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Chemistry Review-1.1
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| Question | Answer |
|---|---|
| What is an acid? | Tastes sour, reacts with metals and carbonates, turns blue litmus paper red, <7 on pH scale |
| What is a base? | Tastes bitter, feels slippery, turns red litmus paper blue, >7 on pH scale |
| What is a Hydrogen ion (H+)? | An atom of hydrogen that has lost its electron. |
| What is a Hydroxide iron (OH-)? | A negatively charged ion.....Gained an electron |
| Element: | Simplest pure substance. Can't be broken into other substances |
| Matter: | Anything that has mass and volume |
| What is all matter composed of? | 1 element or a combination of 2 or more elements |
| Compound | Substance made of 2 or more elements chemically combined |
| Mixture | 2 or more elements in the same place, but NOT chemically combined |
| Democritus | Named the atom |
| Protons | positively charged particles, located in the nucleus |
| Neutrons | no electric charge, located in the nucleus |
| Electrons | negatively charged particles, located in the electron cloud |
| Solid | Definite volume and shape, particles close together |
| Liquid | Definite volume, particles vibrate |
| Gas | No definite volume or shape, particles move past each other easily |
| Density | Mass Volume |
| Melting | Solid-Liquid |
| Freezing | Liquid-Solid |
| Condensation | Gas-Liquid |
| Evaporation | Liquid-Gas |
| Sublimation | Solid-Gas |
| Synthesis | A+B yields AB |
| Decomposition | AB yields A+B |
| Single Replacement | AB+C yields AC+B |
| Double Replacement | AB+CD yields AC+BD |
| Homogeneous Solution | Particles hard to tell apart |
| Heterogeneous Solution | Particles easy to tell apart |
| Atom: | Smallest particle of an element |
| Nucleus: | Center of atom, where the mass is, protons and neutrons |
| Energy Level | A region around the nucleus in which electrons of the same energy are likely to be found |
| Atomic # | order of periodic table, amount of protons |
| Atomic Mass | # of protons + # of neutrons |
| Valence Electrons | electrons in the outermost energy level |
| Ion | atom group of atoms that has an electric charge |
| Ionic Bond | attraction between 2 oppositely charged ions....they form as a result of the attraction between positive and negative ions...lots of energy is needed to break the bond Chemical Formula |
| Covalent Bond | 2 atoms share electrons |
| Polar Bond | Covalent bond in which electrons are shared unequally |
| Nonpolar Bond | Covalent bond in which electrons are shared equally |
| Conservation of Mass | In a chemical reaction, the total mass of the reactants must equal the total mass of the products |
| solvent | solution component that determines the state of matter of the solution (present in greatest amount) |
| solute | substance dissolved in solvent |
| molarity | mol solute volume solution |
| 1 ppm | 1mg L |
| 1ppb | 1mu g L |
| 1ppt | 1nano g L |
| molarity | varies with temperature if temp increases, then molarity decreases |
| molality | mol solute mass solvent, not temp dependent |
| mole fraction | xi is mol component i total mols of solution |
| mole percent | mole fractionx100 |
| ideal solution | no net energy change and change in volume=0 |
| nonideal solution | volume is less than sum of volumes |
| ion-dipole forces | attraction of water dipoles for cations and anions |
| miscible | liquids that mix in all proportions |
| saturated | when equilibrium between undissolved solute and solution, solute has attained its maximum value |
| solubility | concentration of the solute |
| unsaturated | any solution containing less solute than can be held at equilibrium |
| ionic compound solubility | 95% of ionic compounds have solubilities that increase significantly w increasing temp |
| solubility curve | graph of solubility as function of temperature |
| supersaturated | if a solution can be cooled without crystallization occurring |
| Henry's law | S=kPgas, increasing the pressure of a gas in contact w saturated solution increases the number of molecules per unit volume in gas |
| colligative properties | properties that depend on # of solute particles present but not on the identity of solute |
| Raoult's law | Psolv=xsolv*Pat temp solv, vapor pressure of the solvent above a solution is the product of the vapor pressure of solvent and the mole fraction of the solvent in solution |
| Raoult's law | strictly followed only in an ideal solution. not limited to the solvent if a solution also contains volatile solutes |
| fractional distillation | use constant pressure and boil a solution in n aparatus that does vaporizations and condenstations at a constant temp. |
| Kf | molal freezing point depression constant and molal |
| Kb | boiling point elevation constant |
| Semipermeable membranes | sheets or films of amaterial containing a network of microscopic holes or pores through which small solvent molecues can pass, but larger solute molecules cannot |
| Osmosis | net flow of solvent molecules through a semipermeable membrance from a solution of lower concentration to a solution of higher concentration |
| osmotic pressure | pressure required to stop osmosis |
| pi | osmotic pressure in atm |
| pi=MRT | (blank) |
| isotonic | solution hqving same osmotic pressure as body flluids |
| hypertonic | Chemistry Having the higher osmotic pressure of two solutions. |
| hypotonic | Chemistry Having the lower osmotic pressure of two fluids. |
| can't Hoff Factor | (i) used to modify equations for colligative properties by accounting for the presence of ions in solution |
| heterogeneous mixture | sand-water mix |
| colloids | mixtures that lie between true solutions and suspensions |
| colloid | dispersion in an appropriate medium of particles ranging in size from 1 nm to 1000 nm |
| tyndall effect | properties of colloids are diff from true solutions and suspensions. sometimes appear milky cloudy and scater beams of light passing through them |
| coagulate precipitate | high concentration of an electrolyte can cause this |
| electrodialysis | process facilitated by the attractions of ions to an electrode having the opposite charge |
| Q: Typical Composition of Natural Gas is? | A: Methane (CH4)70-90% |
| Q: CH4, Methane, makes up 70-90 % of natural gas. What 3 gases make up the next about 20% in varying amounts? | A: Ethane, C2H6 - 0-20% Propane,C3H8 - 0-20% Butane, C4H10 - 0-20% |
| Q: Why do we use chlorine at PB? | A: Chlorine is an oxidizing agent that distroys cell walls and nutrents in the water |
| Q: Where do we use chlorine at PB? | A: Circulating water, Service Water, and a couple more. Get specifics. |
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