new material for final exam Flashcards
Lower solute concentration than normal, water flows into cell, swells and may burst (hemolysis)
Hypotonic
- Don’t donate protons (H+) very readily, only some of the molecules ionize
- Many molecules remain, only a few ions are formed
- Weak electrolytes
Weak Acids
Gain of electrons
Reduction
What uses redox reactions as a power source?
Batteries
Destruction of metals by oxidation reactions
Corrosion
Causes oxidation
Oxidizing Agents
Causes reduction
Reducing agents
The ability of a liquid to form a membrane-like surface and resist spread
Surface Tension
Used to determine concentrations of solutions
Titration
When the number of equivalents of acids and base are equal
Equivalence point
The study of reaction rates
Kinetics
Liquid to gas
Vaporizing/boiling
Reactants hurtling through space and smashing into each other
Collision Theory
A reaction system in which opposing microscopic processes are in balance
Equilibrium
Loss of electrons
Oxidation
Stress an equilibrium system and it will shift to re-establish an equilibrium system
LeChatelier’s Principle
Prevents contact with oxidizing agents as long as the layer is 100% intact
Painting
The pressure of a gas in equilibrium with its liquid
Vapor Pressure
Holding more dissolved solute with solution than should be possible, “overfull” at this temperature, very unusual
Supersaturated
M, moles solute per 1 liter total solution
Molarity
Some properties of solutions are influenced by the total number of particles of solute dissolved
Colligative Properties
Movement of water across a semi-permeable membrane from high to low concentration
Osmosis
IMFs looser, warmer temperature, flowing, some motion
Liquids
All matter meets the requirements
London Forces
Can act as either an acid or base depending on what interacts with them
Amphoteric
- Donate protons (H+) readily, ionizes nearly 100%
- Essentially no molecules remain in solution (no ions)
- Strong electrolytes
Strong Acids
IMFs tight, cooler temperature, little or no motion
Solids
Have a great attraction for (acceptance of) protons (H+)
- Essentially 100% OH- ions formed and accept H+
- Strong electrolytes
Strong Bases
No IMFs, hotter temperature, lots of independent motion
Gases
The resistance of a liquid to flow
Viscosity
Gas to liquid
Condensing
Do not attract (accept) protons (H+) as well, only a few OH- ions formed, weak electrolytes
Weak Bases
Solid to liquid
Melting
Substances which resist change in pH
Buffers
Blood pH falls below 7.3, expel carbon dioxide through increased breathing rate
Acidosis
The pressure (force) necessary to prevent the flow a water across a concentration gradient
Osmotic Pressure
Liquid to solid
Freezing
Blood pH rises above 7.5, retain carbon dioxide through decreased breathing rate
Alkalosis
May still dissolve more solute, not “full” at this temperature yet
Unsaturated
Coats metal with a more easily oxidized metal that will form a protective layer even after oxidation
Galvanizing
Equal tonicity
Isotonic
Litmus? red to blue Taste? bitter Feel? slippery Reactions with carbonates? none Reaction with active metals? none pH range? 8-14
Bases
Higher solute concentration than normal, water flows out of the cell, shrinks and shrivels (crenation)
Hypertonic
Using the beautiful and difficult to oxidize metals chromium, gold, or platinum to coat more easily oxidized metals
Electroplating
Using a sacrificial chunk of easily oxidized metal attached to the main metal
Cathodic Protection
Requires a grouping within the molecule of O-H, N-H, or F-H and available nonbonding electrons on the other molecule
Hydrogen Bonding
Will dissolve no more solute, “full” at this temperature
Saturated
Requires polar molecules with permanent dipoles
Dipole-Dipole Bonding
Solid directly to gas
Sublimation
Litmus? blue to red Taste? sour Feel? sticky Reaction with carbonates? yes Reaction with active metals? yes pH range? less than 7
Acids
