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Carbon as a Basis for Life

Chapter 4 explores the fundamental importance of carbon in all living organisms. As the backbone of vital biological molecules—including proteins, DNA, carbohydrates, and lipids—carbon enables an incredible diversity of structures and functions. The chapter covers the unique properties of organic compounds, the significance of hydrocarbons in energy production, and the concept of isomerism that affects molecular behavior. It highlights how carbon's ability to form various bonds contributes to the complexity of organic chemistry, defining the essence of life itself.

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Carbon as a Basis for Life

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  1. Carbon as a Basis for Life Chapter 4

  2. The Importance of Carbon • All living organisms based significantly on carbon • Creates a large diversity of biological molecules • Includes: proteins, DNA, carbohydrates, lipids, and others • Distinguishes living form nonliving matter • All these molecules are examples of emergent properties

  3. Defining Organic Chemistry • Organic compounds are anything containing carbon • Hydrocarbon molecules contain only hydrogen and carbon • Simple (CH4) to large and diverse (proteins) • Organic molecule variation exists both w/i individual species and b/w different species • The four main elements of living organisms are? (hint: 96% of the human body) • Valence is the number of covalent bonds an atom can make • Valence electrons are ALL electrons in outermost shell

  4. Carbon’s Ability to Bond • 6 electrons, ? in first shell and ? in outer shell • Can donate or accept electrons equally (form an ion) • Usually shares (covalent bonds) • Single, double, or triple • Makes large, complex molecules possible • Each line between 2 atoms represents 2 shared electrons

  5. Carbon Carbon Bonding • Skeletons of most organic compounds are carbon chains • Straight, branched, or ringed • Number and bond type vary • Examples of hydrocarbons

  6. Hydrocarbons • What constitutes a hydrocarbon? • Main components of fossil fuels b/c come from decomposed living organisms • Not major component of living organisms, but are regions in other molecules • Reactions cause large amounts of energy release • Fats – long, nonpolar, hydrophobic tail • Serve as stored fuel in animals • Used in gasoline

  7. Isomers • 2 molecules with the same # of the same atoms, but different structure = different properties • 3 types • Structural • Covalently bonded and arranged in different orders • Number of configurations increase with increase in number of carbons • Geometric • Covalently the same partners, but different spatial arrangement • Double bonds prohibit rotation • Enantiomer • Mirror images (R- and L-) • Usually one is inactive • Important in pharmaceuticals because both can have different effects

  8. Isomer Examples Cl Geometric Isomer Enantiomer Structural Isomer Cl Cl Cl 2C’s, 2H’s, and 2 Cl’s 1 of each 4C’s and 8H’s

  9. Biomolecular Functioning • Hydrogens can be replaced by other atom groupings • Arrangement determines properties • May participate directly in reactions or indirectly because of shape • Sex hormones as an example • Testosterone vs estradiol • Different actions • Minimal differences in structure

  10. Functional Groups

  11. Addition of water removes 1 phosphate to create ADP HOPO32- abbreviated as Pi ATP ‘stores potential to react with water’ ATP + water releases Energy for cell use Adenosine Triphosphate (ATP) Addition of water

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