1 Chemistry
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| Organic Compounds | Any member of a large class of gaseous, liquid, or solid chemical compounds whose molecules contain carbon
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| Inorganic Compounds | Are of inanimate, not biological origin, and lack carbon and hydrogen atoms
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| Hydrolysis Reaction | Process in which water is used to split a substance into smaller particles
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| Enzymes | Are biological molecules that catalyze (increase the rates of) chemical reactions
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| 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
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| 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)
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| Body Water in Ages | Premies - 80%
Newborns - 70%
6 months - 60%
2 years - 59%
10-15 years - 57%
Adult - 57%
Senior - 45%
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| Fluid Intake | Food - 1600 mL
Water from food - 900 mL
By-products of cellular metabolism - 200 - 300 mL
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| Fluid Loss | Breathing - 500 mL
Evaporation - 600 mL
Urine - 1500 mL
Poop - 100 - 200 mL
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| TPN - IV | IV Fluid that provides nutrients - glucose, protein, electrolytes, trace elements, and lipids
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| Diuresis Diaphoresis Tachypnea | Urine loss - fluid loss
Sweating a lot
Breathing really heavely
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| Solution | Homogenous mixture of 2 or more substances (solute & solvent)
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| Solvent | Medium in which the solvent dissolves in (e.g. water)
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| Solute | Substance dissolved in a solvent to form a solution (e.g. kool aid powder & sugar)
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| 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
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| 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)
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| 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)
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| 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)
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| Suspension | Heterogenous mixture. Large particles that float in a liquid; particles will settle when allowed to stand (e.g. sand in water)
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| Colloid | Mixtures w/ large particles but small enough to remain suspended. Neither a solution or a suspension. Tend to not settle
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| Isotonic | Has same solute concentration as another solution (same osmolarity). Fluid at an equal rate (e.g. 0.9% saline solution - NaCl)
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| 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.
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| 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
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| Diffusion | Particles move from high concentration to low concentration (e.g. like going down the river, with the current).
Simple & Facilitated
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| 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
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| 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
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| 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
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| 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
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| 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)
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| Filtration | Movement of water and solutes from high fluid hydraulic pressure to low fluid hydraulic pressure
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| Hydraulic Pressure | Pressure from force of gravity acting on the fluid (hydrostatic pressure) + pressure created by the pump action of the heart
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| Osmosis | Water across a semi-permeable from low to high solute concentration. Against concentration gradient
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| Osmotic Pressure | Amount of hydrostatic pressure required to stop the osmotic flow of water
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| Oncotic Pressure | Osmotic pressure exerted by colloids
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| 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)
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| 5 Ways that Fluid moves | 1. Selectively Permeable
2. Diffusion
3. Active Transport
4. Filtration
5. Osmosis
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| 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
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| 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
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| 1 Abnormality with Fluid Balance | - Edema - buildup of fluid in the Interstitial Fluid (EFC)
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| 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
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| Crystalliods - what they are | - Treats fluid volume deficit
- Electrolytes or glucose
- No colloids
- Small enough to cross the capillary membranes
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| Colloids - what they are | - Protein
- Macromolecules - then creates fluid shifts; doesn't move out
- Too big to cross the capillary membrane (stays in IVF)
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| 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
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| Problems with Colloids | - Causes fluid shifts from Intracellular and Interstitial spaces into the Intravascular space and can lead to problems
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| 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
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| 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
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| Isotonic Dehydration - Crystalloid | - When fluids and electrolytes are lost in even amounts
- No ICF fluid shifts in isotonic
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| 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
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| 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
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| 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
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| Hypertonic Dehydration - Crystalloid | - Water loss in EFC is greater than solute loss (too much solutes - b/c of H2O loss)
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| Hypertonic Overhydration - Crystalloid | - Too much solute from excess sodium gain
- Hyperosmolarity of the EFC, draws fluid from the ICF into the blood stream
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| 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
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| Hypotonic Dehydration - Crystalloid | - Loosing too much solute and no H2O
- Fluid shifts from bloodstream into the cells = decreased vascular volume = SHOCK
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| 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
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| What does D5W do? | - Used to treat total body water deficits - dehydration
- Expands ECF & ICF
- Isotonic
- Contains energy
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| Compound | Pure substance that can be broken down into 1 or more simpler pure substances using chemical means
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| Element | Pure substance that cannot be broken down into simpler pure substances using ordinary means
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| Atom | Smallest particle of an element that can exist and still have the properties of an element
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| Molecule | Group of two or more atoms that functions as a unit because the atoms are tightly bound together
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| Atomic Weight | Average mass of the atoms of an element in atomic mass units
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| Atomic Number | Number of protons in the nucleus of an atom of that element
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| Molecular Weight | Sum of the atomic weights of all the atoms in a molecule
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| Proton | A positively charged subatomic particle, found in the nucleus of an atom
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| Neutron | An electrically neutral particle found in the nucleus of an atom
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| Electron | A negatively charged subatomic particle found outside the atomic nucleus
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| Isotope | Atoms of the same element containing different numbers of neutrons, and therefore have different masses
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| Ion | An electrically charged atom or group of atoms
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| Cation | (+) charged ion
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| Anion | (-) charged ion
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| Ionic Bonding | A bond formed on the basis of electrostatic forces that exist between oppositely charged ions
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| Covalent Bonding | A bond formed between 2 or more atoms by sharing of electrons
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| Valence | The capacity of an atom for entering into combination with other atoms
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| Ionic Valence | Equal to the number of electrons gained or lost in forming the ionic species
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| Covalence | Equal to the number of electrons from an atom that are involved in shared electron pari bonds with other atoms
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| Equilibrium | Chemical equilibrium is a condition in which 2 opposing chemical reactions occur simultaneously at the same rate
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| 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
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| Avogadro's Law | Equal volumes of all gases @ the same temp & pressure contain the same number of molecules. 6.02 x 10 ^23
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| pH | The pH of a solution is the (-) logarithm of the solution's molar hydronium ion concentration
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| Acid | Substance that's able to donate a hydrogen ion (H+ proton) and therefore increase the concentration of H+ when it dissolves in water
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| 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
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| Base | A substance that is an H+ acceptor; produces an excess of OH- ions when it dissolves in water
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| Electrolyte | A solute that produces ions in solution. An electrolyte solution conducts an electric current
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| Dissociation | Ionization of electrolytes in aqueous solution to produce anions and cations
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| Anabolism | The phase of metabolism in which simple substances are synthesized into the complex materials of living tissue
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| Catabolism | The metabolic breakdown of complex molecules into simpler ones, often resulting in a release of energy
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