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Final exam
old exam questions
57
Chemistry
10th Grade
05/24/2008

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Term
why is water an excellent solvent?
Definition
because of its polar nature
Term
metals can be pulled into a wire so they are?
Definition
ductile
Term
what intermolecular forces are in gases?
Definition
dispersion
Term
what substances are composed entirely of carbon
Definition
diamond and graphite
Term
describe formation of dispersion forces
Definition
Term
describe metallic bond
Definition
Term
what effect does an increase in temperature have on viscosity?
Definition
Term
why does ice float?
Definition
Term
why should experiments measuring heat exchange be in a calorimeter
Definition
Term
what happens to the temperature as liquid evaporates?
Definition
it decreases
Term
which states of matter are the only ones that can flow?
Definition
gases and liquids
Term
there is an iron cube and an aluminum cube that are the same temperature, how are their average kinetic energies different?
Definition
there is no difference
Term
what happens when energy is added to a boiling liquid?
Definition
the temperature does not change
Term
what happens when the vapor pressure of a liquid equals atmospheric pressure?
Definition
the liquid BEGINS to boil
Term
what is the solubility of a gas in a liquid directly proportional to?
Definition
the pressure of gas above liquid
Term
what doesn't ethanol dissolve in?
Definition
turpentine
Term
why does H2O have a greater boiling point than methane?
Definition
because strong hydrogen bonds are found between water molecules
Term
which of these are soluble and insoluble in water?

CuSO4
HCl
NaCl
CF4
Definition
all of them are soluble except for CF4
Term
how many grams of NaOH should be added to H2O to prepare 0.75L of solution w/molarity of 0.020?
Definition
.75L x (0.02/1L) x (40g/1 mol) = .6g
Term
what is osmotic pressure?
Definition
the downward push on the previously diluted solution that prevents any more solvent from passing through
Term
how will and what happens as the volume of the concentrated solution increases?
Definition
happens because more solvent is added and it results in an increase in pressure
Term
what does boiling point elevation do?
Definition
it changes the boiling point
Term
what happens to the reaction as you decrease the volume?
Definition
the forward reaction is favored so it shifts toward the product
Term
what is boiling point proportional to?
Definition
molality
Term
what is the solution outside of a cell when it is hypotonic?
Definition
less concentrated than the inside of the cell
Term
what is the equilibrium constant a measure of?
Definition
the extent to which a reaction proceeds to completion
Term
why does a solute depress the freezing point?
Definition
because the solute disrupts the crystal formation of the solvent
Term
which subatomic particle controls properties?
Definition
the electrons
Term
what is the solubility product and what info does it give about an aqueous solution of an ionic solid?
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
Term
what is the relationship between Le Chatelier's principle and the common ion?
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.
Term
a volatile liquid is?
Definition
one that evaporates easily
Term
why does the equilibrium vapor pressure increase with an increase in temperature
Definition
because there are more particles with higher kinetic energy that want to escape and therefore collide with the container they are in
Term
a substance with a low heat of vaporization has what kind of intermolecular forces?
Definition
weak intermolecular forces
Term
why do gas particles have the most potential energy?
Definition
because of the large spaces between the particles
Term
what measures the average kinetic energy of the particles in an object
Definition
temperature
Term
when does deposition occur?
Definition
when a gas is converted directly into a solid
Term
when a solid is converted into a liquid is it endo or exothermic process?
Definition
endothermic
Term
when do all 3 states of matter exist in equilibrium
Definition
at the triple point
Term
when does dynamic equilibrium exist?
Definition
when the rate of vaporization equals the rate of condensation
Term
under what conditions wil a liquid boil
Definition
when the vapor pressure equals the atmospheric pressure
Term
electrolyte is...?
Definition
a substance that dissolves in water to form a solution that conducts an electric current
Term
molality is not affected by what?
Definition
changes in temperature
Term
a solution containing the maximum amount of solute to a given amount of solvent is
Definition
super saturated
Term
what solution has water as the solvent?
Definition
aqueous
Term
miscible includes
Definition
liquids that can mix each other
Term
what does Raults law state?
Definition
that the magnitude of vapor pressure reduction is proportional to the solutions concentration
Term
volatile is ?
Definition
a substance that will become a gas under existing conditions
Term
what effect does adding solute to solvent have on the freezing point?
Definition
it lowers it
Term
what effect does the addition of a solute have on the vapor pressure?
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.
Term
what are the five kinds of chemical reactions?
Definition
synthesis, decomposition, single replacement, double replacement, and combustion
Term
synthesis?
Definition
two or more substances combining to make a more complex substance

A + B = AB
Term
single replacement?
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
Term
decomposition?
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
Term
double relacenment
Definition
two elements in two compounds change places
so that
AB + CD ---> AD + CB
Term
combustion
Definition
hydrocarbon + oxygen ---> carbon dioxide + water
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
Term
metric conversions?
Definition
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