 12e: 5.1; Focus, 3e: 3.2) 1 Polymes are lone Starmis a li meado of repeating subunits called monomers. Examples: Starch is a polymer composed of glucose monomers. Proteins are polymers composed of amino acid monomers. 1 Dehydration reactions create polymers from monomers. To monomers CHo + Cen one mo elle of water. (See Figure 1.4.) Example: I Hydrolysis occurs when water is added to split large molecules. This reaction is the reverse of dehydration. (See Figure 1.4.) Dehydration eactions * Polymers • Polymers Hydrolysis, Monomers Figure 1.4 Synthesis and breakdown of polymers Carbohydrates serve as fuel and building material (Biology, 12e: 5.2; Focus, 3e: 3.3) 1 Carbohydrates include both simple sugars (glucose, fructose, galactose, etc.) and polymers such as starch and cellulose made from these and other subunits. All carbohydrates have a ratio of 1 carbon:2 hydrogen: 1 oxygen or CH,O. I Monosaccharides are the monomers of carbohydrates. Examples: glucose ous bullet point. (CH,,O.) and ribose (C,H,,Os). Notice the 1:2:1 ratio discussed in the previ- 30 PART IL: A REVIEW OF UNITS WITH SAMPLE QUESTIONS Polysaccharides are polymers of monosaccharides. Examples: starch, cellu- Both starches and cellulose are composed of glucose monomers, but the different ring forms (alpha and beta) and linkages between them result in very different functions. For example, you can digest starch, which has 1-4 alpha linkages, and not cellulose, which has 1-4 beta linkages. Keep this in mind: Change the structure, change the function! • Two functions of polysaccharides are energy storage and structural support. 1. Energy-storage polysaccharides Starch is a storage polysaccharide found in plants. Example: within Glycogen is a storage polysaccharide found in animals. Example: within vertebrate muscle and liver cells. 2. Structural support polysaccharides Cellulose is a major component of plant cell walls. Chitin is found in the exoskeleton of arthropods, such as lobsters and insects, and the cell walls of fungi. It gives cockroaches their "crunch." CONNECT WITH THE COURSE FRAMEWORK LO SYI-1-B: Describe the properties of the monomers and the types of bonds that connect the monomers in biological macromolecules. What do you need to know to master this objective? Complete the following chart as you work through the remainder of this section (part of the chart has been completed for you as an example): Macromolecule Monomers/ Component Molecules Description of the Monomers/Component Molecules How are the Monomers Linked? Carbohydrate Dehydration synthesis Protein Central carbon linked to another C, an amino group, a carboxyl group, and an R group Lipid Fatty acids Glycerol (Phosphate group) Nucleic Acid Lipids are a diverse group of hydrophobic molecules (Biology, 12e: 5.3; Focus, 3e: 3.4) Lipids are all hydrophobic. They aren't polymers because they are assembled from a variety of components. Examples: waxes, oils, fats, and steroids. Fats (also called triglycerides) are made up of a glycerol molecule and three fatty acid molecules. UNIT II: CHEMISTRY OF LIFE i had at it outin his o rail. eth. These chains ste nopolar and therefore hydrophobic. I Saturated fatty acids have no double bonds between carbons tend to pack solidly at room temperature are linked to cardiovascular disease are commonly produced by animals Examples: butter and lard I Unsaturated fatty acids have some C—C (carbon double bonds); these result in kinks tend to be liquid at room temperature are commonly produced by plants Examples: corn oil and olive oil Functions of lipids Energy storage: Fats store more than twice as many calories per gram as carbohydrates! Protection of vital organs and insulation: In humans and other mam-mals, fat is stored in adipose cells. I Phospholipids are a major component of cell membranes. They have a hydrophilic (polar) head that includes a phosphate group. They have two fatty acid tails, which are hydrophobic. They are arranged in a bilayer in forming the cell membrane, with the hydrophilic heads pointing toward the watery cytosol or extracellular environment and hydrophobic tails sandwiched in between (Figure 1.5). WATER 32 Choline Phosphate Glycerol - Hydrophilic Fatty acids Hydrophobic Space-filling model Phospholipid symbol Phospholipid bilayer Figure 1.5 The structure of a phospholipid I Steroids have a carbon skeleton of four rings that are fused together. Cholesterol is a steroid. It is a common component of animal cell membranes. Estrogen and testosterone are steroid hormones. PART II: A REVIEW OF UNITS WITH SAMPLE QUESTIONS Hydrophobic tails Hydrophilic Proteins include a diversity of structures, resulting in a wide range of functions (Biology, 12e: 5.4; Focus, 3e: 3.5) Proteins are polymers made up of amino acid monomers. Amino acids contain a central carbon bonded to a carboxyl group (COOH) at one end, an amino group (NH,) at the other end, a hydrogen atom, and an R group (variable group or side chain). (See Figure 1.6.) Peptide bonds link amino acids. They are formed by dehydration synthesis between the amino and carboxyl groups of adjacent monomers. There are four levels of protein structure (Figure 1.7): Figure 1.6 The structure of an amino acid Primary structure is the unique sequence in which amino acids are joined. Secondary structure refers to one of two three-dimensional shapes that are the result of hydrogen bonding between members of the polypeptide backbone (not the amino acid side chains). Alpha (a) helix has a coiled shape, much like a slinky. Beta (B) pleated sheet has an accordion shape. Tertiary structure has a complex globular shape resulting from interactions between the side chains (R groups), such as hydrophobic interactions, van der Waals interactions, hydrogen bonds, and disulfide These R group interactions determine the shape of globular pro-teins. Enzymes are one example of globular proteins. Quaternary structure refers to the association of two or more polypeptide chains into one large protein. Hemoglobin is a globular protein with quaternary structure because it is composed of four polypeptide chains. Protein shape is crucial to protein function. When a protein does not fold properly, its function is changed. This can be the result of a single amino acid substitution, such as in the abnormal hemoglobin typical of sickle-cell disease. A protein is denatured when it loses its shape and ability to function because of heat, a change in pH, or some other disturbance. Keep this in mind: Change the structure, change the function! Primary structure Secondary structure Tertiary structure Figure 1.7 Levels of protein structure Quaternary structure UNIT II: CHEMISTRY OF LIFE Nucleic acids store, transmit, and help express hereditary information (Biology, 12e: 5.5; Focus, 3e: 3.6) acids. Their monomers are nucleotides. DINA (deoxyribonucleic acid) and RNA (ribonuelic acid) are the two nude Nucleotides are made up of three parts (Figure 1.8): Nitrogenous base (adenine, thymine, cytosine, and guanine in DINA: adenine, uracil, cytosine, and guanine in RNA) Grout - Pentose (5-carbon) sugar (deoxyribose in DNA or ribose in RNA) sugar Nucleotide Phosphate group DNA is the molecule of heredity. Figure 1.8 The components of nucleic acids It is a double-stranded helix. Its nucleotides are adenine, thymine, cytosine, and guanine. Adenine nucleotides will hydrogen bond to thymine nucleotides; cytosine nucleotides will hydrogen bond to guanine nucleotides. RNA is single-stranded. Its nucleotides are adenine, uracil, cytosine, and gua-nine. Note that it does not have thymine. " Nucleic acids have directionality, determined by the 3' and 5' carbons of the sugar. This will determine the direction of DNA replication and transcription (5' to 3'). Which of the following statements carbon is false? Monomers/Components Examples Functions Macromolecules/Polymers Sugars, starch, glycogen, Carbohydrates Monosaccharides cellulose Energy, energy storage, structural Lipids Fatty acids and glycerol Proteins Amino acids Fats, oils Hemoglobin, enzymes Important energy source, insulation, phospholipids of plasma membrane Antibodies, movement, membrane receptors Nucleic acids Nucleotides (sugar, phosphate group, nitrogenous base) DNA, RNA Genetic information, code for amino acid sequences SUMMARY TABLE Level 1: Knowledge/Comprehension Questions The Level 1, Knowledge/Comprehension, questions review essential content knowledge but don't represent the type of question you will see on the AP Exam. The Level 2, Application/Synthesis, questions are similar to those you will see on the exam. 1. Which list of components characterizes RNA? (A) the adhesive properties of water. (A) a phosphate group, deoxyribose, and uracil (B) surface tension that is the result of the (B) a phosphate group, ribose, and uracil cohesive properties of water. (C) a phosphate group, ribose, and thymine (C) covalent bonds formed along the water's D) an amino group, deoxyribose, and uracil surface. D) cohesive bonding between the needle or 2. If you are careful, it is possible to float a pin paperclip and water. or even a paperclip on the surface of water. This can be explained by 34 PART II: A REVIEW OF UNITS WITH SAMPLE QUESTIONS American Heart iation

ChatGPT said:

Let’s cook, Hiro — this is a solid AP Bio grind plan you’ve got going here! Since you dropped all this, let’s break it down into digestible nuggets so you can master the essentials for this Chemistry of Life unit. Here’s a clean, study-friendly summary of what you need to know:

📖 AP BIO UNIT 1: Chemistry of Life — Essentials

🔬 Subatomic Particles

🧪 Types of Bonds

💧 Properties of Water (Thanks to Hydrogen Bonding)

🧫 pH Scale & Buffers

• pH scale: 0 (acidic) → 7 (neutral) → 14 (basic)

• Acid: [H⁺] > [OH⁻]

• Base: [H⁺] < [OH⁻]

• Buffer: Resists changes in pH — accepts or donates H⁺ (like carbonic acid in blood)

🌿 Carbon’s Role

• Can form 4 covalent bonds

• Creates chains, rings, branched structures

• Forms single, double, triple bonds

• Important elements: CHONPS (Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorus, Sulfur)

🥖 Macromolecules

Dehydration synthesis: Builds polymers by removing H₂O
Hydrolysis: Breaks polymers by adding H₂O

🧬 Protein Structure

1. Primary — amino acid sequence

2. Secondary — alpha helices, beta sheets (H bonds)

3. Tertiary — 3D folding (R group interactions)

4. Quaternary — multiple polypeptides joining

Denaturation: Loss of shape (and function) due to heat or pH changes