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Inorganic Compounds

Inorganic Compounds. Matter and Energy. Matter—anything that occupies space and has mass (weight). The “stuff” of the universe. Matter and Energy. Energy—the ability to do work. Energy is massless and takes up no space. Energy can be measured only by its effects upon matter.

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Inorganic Compounds

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  1. Inorganic Compounds

  2. Matter and Energy Matter—anything that occupies space and has mass (weight). The “stuff” of the universe.

  3. Matter and Energy • Energy—the ability to do work. Energy is massless and takes up no space. Energy can be measured only by its effects upon matter. HuMo is a device that equips your clothing with kinetic energy harvesting capabilities. In this way it enables you to use the physical capability of your body to power devices we rely on in modern life. This version embeds the system in a jacket where the energy is harvested from the normal arm swing of the wearer as they walk. The power in this jacket is applied directly to lighting, keeping the wearer safe while running or walking the streets in the morning or evening A normal walking arm swing produces approximately ½ watt of energy.

  4. Matter and Energy

  5. Types of Energy Chemical Energy is stored in the bonds of chemical substances. When bonds are broken potential (stored) energy is unleashed and becomes kinetic energy (energy in action). catabolism destructive metabolism vs. anabolism constructive metabolism

  6. Types of Energy Electrical Energy results from the movement of charged particles (ions). In your body an electrical current is produced when ions move across cell membranes. Think about nerve impulses. http://highered.mcgraw-hill.com/sites/0072495855/student_view0/chapter2/animation__how_the_sodium_potassium_pump_works.html

  7. Types of Energy Mechanical Energy is energy directly involved in moving matter. When you ride a bike your legs provide the mechanical energy that moves the pedals.

  8. Types of Energy Radiant Energy travels in waves. It is the energy of the electromagnetic spectrum. Think X-Rays, infrared radiation, visible light, radio, and UV. Ultraviolet (UV) photons harm the DNA molecules of living organisms in different ways. In one common damage event, adjacent bases bond with each other, instead of across the “ladder.” This makes a bulge, and the distorted DNA molecule does not function properly . Special repair enzymes usually fix this damage, but not always.

  9. Composition of Matter Elements—fundamental units of matter. Elements are unique substances that cannot be broken down into simpler substances by ordinary chemical methods.

  10. Composition of Matter 96% of the body is made from four elements • Carbon (C) • Oxygen (O) • Hydrogen (H) • Nitrogen (N)

  11. Composition of Matter Atoms—building blocks of elements

  12. Molecules and Compounds Molecule—two or more like atoms combined chemically Figure 2.4 Two hydrogen atoms combine to form a molecule of hydrogen gas. This is an example of a covalent bond.

  13. Molecules and Compounds Compound—two or more different atoms combined chemically Figure 2.4

  14. Chemical Reactions Chemical Reactions occur whenever atoms combine with or dissociate from other atoms. When atoms unite chemically, chemical bonds are formed. Atoms dissociate from other atoms when chemical bonds are broken. Your metabolism is the sum total of all of the chemical reactions in your body.

  15. Patterns of Chemical Reactions • Synthesis reaction (A + BAB) • Atoms or molecules combine to form a larger, more complex molecule • Energy is absorbed for bond formation • Synthesis reactions underlie all anabolic (constructive) activities that occur in body cells.

  16. Synthesis Reaction Figure 2.10a

  17. Patterns of Chemical Reactions • Decomposition reaction (ABA + B) • Molecule is broken down into smaller molecules, atoms, or ions. • Synthesis reactions in reverse • Chemical energy is released when bonds are broken • Underlie all catabolic (destructive) processes that occur in body cells.

  18. Decomposition Reactions Figure 2.10b

  19. Patterns of Chemical Reactions • Exchange Reactions • (AB + CAC + B) • (AB + CD AD + CB) • Involve both synthesis and decomposition reactions. • Bonds are both made and broken.

  20. Patterns of Chemical Reactions Figure 2.10c

  21. Biochemistry: Essentials for Life • Organic compounds • Contain carbon • Most are covalently bonded • Example: C6H12O6 (glucose) • Inorganic compounds • Lack carbon • Tend to be simpler compounds • Example: H2O (water)

  22. Water High heat capacity-water absorbs and releases large amounts of heat before its temperature changes appreciably. Thus preventing sudden changes in body temperature due to environmental conditions and physical activity/inactivity.

  23. Water Polarity/solvent properties-water is an excellent solvent due to its polarity.

  24. Water Chemical Reactivity-water is an important reactant in chemical reactions like the digestion of food. These are called hydrolysis reactions. Here sucrose hydrolysis breaks a sucrose molecule down into glucose and fructose.

  25. Water Cushioning-water serves a protective function in the human body. Water (in the form of cerebrospinal fluid) provides cushioning to the brain protecting it from physical trauma.

  26. Important Inorganic Compounds • Salts are inorganic compounds containing cations other than H+ and anions other than the hydroxyl ion (OH-) • Easily dissociate into ions in the presence of water • Vital to many body functions-found primarily in teeth and bones (calcium and phosphorous-based) • Include electrolytes which conduct electrical currents

  27. Important Inorganic Compounds • Acids • Release hydrogen ions (H+) • Are proton donors • Bases • Release hydroxyl ions (OH–) • Are proton acceptors Acids and bases can conduct an electrical current • Neutralization reaction • Acids and bases react to form water and a salt

  28. pH • Measures relative concentration of hydrogen ions • pH 7 = neutral • pH below 7 = acidic • pH above 7 = basic • Buffers—chemicals that can regulate pH change Figure 2.12

  29. Table 2.4 pH Values of Selected Substances (pg 41)

  30. Buffers • Resist changes in pH • convert strong acids or bases to weak ones • Physiological buffer • system that controls output of acids, bases or CO2 • urinary system buffers greatest quantity, takes several hours • respiratory system buffers within minutes • Chemical buffer systems • restore normal pH in fractions of a second • bicarbonate, phosphate and protein systems

  31. Bicarbonate Buffer System • Solution of carbonic acid and bicarbonate ions • CO2 + H2O  H2CO3 HCO3- + H+ • Reversible reaction important in ECF • CO2 + H2O  H2CO3 HCO3- + H+ • lowers pH by releasing H+ • CO2 + H2O  H2CO3 HCO3- + H+ • raises pH by binding H+ • Functions with respiratory and urinary systems • to lower pH, kidneys excrete HCO3- • to raise pH, kidneys and lungs excrete CO2

  32. Phosphate Buffer System • H2PO4-  HPO42- + H+ • as in the bicarbonate system, reactions that proceed to the right release H+ and  pH, and those to the left pH • Important in the ICF and renal tubules • where phosphates are more concentrated and function closer to their optimum pH of 6.8 • constant production of metabolic acids creates pH values from 4.5 to 7.4 in the ICF, avg.. 7.0

  33. Protein Buffer System • More concentrated than bicarbonate or phosphate systems especially in the ICF • Acidic side groups can release H+ • Amino side groups can bind H+

  34. Respiratory Control of pH • Neutralizes 2 to 3 times as much acid as chemical buffers can • Collaborates with bicarbonate system • CO2 + H2O  H2CO3 HCO3- + H+ • lowers pH by releasing H+ • CO2(expired) + H2O  H2CO3 HCO3- + H+ • raises pH by binding H+ •  CO2 and  pH stimulate pulmonary ventilation, while an  pH inhibits pulmonary ventilation

  35. Renal Control of pH • Most powerful buffer system (but slow response) • Renal tubules secrete H+ into tubular fluid, then excreted in urine

  36. H+ Secretion and Excretion in Kidney (carbonic anhydrase)

  37. Limiting pH • Tubular secretion of H+ (step 7) • continues only with a concentration gradient of H+ between tubule cells and tubular fluid • if H+ concentration  in tubular fluid, lowering pH to 4.5, secretion of H+ stops • This is prevented by buffers in tubular fluid • bicarbonate system • Na2HPO4(dibasic sodium phosphate) + H+  NaH2PO4 (monobasic sodium phosphate) + Na+ • ammonia (NH3),from amino acid catabolism, reacts with H+ and Cl-  NH4Cl (ammonium chloride)

  38. Buffering Mechanisms in Urine

  39. Acid-Base Balance

  40. Acid-Base & Potassium Imbalances • Acidosis • H+ diffuses into cells and drives out K+, elevating K+ concentration in ECF • H+ buffered by protein in ICF, causing membrane hyperpolarization, nerve and muscle cells are harder to stimulate, CNS depression from confusion to death

  41. Acid-Base & Potassium Imbalances • Alkalosis • H+ diffuses out of cells and K+ diffuses in, membranes depolarized, nerves overstimulate muscles causing spasms, tetany, convulsions, respiratory paralysis

  42. Disorders of Acid-Base Balances • Respiratory acidosis • rate of alveolar ventilation falls behind CO2 production • Respiratory alkalosis (hyperventilation) • CO2 eliminated faster than it is produced • Metabolic acidosis •  production of organic acids (lactic acid, ketones), alcoholism, diabetes, acidic drugs (aspirin), loss of base (chronic diarrhea, laxative overuse) • Metabolic alkalosis (rare) • overuse of bicarbonates (antacids), loss of acid (chronic vomiting)

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