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Pitt NUR 0012 - Body Cavities
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NUR 0012 1st Edition Lecture 3 Outline of Last Lecture I. Negative feedback mechanismsII. Positive feedback mechanismsA. Beneficial and harmful examplesIII. Anatomical positionIV. Directional terminologyV. Anterior body regionsVI. Posterior body regionsVII. Abdomen divisionsVIII. Sectional approach to studying A and P Outline of Current LectureI. Body CavitiesA. Dorsal B. VentralC. Serous membranesII. ChemistryA. ElementsB. Protons, electrons, and neutronsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.C. Difference between a molecule and a compound and examples of eachD. ConcentrationsE. Different types of bonds and how they relate to reactivityCurrent LectureI. Body CavitiesA. Cavities within cavities maximize spaceB. Dorsal: Cranial and vertebral cavitiesC. Ventral1. Thoracic (superior mediastinum, pleural, pericardial): contains heart and lungs2. Abdominopelvic3. Serous membranes: double walled, parietal (“wall”, tougher) and visceral (layer right next to organ) layers separated by pericardial space with serous fluida. Analogy: a fist going into a balloonII. ChemistryA. Major elements1. Oxygen, carbon, hydrogena. In most organic molecules2. N, S, Fl, P, K electrolytes, etc.3. Don’t need to memorize chart just know some elements in the bodyB. Protons: positively charged in nucleusC. Neutrons: uncharged in nucleus1. Different isotopes result from change in neutron numbera. Some are radioactive: used for medical imaging, damage DNA, etc.D. Electrons: negatively charged orbit around nucleus in electron cloudE. Molecule: formed by the joining of two or more atoms by chemical bondingF. Compound: two or more different elements joined by chemical bonds1. Example: CO2 , H2O, NaCl, CaCl2, HCl, H2CO3 (carbonic acid, important buffer), H2SO4 (sulfuric acid), NaOH (sodium hydroxide), NaHCO3 (sodium bicarbonate)2. NaCl and CaCl2 are important electrolytesG. Isomer: same compound (chemical composition) but different arrangement1. Can have very different chemical properties: relates to drugs having different effects on the bodyH. Different mixtures in body1. In solution: solute dissolved in solvent2. Colloid: when solute particles slightly larger they don’t settle outa. Jello, blood plasma (mainly water with larger particles suspended in it)3. Suspension: solute particles very large settle out may scatter lighta. Blood: plasma floats I. Concentration measured in many ways1. Solvent: present in greatest amount2. Solute: present in smaller amounts, dissolved in solvent3. % solution: (g solute)/(100 mL) solvent4. Molar solution: (moles of solute)/(1L) solvent5. Milliequivalent: takes charge of electrolytes into account but very similar to molar6. Example: .9% NaCl = 290mosm NaCl = isotonic saline (normal)J. Ionic bonds: electrons transferred between atoms1. Cations: positively charged ions2. Anions: negatively charged ions3. Loss of electrons: oxidation4. Gain of electrons: reduction5. Ionic compounds dissociate into their ions in polar solvents (water for example)6. Electrolytes: salts that dissociate into their ions in water7. Water is polar because it has positive and negative parts: keeping dissociated ions separateK. Nonpolar covalent bonds: electrons shared equally, no difference in charge (no net dipole moment)1. Normally only dissolve in nonpolar solvents: like dissolves like2. Single covalent bond: methane CH43. Diatomic molecules (double covalent bond): O2 etc.L. Polar covalent bonds: electrons not shared equally, have a dipole moment1. Usually dissolve in polar solvents2. Example: water, more negative O and more positive H3. Has to do with electronegativity: example, O more electronegative than H so attracts electrons more easily (higher affinity for electrons)4. Hydrogen bonds: very weak, occur between adjacent water moleculesa. Create surface tensionb. Intramolecular bonds in complex molecules in our body: proteins for example1) Hydrogen bonding can determine shape, how receptors work etc. M. Reactivity and bonding1. Ionic bonds most reactive2. Polar covalent bonds3. Nonpolar covalent bonds least reactive N. Water is the universal solvent: key for most life processes1. Polar: anything that dissolves in water2. Nonpolar: don’t dissolve in watera.


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