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34 Cards in this Set
- Front
- Back
Solid
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has definite shape and volume
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Liquid
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Has a definite volume but takes the shape of its container.
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Gas Pressure
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Force created when particles hit container walls.
1.measure of: 1 atm=29.9 inches of Hg=760mmHg. 2.More molecules in container at same temperature increases pressure. 3.P=force/Area |
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Gas Volume
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Equal to the volume of container.
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Partial Pressure (Pp)
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Amount of a gas mixture id the sum of the partial pressures of the gases in the mixture
OR The total pressure of a mixture multiplied by the % of gas in the mixture is the partial pressure of that gas in the mixture. |
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Solution
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Mixture of one substance dispersed uniformly in another substance.
A. Solute - substance to be dispersed. B. Solvent - substance that contains the solute; ususally present in a greater amount than solute. C. Solute and Solvent do NOT react with each other so they can be mixed in various proportions. D. May be gases, liquids or solids;solution has same state as solute E. Characterstics 1.Small single particles that go through a filter and semipermeable membrane. 2.Uniformly Dispersed to give homogeneous solution that is transparent. 3. Particles do not settle out of solution. |
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Ionic Solution
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A. To form liquid or solid solutions, there must be an attraction between the solute and the solvent so that both will seperate into individual ions or molecules.
B. Polar H of water attracts the Cl of ionic NaCl; polar O attracts the NA-; thus NaCl dissolves in water forming an ionic solution. |
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Solubility
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The amount of solute that can dissolve in a solvent.
A. Like dissolves Like 1. Polar solvents attract polar solutes to form ionic solutions 2. Polar solvents(water) do not attract nonpolar solutes(iodine) |
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Unsaturated Solution
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has less than the maximum amount of solute.
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Saturated Solution
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contains the maximum amount of solute.
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Colloid
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Particles are larger molecules or groups of molecules or ions.
1. Homogeneous mixture inwhich particles do NOT seperate out. 2. Particles pass through some filters but not semipermeable membranes. 3. Light into a colloid produces a Tyndall effect (like headlight into a fog) types: Aerosols, Foams, Emulsions, Sols (blood plasma, paint, cement, pearls). |
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Suspension
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heterogeneous, nonuniform, opaque mixture.
Particles are often visible. Muddy water, pennicilin. |
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Diffusion
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particles spreading out following a concentration gradient until all particles are equally distributed.
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Osmosis
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solvent water moves through a semipermeable membrane from a dilute solution(more water molecules) to a concentrated solution(less water molecules)
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Dialysis
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small particles and water through a semipermeable membrane.
A. Seperates solutions from colloids B. Used to remove urea and other wastes from blood when kidneys fail. |
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Isotonic
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equal in osmotic pressure to the osmotic pressure within the cell.
No change in cell. |
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Hypotonic
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less solutes and more water in the solution outside the cell.
Water moves into the more concentrated solution inside the cell Causes cell to swell and possibly burst. Hemolysis - causes red blood cells to rupture. |
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Hypertonic
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more solutes and less water in the solution outside the cell.
Water moves out of the cell to the more concentrated solution causes cells to shrivel up |
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Crenation
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- causes red blood cells to shrivel.
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Acid
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Substances that produce H+ when dissolved in water.
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Ionic bond
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USUALLY metal and a non-metal
metal donates one or more electrons (cation) to a non-metal (anion) which takes it. Ionic substances in solution conduct electricity because the ions are free to move and carry the electrical charge from the anode to the cathode. |
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Covalent Bond
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sharing electrons
Occurs between 2 nonmetals usually Identical nonmetals equal sharing - nonpolar covalent bond |
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Polar Covalent Bond
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Nonidentical Nonmetals
shared unequally i.e. H2O O is a big electron compared to H |
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Polyatomic Molecule
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Polyatomic ion – charged particle composed of 2 or more atoms covalently bonded together
Nonmetal P, S, C, & N will covalently bond to O to form a polyatomic ion Have negative charge of -1, -2, or -3 SO4–2, NO3–1, PO4–3, HPO4–2, H2PO4– Exceptions: OH–, CN–, NH+ |
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Molar Mass
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Total AMU of all atoms.
expressed as Grams |
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Exothermic reaction
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reactions release heat
reactant + reactant ->product + kalories when energy of PRODUCTS is LOWER than the energy of the REACTANTS, heat is released. |
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Endothermic reaction
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reactions absorb heat
kalories +reactant ->product when the energy of the REACTANTS is lower than the energy of the PRODUCTS, heat is absorbed. |
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Base
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substance that produces OH when disolved in water.
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pH Scale
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convenient way to describe the acidity of a solution.
pH scale 1 - 14 pH1 being most acidic pH14 being most basic pH7 being nuetral |
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neutralization
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any acid + any base forms salt+water
complete nuetralization when the molarity of the acid present equals molarity of the base present; the pH is 7 |
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buffer
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a solution that resists a change in pH.
buffers contain a weak acid and a salt of that acid or a weak base and a salt of that base; strong acids and bases cannot make buffer solutions. |
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Naming
Covalent and Ionic Bonds |
end with -ide
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Naming
polyatomic ions |
end with -ite or -ate
1less O is -ite 1more O is -ate |
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prefixes
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1 mono
2 di 3 tri 4 tetra 5 penta 6 hexa 6 hepta 8 octa 9 nona 10 deca |