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Chemistry: Atoms, Bonds, and Compounds in Life

Dive into the world of chemistry with a focus on atoms, covalent and ionic bonds, water properties, hydrogen bonding, mixtures, solutions, acids, bases, pH scale, organic compounds, carbohydrates, lipids, proteins, and nucleic acids. Explore the fundamental building blocks of life!

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Chemistry: Atoms, Bonds, and Compounds in Life

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  1. Do Now • Draw an atom of oxygen • Draw two atoms of hydrogen bonded to one atom of oxygen • What type of bond do O and H form? • What is a covalent bond? • What is an ionic bond? • What is an isotope?

  2. Chapter 4 Organic Chemistry

  3. 4-1 Water • 75% of earth’s surface • Most abundant compound in living things • Liquid at room temperature • Expands when freezes • Necessary for life

  4. Charged molecule – polar • E- unevenly distributed • “little magnet” • Polarity allows water to stick to others and go in between other molecules

  5. Water Molecule

  6. Cohension – water sticking to water • Adhesion – water sticking to other things

  7. Hydrogen Bonding

  8. Mixtures • Substances are physically mixed but have not formed new chemical bonds • Different substances in a mixture retain their usual properties

  9. Ex. Table salt and iron filings, sugar and sand • Homogeneous – spread evenly throughout

  10. Solutions • Solutions - Mixtures that are liquid • Solvent - the liquid substance that makes up the bulk of the solution • Water is the universal solvent. • Solute – other substances that are dissolved in the solvent

  11. Concentration – the measurement of the amount of solute dissolved in a fixed amount of solution • Aqueous solutions – solutions in which water is the solvent

  12. Solutions • When ionically bonded compounds dissolved in water they dissociate or break apart into individual ions • NaCl  Na+ + Cl- • HCl  H+ + Cl-

  13. H+ • Most chemically reactive ion • Single proton – no e- • Attacks chemical bonds • Acids release H+

  14. Bases • NaOH  Na+ + OH- • Bases release OH-

  15. Strong acids and bases are highly reactive – attack and break chemical bonds – dangerous to living tissues

  16. Neutralization Reaction • Mixing an acid and a base OH- cancels H+ • H+ + OH-  H2O

  17. Acids and Bases

  18. pH – a measure of the relative amounts of hydronium (H3O or H+) and hydroxide ions (OH-) • pH = power of hydrogen • In water these ions form naturally • Pure water contains equal numbers of H+ and OH- ions • Neutral – OH- = H+

  19. pH Scale • Ranges from 0 to 14 • 0 is very acidic – H+ • 7 is neutral OH- = H+ • 14 is very basic (alkaline) OH-

  20. A difference of 1 on the pH scale is actually a difference of 10 times the strength of acids or bases

  21. Acids • Acid solution – contains many more H+ ions that OH- ions • Ex. HCl (hydrochloric acid) or H2SO4 (sulfuric acid) • Have a sour taste, produce a tingling or burning sensation if they come in contact with skin, highly corrosive when concentrated • Ex. Citric acid – oranges, lemons and grapefruits

  22. Bases • Base solution – a solution that contains many more hydroxide ions (OH-) than hydronium ions (H3O+) • Ex. NaOH • Alkaline refers to bases • Have a bitter taste, feel slippery

  23. Importance of pH • certain pH’s are needed for different reactions in the body • Certain organisms need a certain pH to live • Ex. Fish

  24. Suspensions • A mixture in which particles spread through a liquid or gas but settle overtime

  25. 4-2 Chemical Compounds in Living Things • Elements • 90 naturally occurring • 11 common in organisms • 20 trace • 96.3% of the body – C, N, O, H

  26. In varying combinations the elements C, H, N, O make up practically all the chemical compounds in living things

  27. Inorganic Compounds • No C • Exception – CO2 • Ex. Water, minerals, salts

  28. Organic Compounds • Have C • “organic chemistry” • C makes about 2 million compounds

  29. Carbon is unique – remarkable ability to form stable and strong covalent bonds • Carbon can form 4 single covalent bonds • Methane – CH4 – chemical formula • Structural Formula

  30. Carbon can bond with O, N, P, S • Carbon can form chains of C atoms – unlimited length • C atoms can bond either single, double or triple • Carbon needs 4 bonds to be “happy”

  31. Carbon Atoms FormCovalent Bonds

  32. Carbon Formations • Chains • Rings • Mixes of single, double, triple bonds

  33. Polymerization • Taking smaller C compounds and joining them to form larger compounds

  34. Monomers • Small compounds • Ex. sugar

  35. Polymers • Many monomers joined together

  36. Macromolecule • A large polymer • Macro = giant • Polymerization allows us to join monomers together to get complex molecules • Ex. Alphabet – 26 letters – many combinations make many words

  37. 4.3 Compounds of Life • 4 groups of organic compounds • Carbohydrates – pasta, bread • Lipids – fats, oils, waxes • Proteins – meat • Nucleic acids – DNA and RNA

  38. Carbohydrates • Ex. Sugars and starches made of C, H, O • O to H ratio 1:2 like water, C varies • 1C:2H:1O

  39. Monosaccharides • Simplest carbohydrate • One sugar • Ex. Glucose – sugar – green plants make Fructose – in fruits Galactose – in milk

  40. All three – C6H12O6 • The 3 differ on how the atoms are arranged • Isomer - have the same number of atoms but they are arranged differently

  41. Importance of Sugars • Contain a lot of energy • Energy stored in the bonds • Break bonds  release energy

  42. Dehydration Synthesis • Complex carbohydrates made by the process of polymerization • Chemical bonds linked • Bond formed between OH-’s • Dehydration synthesis – removes a water, two monomers join • Fig. 4-12

  43. Dissacharide • Made of 2 monomers • Ex. Sucrose – table sugar • Maltose – malt sugar • Lactose – milk sugar

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