Term
| why is water an excellent solvent? |
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Definition
| because of its polar nature |
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Term
| metals can be pulled into a wire so they are? |
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Definition
|
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Term
| what intermolecular forces are in gases? |
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Definition
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Term
| what substances are composed entirely of carbon |
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Definition
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Term
| describe formation of dispersion forces |
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Definition
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Term
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Definition
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Term
| what effect does an increase in temperature have on viscosity? |
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Definition
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Term
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Definition
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Term
| why should experiments measuring heat exchange be in a calorimeter |
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Definition
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Term
| what happens to the temperature as liquid evaporates? |
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Definition
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Term
| which states of matter are the only ones that can flow? |
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Definition
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Term
| there is an iron cube and an aluminum cube that are the same temperature, how are their average kinetic energies different? |
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Definition
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Term
| what happens when energy is added to a boiling liquid? |
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Definition
| the temperature does not change |
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Term
| what happens when the vapor pressure of a liquid equals atmospheric pressure? |
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Definition
| the liquid BEGINS to boil |
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Term
| what is the solubility of a gas in a liquid directly proportional to? |
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Definition
| the pressure of gas above liquid |
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Term
| what doesn't ethanol dissolve in? |
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Definition
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Term
| why does H2O have a greater boiling point than methane? |
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Definition
| because strong hydrogen bonds are found between water molecules |
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Term
which of these are soluble and insoluble in water?
CuSO4
HCl
NaCl
CF4 |
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Definition
| all of them are soluble except for CF4 |
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Term
| how many grams of NaOH should be added to H2O to prepare 0.75L of solution w/molarity of 0.020? |
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Definition
| .75L x (0.02/1L) x (40g/1 mol) = .6g |
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Term
| what is osmotic pressure? |
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Definition
| the downward push on the previously diluted solution that prevents any more solvent from passing through |
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Term
| how will and what happens as the volume of the concentrated solution increases? |
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Definition
| happens because more solvent is added and it results in an increase in pressure |
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Term
| what does boiling point elevation do? |
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Definition
| it changes the boiling point |
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Term
| what happens to the reaction as you decrease the volume? |
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Definition
| the forward reaction is favored so it shifts toward the product |
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Term
| what is boiling point proportional to? |
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Definition
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Term
| what is the solution outside of a cell when it is hypotonic? |
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Definition
| less concentrated than the inside of the cell |
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Term
| what is the equilibrium constant a measure of? |
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Definition
| the extent to which a reaction proceeds to completion |
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Term
| why does a solute depress the freezing point? |
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Definition
| because the solute disrupts the crystal formation of the solvent |
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Term
| which subatomic particle controls properties? |
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Definition
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Term
| what is the solubility product and what info does it give about an aqueous solution of an ionic solid? |
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Definition
| the sp is represented in equations by Ksp. It tells how soluble an ionic solid is in a certain aqueous solution. Increase in Ksp means highly soluble and a decrease in Ksp means not very soluble |
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Term
| what is the relationship between Le Chatelier's principle and the common ion? |
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Definition
| LC says when you put stress through temperature, concentration or pressure, the system works to relive the stress. When a common ion is added it increases the concentration of that ion and the system will shift to the left. |
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Term
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Definition
| one that evaporates easily |
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Term
| why does the equilibrium vapor pressure increase with an increase in temperature |
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Definition
| because there are more particles with higher kinetic energy that want to escape and therefore collide with the container they are in |
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Term
| a substance with a low heat of vaporization has what kind of intermolecular forces? |
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Definition
| weak intermolecular forces |
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Term
| why do gas particles have the most potential energy? |
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Definition
| because of the large spaces between the particles |
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Term
| what measures the average kinetic energy of the particles in an object |
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Definition
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Term
| when does deposition occur? |
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Definition
| when a gas is converted directly into a solid |
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Term
| when a solid is converted into a liquid is it endo or exothermic process? |
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Definition
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Term
| when do all 3 states of matter exist in equilibrium |
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Definition
|
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Term
| when does dynamic equilibrium exist? |
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Definition
| when the rate of vaporization equals the rate of condensation |
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Term
| under what conditions wil a liquid boil |
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Definition
| when the vapor pressure equals the atmospheric pressure |
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Term
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Definition
| a substance that dissolves in water to form a solution that conducts an electric current |
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Term
| molality is not affected by what? |
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Definition
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Term
| a solution containing the maximum amount of solute to a given amount of solvent is |
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Definition
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|
Term
| what solution has water as the solvent? |
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Definition
|
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Term
|
Definition
| liquids that can mix each other |
|
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Term
| what does Raults law state? |
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Definition
| that the magnitude of vapor pressure reduction is proportional to the solutions concentration |
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Term
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Definition
| a substance that will become a gas under existing conditions |
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Term
| what effect does adding solute to solvent have on the freezing point? |
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Definition
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Term
| what effect does the addition of a solute have on the vapor pressure? |
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Definition
| when you add solute you have solute mixed with solvent and fewer solvent particles at surface because the solute particles cause an interference, so fewer can escape. |
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Term
| what are the five kinds of chemical reactions? |
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Definition
| synthesis, decomposition, single replacement, double replacement, and combustion |
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Term
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Definition
two or more substances combining to make a more complex substance
A + B = AB |
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Term
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Definition
a neutral element becomes an ion as it replaces another ion in the compound
n the case of a positive ion being replaced: A + BC ----> B + AC
or
In the case of a negative ion being replaced: A + BC ----> C + BA |
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Term
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Definition
one substance is broken down into two or more, simpler substances. This type of reaction is the opposite of a synthesis reaction
AB---> A+B |
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Term
|
Definition
two elements in two compounds change places
so that
AB + CD ---> AD + CB |
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Term
|
Definition
| hydrocarbon + oxygen ---> carbon dioxide + water |
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Term
| charges of the monoatomic ions? |
|
Definition
group and charge
1 is +1
2 is +2
13 is +3
15 is -3
16 is -2
17 is -1
18 is 0 |
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Term
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Definition
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