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Understanding the Chemistry of Life: From Atoms to Compounds

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julio
21 diapositives · 427 Views · Sep 20, 2014

Chapter 6 delves into the fundamental building blocks of matter—atoms and elements—and their crucial roles in life. It outlines the major and trace elements in the human body, detailing how atoms combine to form compounds through covalent and ionic bonds. The text explains the structure of atoms, the significance of isotopes, and the nature of chemical reactions, including metabolism and pH balance. By exploring these concepts, we gain insights into the composition and interaction of substances that sustain living organisms.

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  1. The Chemistry of Life Chapter 6

  2. Atoms and their interactions • Elements – are substances that can’t be broken down into simpler substances

  3. Natural Elements in living things • Major elements in the human body: C, H, O, N • Make up more than 96% of the mass of the human body

  4. Trace Elements • Trace: Ca, P, K, S, Na, Cl, Mg, Fe, Zn, Cu, I, Mn, B, Cr, Mo, Co, Se, F • Vital role in maintaining healthy cells

  5. Atoms: the building blocks of elements • Atom – smallest particle of an element that has the characteristics of that element • Structure effects their properties and chemical behavior

  6. The structure of an atom

  7. Nucleus – center of the atom • Protons – positive charge • Neutrons – neutral charge • Electrons – around nucleus w/ negative charge

  8. Electron Energy Levels • 1st – can hold 2 electrons • 2nd – can hold 8 electrons • 3rd – can hold 8 electrons • Are there other energy levels?

  9. Isotopes • Atoms that have the same # of protons, but a different # of neutrons • Named by # protons & neutrons (combined total) • EX: carbon-12 vs. carbon-14

  10. WHY Isotopes are useful to scientists • Some nuclei of isotopes are unstable and break apart. • Give off radiation. • Can be used in medicine to diagnose or treat some diseases.

  11. Compounds • Bonding – determined by valence electrons. • 2 or more different atoms chemically combined in a specific ratio.

  12. Covalent Bonds • Electrons are shared & creates a molecule

  13. Molecules • A group of atoms held together by covalent bonds • Ex: Water (H2O)

  14. Ionic Bonds • Ionic bonds – electrons are gained or lost by individual atoms. • Ions are formed. • Ex: Salt: • Ionic Bond b/t Na+ & Cl-

  15. Ions • An ion is a charged particle made of atoms • Atoms that gain or lose electrons have an electrical charge.

  16. Chemical Reactions • Mixture – a combination of substances in which chemicals retain their original properties.

  17. Chemical Reactions • Metabolism – all chemical reactions that occur within an organism

  18. Chemical Reactions • Solution – mixture in which substances are evenly distributed in another substance • Solutes – the substances that are dissolved • Solvent – the substance that things are dissolved in

  19. Chemical equations Ex: 2H2 + O2 2H2O • Large numbers mean how many atoms / molecules of a compound you have • Small numbers indicate how many of that type of atom you have • Symbols are chemical symbols from the periodic table

  20. pH • pH – the measure of how acidic or basic a solution is.

  21. pH • Acid – any substance that forms hydrogen ions in water (H+); pH of below 7 • Base – any substance that forms hydroxide ions in water (OH-); pH above 7