click below
click below
Normal Size Small Size show me how
Chemistry 1
1 Chemistry
Organic Compounds | Any member of a large class of gaseous, liquid, or solid chemical compounds whose molecules contain carbon |
Inorganic Compounds | Are of inanimate, not biological origin, and lack carbon and hydrogen atoms |
Hydrolysis Reaction | Process in which water is used to split a substance into smaller particles |
Enzymes | Are biological molecules that catalyze (increase the rates of) chemical reactions |
Fluid Functions | 1. Help maintain body temp & cell shape 2. Facilitate the transport of nutrients, hormones, proteins, and other molecules into cells 3. Aid in the removal of cellular metabolic waste products 4. Acts as a component in body cavities/spaces |
Total Body Water | Intracellular Fluid (2/3) Interstitial Fluid (around cells) (3/4 of EFC) Intravascular Fluid (liquid portion of blood) (1/4 of EFC) Transcellular (fluid in spaces/cavities) (1/3 of EFC) |
Body Water in Ages | Premies - 80% Newborns - 70% 6 months - 60% 2 years - 59% 10-15 years - 57% Adult - 57% Senior - 45% |
Fluid Intake | Food - 1600 mL Water from food - 900 mL By-products of cellular metabolism - 200 - 300 mL |
Fluid Loss | Breathing - 500 mL Evaporation - 600 mL Urine - 1500 mL Poop - 100 - 200 mL |
TPN - IV | IV Fluid that provides nutrients - glucose, protein, electrolytes, trace elements, and lipids |
Diuresis Diaphoresis Tachypnea | Urine loss - fluid loss Sweating a lot Breathing really heavely |
Solution | Homogenous mixture of 2 or more substances (solute & solvent) |
Solvent | Medium in which the solvent dissolves in (e.g. water) |
Solute | Substance dissolved in a solvent to form a solution (e.g. kool aid powder & sugar) |
Solubility | Maximum amount of solute that will dissolve in a given amount of solvent (e.g. how much kool aid can dissolve in water). Given in g solute/100g H20 |
3 Factors of solubility | 1. Nature of the solute/solvent 2. Temperature (e.g. heating up water to put more kool aid in it) 3. Pressure (Henry's Law) |
Henry's Law - Solubility & Pressure Relationship | Solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution (e.g. pop - bottled up under pressure; when we open it the gas releases = gets flatter) |
3 types of solutions based on solubility | 1. Saturated - the perfect amount of kool aid in water (not too much, not too little) 2. Unsaturated - 1/2 the kool aid in water - could add more 3. Supersaturated - changing the solvent state to add more solute in it (e.g. heating up H2O to add more) |
Suspension | Heterogenous mixture. Large particles that float in a liquid; particles will settle when allowed to stand (e.g. sand in water) |
Colloid | Mixtures w/ large particles but small enough to remain suspended. Neither a solution or a suspension. Tend to not settle |
Isotonic | Has same solute concentration as another solution (same osmolarity). Fluid at an equal rate (e.g. 0.9% saline solution - NaCl) |
Hypotonic | Lower solute concentration than another solution (lower osmolarity). Solute concentration is greater inside the cell, free water concentration is greater outside. Free water flows into cell. |
Hypertonic | Higher solute concentration than another solution (higher osmolarity). Solute concentration is greater outside the cell, the free water concentration is greater inside. Free water flows out of cell |
Diffusion | Particles move from high concentration to low concentration (e.g. like going down the river, with the current). Simple & Facilitated |
Simple Diffusion | Cell walls composed of sheets of lipids with many minute protein pores. Substances must be small enough, lipid soluble, and have a concentration gradiant |
Facilitated Diffusion | Large lipid insoluble substances must diffuse into the cell with a carrier substance. Always require a carrier substance and a concentration gradient (e.g. glucose binds with carrier to become a lipid soluble |
5 Factors that Increase Diffusion | 1. Increased Temperature 2. Increased concentration of particle 3. Decreased size or molecular weight of the particle 4. Increased SA available 5. Decreased distance medium |
Active Transport | - Movement if substance by the use of energy (ATP), and/or a carrier molecule - Works against a concentration gradient - Low to high concentration gradient |
Sodium-Potassium Pump | - Actively transports sodium out of the cell and potassium into the cell - Uses ATP as energy to all them to go across (basically opens up a gate thingy) |
Filtration | Movement of water and solutes from high fluid hydraulic pressure to low fluid hydraulic pressure |
Hydraulic Pressure | Pressure from force of gravity acting on the fluid (hydrostatic pressure) + pressure created by the pump action of the heart |
Osmosis | Water across a semi-permeable from low to high solute concentration. Against concentration gradient |
Osmotic Pressure | Amount of hydrostatic pressure required to stop the osmotic flow of water |
Oncotic Pressure | Osmotic pressure exerted by colloids |
5 Uses for Fluid Therapy | 1. Restore fluid balances (ie. dehydrated, low blood) 2. Restore electrolytes balance (if they cannot eat) 3. Restore acid-base balance 4. Administer meds quickly (ie. heart attack/stroke) 5. Nutritional maintenance (TPN) |
5 Ways that Fluid moves | 1. Selectively Permeable 2. Diffusion 3. Active Transport 4. Filtration 5. Osmosis |
4 (first 2) Normal Conditions with Fluid Balance | 1. Fluid balances are maintained via hydrostatic and colloid oncotic pressures 2. In the arteriole, hydrostatic pressure is greater then colloid oncotic pressure resulting in a net outflow of fluid |
4 (last 2) Normal Conditions with Fluid Balance | 3. Venules = smaller hydrostatic pressure, therefore the colloid oncotic pressures draws fluid back into the venules 4. Any buildup of fluid in the interstitial space should be absorbed by the lymphatic system |
1 Abnormality with Fluid Balance | - Edema - buildup of fluid in the Interstitial Fluid (EFC) |
4 Reasons why Edema occurs | 1. Increased Hydrostatic Pressure - or heart pumping harder 2. Increased Vascular Permeability - burns, infections, more fluid leaking out 3. Decreased Oncotic Pressure - not enough colloid/fluid 4. Decreased Lymph drainage - blocked/diseased |
Crystalliods - what they are | - Treats fluid volume deficit - Electrolytes or glucose - No colloids - Small enough to cross the capillary membranes |
Colloids - what they are | - Protein - Macromolecules - then creates fluid shifts; doesn't move out - Too big to cross the capillary membrane (stays in IVF) |
Colloids - what they do | - Increase the osmotic/oncotic pressure & volume in the vascular system by drawing/attracting fluid from interstitial & intercellular spaces (good for if you need to decrease fluid in certain spaces - Edema) - Corrects hypotension - Replenishes protein |
Problems with Colloids | - Causes fluid shifts from Intracellular and Interstitial spaces into the Intravascular space and can lead to problems |
3 types of Crystaloids | 1. Isotonic - fluid has same osmolarity as plasma 2. Hypotonic - fluid has fewer solutes than plasma 3. Hypertonic - fluid has more solutes than plasma |
Isotonic - Crystalloid | - Same osmolality as body fluids - Fluids will not shift across compartments but the volume that's infused will be distributed equally to wherever it's needed |
Isotonic Dehydration - Crystalloid | - When fluids and electrolytes are lost in even amounts - No ICF fluid shifts in isotonic |
5 causes of Isotonic Dehydration | 1. Diuretic Therapy - fluid abnormalities 2. Excessive vomiting 3. Excessive urine loss 4. Hemorrhage - bleeding out & losing solutes/solvents 5. Decreased fluid intake |
Isotonic Overhydration - Crystalloid | - Excessive fluids in the EFC - EFC expands; fluids do not shift between spaces - e.g. if we give too much and the body isn't able to get rid of it fast enough |
Hypertonic - Crystalloid | - Osmolarity greater than body fluids - Cause fluid shift out of ICF and into EFC (can cause cells to dehydrate) - Lots of Solutes - attracts fluid - Good for when we need fluid; not H2O |
Hypertonic Dehydration - Crystalloid | - Water loss in EFC is greater than solute loss (too much solutes - b/c of H2O loss) |
Hypertonic Overhydration - Crystalloid | - Too much solute from excess sodium gain - Hyperosmolarity of the EFC, draws fluid from the ICF into the blood stream |
Hypotonic - Crystalloid | - Osmolarity less than body fluids - Fluids shift from EFC to ICF (can treat hypotonic dehydration) - Puts fluid into cells - can lead to swelling & rupture |
Hypotonic Dehydration - Crystalloid | - Loosing too much solute and no H2O - Fluid shifts from bloodstream into the cells = decreased vascular volume = SHOCK |
Hypotonic Overhydration - Crystalloid | - Having too much H2O and no food/electrolytes (just water diet) - Osmolarity of the ECF decreases - Fluid moves into the IFC, fluid spaces expand |
What does D5W do? | - Used to treat total body water deficits - dehydration - Expands ECF & ICF - Isotonic - Contains energy |
Compound | Pure substance that can be broken down into 1 or more simpler pure substances using chemical means |
Element | Pure substance that cannot be broken down into simpler pure substances using ordinary means |
Atom | Smallest particle of an element that can exist and still have the properties of an element |
Molecule | Group of two or more atoms that functions as a unit because the atoms are tightly bound together |
Atomic Weight | Average mass of the atoms of an element in atomic mass units |
Atomic Number | Number of protons in the nucleus of an atom of that element |
Molecular Weight | Sum of the atomic weights of all the atoms in a molecule |
Proton | A positively charged subatomic particle, found in the nucleus of an atom |
Neutron | An electrically neutral particle found in the nucleus of an atom |
Electron | A negatively charged subatomic particle found outside the atomic nucleus |
Isotope | Atoms of the same element containing different numbers of neutrons, and therefore have different masses |
Ion | An electrically charged atom or group of atoms |
Cation | (+) charged ion |
Anion | (-) charged ion |
Ionic Bonding | A bond formed on the basis of electrostatic forces that exist between oppositely charged ions |
Covalent Bonding | A bond formed between 2 or more atoms by sharing of electrons |
Valence | The capacity of an atom for entering into combination with other atoms |
Ionic Valence | Equal to the number of electrons gained or lost in forming the ionic species |
Covalence | Equal to the number of electrons from an atom that are involved in shared electron pari bonds with other atoms |
Equilibrium | Chemical equilibrium is a condition in which 2 opposing chemical reactions occur simultaneously at the same rate |
Law of Mass Action | @ a constant temp the product of the active masses on one side of a chemical equation when divided by the product of the active masses on other side of the chemical equation is a constant regardless of the amounts of each substance present at the begi |
Avogadro's Law | Equal volumes of all gases @ the same temp & pressure contain the same number of molecules. 6.02 x 10 ^23 |
pH | The pH of a solution is the (-) logarithm of the solution's molar hydronium ion concentration |
Acid | Substance that's able to donate a hydrogen ion (H+ proton) and therefore increase the concentration of H+ when it dissolves in water |
Salts | Ionic compounds that can be formed by replacing one or more of the H ions of an acid by a different (+) ion. Contains a metal ion as the (+) ion and a nonmetal ion as the (-) ion |
Base | A substance that is an H+ acceptor; produces an excess of OH- ions when it dissolves in water |
Electrolyte | A solute that produces ions in solution. An electrolyte solution conducts an electric current |
Dissociation | Ionization of electrolytes in aqueous solution to produce anions and cations |
Anabolism | The phase of metabolism in which simple substances are synthesized into the complex materials of living tissue |
Catabolism | The metabolic breakdown of complex molecules into simpler ones, often resulting in a release of energy |