Term
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Definition
time(s)
length(m)
Mass(kg)
Temperature(K)
amount of substance(Mole) |
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Definition
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Definition
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Definition
if making the number "bigger"(-)
if making the number "smaller"(+) |
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Definition
| when(+) or (-) use the least amount of sig figs |
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Definition
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Definition
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Definition
experimental - accepted
divided by accepted value
times 100 |
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Term
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Definition
particles vibrate but cannot move aroung
fixed shape
not compressible
fixed volume |
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Term
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Definition
particles can move around but are still close together
not compressible
fixed volume |
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Term
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Definition
Particles can separate and move freely in container
compressible
variable volume |
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Term
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Definition
Can be observed w/o changing the identity of the substance
melting, boiling point,density |
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Term
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Definition
describes the ability of a substance to undergo changes in identity
flammable,tarnishes in air |
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Term
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Definition
Changes the form of the substance without changing its identity
phase changes |
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Term
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Definition
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Term
| Law of conservation of mass |
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Definition
| mass neither be created or destroyed |
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Term
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Definition
evaporation L to G
condensation G to L
melting S to L
freezing L to S
sublimation S to G
deposition G to S |
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Term
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Definition
medium to large sized particles that do not settle
salad dressing |
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Term
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Definition
small particles form a solution
particles do not settle
rubbing alchohol |
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Term
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Definition
| seperate substances based on their attraction to the water and their ability to be drawn across te paper |
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Term
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Definition
| differences in boiling points |
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Term
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Definition
| porous barrier separates solids and liquids |
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Term
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Definition
| solid changges into a vapor without melting |
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Term
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Definition
a pure substance made of the same type of atom
117
cannot be broken down |
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Term
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Definition
conatins atoms of different elements chemically combined together
formula |
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Term
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Definition
| anything that has mass and takes up space |
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Term
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Definition
| first proposed the idea of an atome |
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Term
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Definition
| protons and neutrons surrounded by an electron cloud |
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Term
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Definition
1- charge
elctron cloud
0 amu
J.J. discovered it using the cathode ray |
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Term
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Definition
1+ charge
1 amu
nucleus
Rutherford discovered it using the gold foil experiment |
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Term
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Definition
0 charge
nucleus
1 amu
Chadwhick |
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Term
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Definition
| a unit of amss used to express weight of atoms and molecules |
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Definition
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Definition
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| how to read the periodic table |
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Definition
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Term
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Definition
| (mass of first isotope)(X) + (mass of second isotope)(1-X)solve for x and plug it in |
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Definition
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Definition
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Definition
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Definition
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Definition
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Term
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Definition
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Term
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Definition
Total Time = (length of one half-life) (# of half lives)
Remaining Mass = initial mass / 2 number of half lives
Initial Mass = (remaining mass) (2 number of half lives )
(2 number of half lives ) = initial mass/remaining mass |
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Term
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Definition
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Term
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Definition
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Term
colors of the electro-magnetic spectrum
(lowest to highest frequency) |
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Definition
| red orange yellow green blue indigo violet |
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Term
| electromagnetic spectrum(longest to shortest wavelength) |
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Definition
| Radio micro infrared visible ultraviolet x-rays gamma rays |
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Term
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Definition
3.00*10^8 m/s
3.00 * 10 ^17 nm/s |
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Term
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Definition
| treats electron as a wave |
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Term
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Definition
electrons move in exact paths called orbitals
only worked for hydrogen |
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Term
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Definition
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Term
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Definition
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Term
| how many electrons can each orbital hold |
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Definition
| 2 electrons with opposite spin |
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Term
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Definition
| splitting a heavy nucleus into two nuclei with smaller masses |
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Term
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Definition
| two small nuclei are joined together |
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Term
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Definition
| Mass Defect = (mass of isotope) – (# of p+) (mass of one proton) – (# of neutrons) (mass of one neutron) |
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Term
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Definition
principle quantum number
specifies the energy level and the energy of an electron in an atom |
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Term
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Definition
azimuthal quantum number specifies the sub level and the shape of the orbital
§l = 0 corresponds to a s sublevel
§l = 1 corresponds to a p sublevel
§l = 2 corresponds to a d sublevel
§l = 3 corresponds to an f sublevel |
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Term
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Definition
magnetic quantum number specifies orbitals and labels the different orbitals of a given sublevel
§So, if l = 0 (an s orbital), ml =0
§If l = 1 (a p orbital), ml =-1, 0, +1
§If l = 2 (a d orbital), ml =-2,-1,0,+1,+2
§If l = 3 (an f orbital), ml = -3,-2,-1,0,+1,+2,+3 |
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Term
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Definition
spin quantum number
specifies the direction of spin of the two electrons within an orbital |
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Term
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Definition
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Term
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Definition
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Term
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Definition
| there is a periodic repetition of chemical and physical properties when elements are arranged in increasing atomic number |
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Term
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Definition
Alkali metals
left
1 valence electron
very reactive
lose |
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Term
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Definition
Alkaline Earth metals
left
2 valence
reactive
gain |
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Term
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Definition
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Term
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Definition
halogens right 7
reactive gain |
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Term
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Definition
noble gases
right
8 valence
very stable
neither |
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Term
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Definition
left
good conductors of heat and electricity
malleable
ductile
luster
lose electrons when they are heated |
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Term
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Definition
staircase elements
less brittle
semiconductors of electricity
some have luster |
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Term
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Definition
right
poor conductors of heat and electricity
brittle
many are gases
gain or share when they heat |
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Term
| 4 blocks of the periodic table |
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Definition
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Term
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Definition
the energy required to remove the outermost electron from a gaseous atom
increase across
decrease down |
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Term
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Definition
measure of the ability of an atomic to attract electrons
increase across
decrease down |
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Term
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Definition
| neutral atoms likely-hood of gaining an electron |
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Term
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Definition
| atoms want 8 valence electrons |
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Term
| successive ionization energy |
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Definition
| it takes more an more energy each time you remove an electron |
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Term
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Definition
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Term
| properties of ionic compounds |
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Definition
good conductors of electricity when in aqueous state and when in molten state
hard rigid brittle |
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Term
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Definition
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Term
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Definition
| number of valence electrons in a circle |
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Term
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Definition
| valence electrons are removed and are used by all toms |
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Term
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Definition
| a shared pair of electrons |
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Term
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Definition
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| differences in electronegativity pull the electrons to one side of a compound |
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Term
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Definition
0 nonpolar
less than .4 mostly covalent
.4 to 1.7 polar covalent
greater than 1.7 ionic |
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Term
| 7 shapes of the molecules |
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Definition
trigonal planar
linear
tetrahedral
pyramidal
bent
trigonal pyramidal
octahedral |
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Term
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Definition
| reactant+reactant=product |
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Term
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Definition
A+B=AB
combustion (something burns) |
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| element that are lower on the activity series cannot replace things higher on the activity seies |
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Term
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Definition
1mol=6.2X10^23
avagadro's number |
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Term
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Definition
| relationship between the number of particles and volume of a gas |
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Term
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Definition
| mass of 1 mol of an element or compound |
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Term
| law of definite proportions |
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Definition
| a compound is always composed of the same elements in the same proportion no matter how large or how small the sample size |
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Term
| Law of multiple proportions |
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Definition
| masses of one element that combine with a fixed mass of another will do so in a ratio of small whole numbers. |
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Term
| percent mass of an element in a compound |
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Definition
| %comp.=total mass of element/total mass of compound (X 100) |
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Term
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Definition
| smallest whole number ratio of elements in a compound |
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Term
| finding the empirical formula |
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Definition
1. find the mass of each element
2. fin the moles of each element
3. divide moles by the smallest number to find subscripts
4. must be whole numbers |
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Term
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Definition
| "true formula" the actual number of atoms in a compound, either the same as or a whole-number multiple of the empirical formula |
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Term
| finding the molecular formula |
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Definition
1. Find the EF
2. find the EF mass
3. Divide Molar Mass(given in problem)by the empirical formula mass
4. Multiple each subscript in your EF by the from step 3 |
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Term
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Definition
| Any salt that has water chemically bonded to the ions in the crystal structure is a hydrate or hydrated crystal |
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Term
| Writing formulas and names of hydrates |
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Definition
| numerical prefixes are used to indicate the # of water molecules that are attached to the ionic compound |
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Term
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Definition
| a substance that absorbs water from the air is said to be hygroscopic |
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Term
| finding the hydrate formula |
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Definition
1. determine grams of h20 lostt due to heating
2. convert g H20 to moles & convert g of anhydrate to moles
3. divide moles of H20/moles of anhydrate |
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Term
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Definition
| determines the amount of product that can be formed b/x it gets up b4 the other reactants |
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Term
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Definition
| other reactants that areleft over when a reaction stops |
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Term
| determining limiting reactant |
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Definition
Determine which reactant is limiting by converting the grams of each reactant to moles and then dividing each answer by its coefficient given in the equation. The reactant with the smallest answer is the limiting reactant.
2. use stoichiometry to determine the amount of product produced by the moles of limiting reactant |
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Term
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Definition
measure of the efficiency of a chemical reaction
theoretical yield-the calculated amount
actual yield- amount produced when the reaction is carried out in the lab |
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Term
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Definition
expand to fill their containers
fluid
low density
compressible
effuse and diffuse |
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Term
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Definition
particles are always in motion
volume of individual particles=zero
collisions of the particles with container walls causue the pressure exterted
particles exert o forces on each other
average kinetic energy is proportional to K temp of a gas |
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Term
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Definition
ELASTIC
when particles collide no energy is lost |
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Term
| kinetic energy of gas particles |
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Definition
all have the same average kinetic energy
KE=(1/2)mv^2
@ the same temp small molecules move FASTER than large molecules |
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Term
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Definition
rate of gas mixing
result of random movement of gas particles
rate increases with temperature
small faster than large
high to low concentration |
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Term
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Definition
| gas escaping from a tiny opening |
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Term
| Grahms law of diffusion and effusion |
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Definition
high to low concentration
rate of diffusion/effusion for a gas is inversely proportional tothe square root of the MM of the gas |
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Term
| Grahms Law of Diffusion and Effusion |
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Definition
| rate of a/rate of b=M of B/M of A |
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Term
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Definition
force per area unit
gases exert_____________ when they collide with he sides of their container |
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Term
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Definition
pressure exerted by the stomsphere
lower at higher altitudes
measured with a barometer |
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Term
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Definition
| pressure is equal tothe difference in hight of HG in the two arms |
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Term
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Definition
| pressure of gas equal 750-height difference |
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Term
| Dalton law of partial pressure |
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Definition
| the total pressure of a mixture of gases is the sum of the pressure of all the gases in the mixtures |
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Term
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Definition
| holds atoms/ions together in ionic, covalent, or metallic bonds |
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Term
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Definition
hold identical molecules together
generally weaker that covalent bonds
dipole-dipole,hydrogen, London dispersion |
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Term
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Definition
a molecule or a part of a molecule that contains both partial positive and partial negative regions
created when ther is a large difference in EN |
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Term
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Definition
have a large difference in eletronegativity, thus creating a large dipole, or hihgly polar bond
VERY strong attraction |
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Term
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Definition
| the constant motion fo electrons create temporary dipoles |
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Term
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Definition
definite volume but no definite shape(take that of the container)
high density
not compresabel
diffuse
surface tension
fluid |
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Term
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Definition
the resistance fo a liquid to flow
stronger intermolecular forces mean higher viscosity |
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Term
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Definition
| the rise of liquids through slim tubes or permeable substances due to sdhesive and cohesive forces; adhesive>cohesive |
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