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Chemistry and Biochemistry

Chemistry and Biochemistry. For Advanced Diploma students of the WEA Hunter Academy of Complementary Health. An Introduction. John Radvan BSc (Molecular Biology) Keen interest in Complementary Health E-Learning advocate Crazy geek Chronic watcher of the ‘Big Bang Theory’

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Chemistry and Biochemistry

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  1. Chemistry and Biochemistry For Advanced Diploma students of the WEA Hunter Academy of Complementary Health (c) WEA Hunter Academy of Complementary Health. Created by John Radvan. Reproduction or transmission without the express permission of the author is prohibited.

  2. An Introduction • John Radvan • BSc (Molecular Biology) • Keen interest in Complementary Health • E-Learning advocate • Crazy geek • Chronic watcher of the ‘Big Bang Theory’ • @jradsy on Twitter

  3. Housekeeping • OHS Discussion • Introductions • Form signing • Subject Outline • Questions?

  4. Class Format • Believer in ‘casual’ learning – but that doesn’t mean you can slack off! • Lots of information, but lots of interaction • Chalk and talk • Discussions • Group Activities • Study and Research • Flexible students stay in touch!

  5. Chapter One ELEMENTS, COMPOUNDS, CHEMISTRY, LIFE

  6. What is life really made of? Click the link and watch life unfold. Best played to ‘What a Wonderful World’ http://bit.ly/9PnNEj

  7. Elements • Definition of matter – ‘stuff’ • Matter – has mass, volume and occupies space • Matter is made from atoms • Atoms that are of the same type are called ‘elements’

  8. Elements • 4 major ‘life elements’ – Carbon, Oxygen, Hydrogen and Nitrogen (96% of body) • Other elements are ‘trace elements’ as they are needed in small amounts

  9. Atoms • On page 4, read ‘why are elements the way they are?’ • Draw a picture in your notes highlighting where the Protons, Neutrons and Electrons are. • These are ‘subatomic particles’, each particle has a ‘charge’. Protons (+), Neutrons (0) and Electrons (-)

  10. Elements of Life • Look at Table 1.1 on page 5. Work alone or together to list all the things you think could go wrong if the body were to lack each element. Write these down. • Are there any terms on this page you have never heard? If so, check the glossary!

  11. States of Matter

  12. Compounds • Pure substance made up of two or more elements • Eg – Water is made up of H and O • The important point to remember is that compounds are made up of atoms that are bonded together • 20 million known compounds are out there! • Compounds are displayed by different formulas (eg – H2O = 2 x H and 1 x O)

  13. Covalent Bonds • Covalent bonds – this is a ‘sharing’ of electrons in order to fill valence shells. Forms a ‘figure 8’ of sorts. These are usually found between nonmetals, or between a nonmetal and a metalloid. • Look at Table 1.2 on page 9

  14. Ionic Bonds • Protons (+) and electrons (-) are in equal numbers in an atom • If an electron is REMOVED it is now a positively charged ion (cation) • If an electron is ADDED it is now a negatively charged ion (anion) • Ionic bonds – this is simple positive-negative attraction. An anion attracts a cation. Thus a bond is formed. These are usually found between a metal and a nonmetal.

  15. Hydrogen Bonds • H atom bonded to N or O • Water is good example • VERY important in organic chemistry • Strong bond, requires high temperature to break

  16. Chapter Two WATER: THE SOLVENT OF LIFE

  17. Why is water special? • Read the first paragraph under this section on Page 15 • The polarity of water is the reason that water stays in a glass and doesn’t fly out into the atmosphere • If we want to separate water from itself, we add heat, which creates steam!

  18. Solutions • Mixtures are classified homogeneous or heterogeneous on the macroscopiclevel – define these terms! • Solutions are something IN something, (solute in solvent)

  19. Saltwater • NaCl is common table salt • When salt is exposed to water, the slightly positive Na is attracted to the slightly negative O on the water (and the negative Cl is attracted to the H) • This causes water to ‘surround’ the NaCl forming a hydration cell, which puts itself between all the little NaCl molecules

  20. Solubility • Define these terms: • Hydrophobic • Hydrophilic • Colloid • Polar molecules dissolve in polar solvents • Nonpolar molecules dissolve in nonpolar solvents • Polar and nonpolar generally do not dissolve– just like oil and water

  21. Water Ionisation • Work together or alone to draw a diagram that explains how water ionises. Use page 17 to help you. • The goal is to explain graphically how OH- and H3O+ is created.

  22. Acids and Bases • Liquid water has a tendency to ionise, but the rate of ionisation and the reverse reaction is equal – this is ‘equilibrium’ • When an acidic or basic solution enters the water they disturb the balance. • Acids increase the amount of H+ in the water • Bases increase the amount of OH- in the water

  23. Acid example • HCl on its own is a poisonous gas • In water, the H bonds with H2O to yield H3O+ • This leaves Cl- behind • Thus: HCl + H2O  H3O+ + Cl-

  24. pH and pOH • The pH scale exists between 0-14 • If pH< 7 = acid • pH > 7 = base • pH = 7, neutral (water) • pOH is concentration of [OH-] • pH + pOH = 14

  25. Strength • Acids and Bases are not equally strong • A strong acid/base ionizes (splits) completely • A weak acid/base partially ionizes • Look at Figure 2.5 on page 18

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