Term
| What cannot be broken down or decomposed? |
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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
rigid, geometric, network lattice
definite shape and definite volume
particles vibrate in fixed position
closely packed particles
strong intermolecular forces
small distance between particles |
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Term
|
Definition
definite volume , no definite shape
has surface tension and viscosity
particles can flow past one another |
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Term
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Definition
spreads to fill the entire container
no definite shape no definite volume
random, constant , straight-line motion
weak intermolecular forces |
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Term
|
Definition
forces between molecules
solids have strong forces, and gases have weak forces |
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Term
| what is AVERAGE KINETIC ENERGY? |
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Definition
energy of particle motion
TEMPERATURE |
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Term
| when does potential energy change? |
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Definition
changes during a phase change
energy of how the particles are spread out |
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Term
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Definition
elements and compounds
only one type of particle |
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Term
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Definition
| a combinations of elements and/or compounds |
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Term
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Definition
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Term
| KINETIC MOLECULAR THEORY OF GASES |
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Definition
* gases move in constant random straight line motion
* gases do not lose or gain energy when they collide -- they have elastic collisions
*gas particles have a volume that is insignificant compared to the volume of the total gas
* average kinetic energy is temperature
* gas particles have no significant forces between them |
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Term
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Definition
high temperature -- move very fast
low pressure -- very far apart |
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Term
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Definition
solid -liquid equilibrium
(s)-->(l) |
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Term
| VOLUME -TEMPERATURE OF GASES |
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Definition
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Term
|
Definition
solid-liquid equilibrium
(l)-->(s) |
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Term
BOILING /EVAPORATION
VAPORIZATION |
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Definition
liquid-gas equilibrium
(l)-->(g) |
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Term
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Definition
liquid-gas equilibrium
(g) --> (l) |
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Term
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Definition
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Term
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Definition
(g) --> (s)
like frost on your windows |
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Term
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Definition
temperature does NOT change
kinetic energy does not change
potential energy changes |
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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
gram formula mass
(add up the pieces using mass from the Periodic Table) |
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Term
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Definition
A3 + 2B --> AB2
coming together to make one product |
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Term
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Definition
1 reactant breaking down into more than one product
AB ---> A + B |
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Term
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Definition
1 element and 1 compound replacing part of each other
A + BC --> B + AC |
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Term
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Definition
compound 1 + compound 2 replacing part of each other
ex. PbCl + K(NO3) --> KCl + Pb(NO3) |
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Term
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Definition
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Term
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Definition
| boiling, melting, freezing, condensation, evaporation, solidifcation,sublimation, deposition |
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Term
| 5 types of CHEMICAL REACTIONS |
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Definition
| synthesis, decomposition, single replacement, double replacement, combustion |
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Term
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Definition
| the simplest unit of an element |
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Term
| Which subatomic particles have mass? |
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Definition
protons and neutrons
a mass of 1 amu each |
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Term
| Which subatomic particle has almost no mass and is very small? |
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Definition
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Term
| According to the wave mechanical model of the atom, where are electrons located? |
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Definition
| orbitals , regions of high probability of finding an e- |
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Term
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Definition
| electrons in the outermost shell (the last number in the e- configuration) |
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Term
|
Definition
same protons and atomic number and symbol
different mass number and different numbers of NEUTRONS |
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Term
How do we calculate atomic mass?
( THIS IS NOT MASS NUMBER!!) |
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Definition
mass multiply by abundance (in decimal percent , to the left, to the left like Beyonce :) The abundance decimal point gets moved NOT the mass.
C-12 mass 12.01 abundance 98.7%
(12x0.987) + ... |
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Term
|
Definition
the most likely region to find an electron
(areas of high probability) |
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Term
|
Definition
1) e- absorb energy
2) go to a higher level "excited state" (unstable)
3) go to a lower level
4) release a photon of light (bright line atomic spectra) |
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Term
|
Definition
| number of protons + number of neutrons (added up) |
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Term
|
Definition
number of protons
can be found on the periodic table |
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Term
| ATOM ELECTRICALLY NETURAL |
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Definition
| because # of protons = # of electrons |
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Term
|
Definition
| electron jumped up to a higher energy shell |
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Term
| BRIGHT LINE ATOMIC SPECTRA |
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Definition
unique "fingerprint" that can identify an element
produced when electron goes to a lower energy level and releases photon of light |
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Term
|
Definition
positive and has the most mass
weakest power |
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Term
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Definition
most penetrating power
pure energy
no mass , no charge |
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Term
|
Definition
nuclear power
U + n --> Ba + Kr + 3 n + energy
to split apart |
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Term
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Definition
H + H --> He + energy
to combine |
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Term
|
Definition
one element decaying and becoming a new element
X --> |
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Term
|
Definition
one element and a particle becoming a new element
X + beta/gamma/alpha ---> |
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Term
|
Definition
I-131 thyroid treatment
Co-60 cancer
C-14 date organic material
U-238 date rocks |
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Term
| PROS and CONS NUCLEAR POWER |
|
Definition
pros + cheap, clean, less pollution
cons - radioactive waste, possible breakdown and radiation leaks/sickness |
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Term
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Definition
the time it takes for a sample size to decay with only half remaining
half-life is a steady, constant rate |
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Term
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Definition
| gases at the same temp and pressure, will have equal volume and equal number of molecules |
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Term
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Definition
| Given a balanced equation, if the problem goes from moles to moles - --use molar ratios to solve |
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Term
|
Definition
mass and charge are both conserved
Given a balanced equation
if a problem is about grams and grams - - use conservation of mass to add/subtract to find the answer |
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Term
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Definition
electrons in the outermost shell
the last number in an electron configuration |
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Term
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Definition
have same number of valence e-
same group |
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Term
|
Definition
radii get smaller (positive nucleus pulls e- inward)
IE increases
EN increases
less metallic character |
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Term
|
Definition
atomic radii get larger, more e- shells
IE decreases
EN decreases
metallic character increases |
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Term
|
Definition
lose e-
malleable
luster/shiny
solid (except mercury)
ductile
good conductors b/c of free mobile e- (sea of e-)
hi density
*they become totally different when they react to become ionic
want to lose e |
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Term
|
Definition
dull
brittle
solids or gases (except Br)
poor conductors (no free mobile e-)
want to gain e- , high EN |
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Term
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Definition
metals with nonmetals
transfer of e-
high melt point
dissolve /soluble in water
conducts in water (electrolyte) |
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Term
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Definition
nonmetal with nonmetal
shares e-
low melt point |
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Term
|
Definition
shares unevenly
EN difference high
asymmetrical
soluble in water |
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Term
|
Definition
shares evenly
EN difference low or zero
symmetrical
insoluble in water
poor conductor |
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Term
|
Definition
dot represent valence e-
if more than one atom present, show how the electrons are transferred (if ionic) or shared (if covalent) |
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Term
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Definition
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Term
|
Definition
heat is absorbed
A + heat --> B + C
feels cool , because the rxn absorbs energy from the surroundings
heat of reaction is +
Table I |
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Term
|
Definition
heat is released
A --> B + C + heat
feels warm, because the rxn releases energy to the surroundings
heat of reaction is -
Table I |
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Term
|
Definition
disorder of a system
solid is least , gases are the most
the more molecules the more disorder |
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Term
| Nature and SPONTANEOUS RXNS |
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Definition
greater disorder , more entropy
usually also exothermic, but not always |
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Term
|
Definition
there must be collisions for molecules to react
there must me sufficient energy to react
there must be more stability in the products formed |
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Term
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Definition
| if the reaction rate increases, the time it takes is less |
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Term
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Definition
| higher temp, more kinetic energy, more collisions, faster rxn |
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Term
| CONCENTRATION AND RXN RATE |
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Definition
| more particles per volume, more collisions, faster rxn |
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Term
| SURFACE AREA AND RXN RATE |
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Definition
| crushing/powder, grinding makes more surface area for more possible collisions, faster rxn |
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Term
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Definition
| Table J, higher is more reactive |
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Term
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Definition
| creates an alternate pathway with a lower activation energy ( faster) |
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Term
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Definition
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Term
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Definition
| the minimum energy required for the rxn to occur |
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Term
|
Definition
H+ donor
H..., usually
sour
reacts with metals
pH below 7 |
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Term
|
Definition
H+ acceptor
...OH, usually
bitter
slippery
pH above 7 |
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Term
|
Definition
| Acid + Base ---> ionic salt and HOH |
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Term
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Definition
| moles of solute / liter of solution |
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Term
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Definition
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Term
|
Definition
| increase H+ by 10*10 = 100 times more acidic |
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Term
|
Definition
decrease in H+ 10^3 = 1000 less basic (going closer to neutral)
1/1000 of H+ |
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Term
|
Definition
lose electrons oxidation
oxidation # goes up
e- are on the product side
oxidized
reducing agent |
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Term
|
Definition
gain e- reduction
e- are on the reactant side
oxidation # goes down
reduced
oxidizing agent |
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Term
|
Definition
|
|
Term
|
Definition
anode is where oxidation occurs
cathode is where reduction occurs |
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Term
| voltaic cell vs electrolytic |
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Definition
voltaic requires a salt bridge that lets ions flow
voltaic, no battery , so it is spontaneous
voltaic : chemical energy converted to electrical
electrolytic requires a battery, not spontaneous
electrolytic : electrical energy converts to chemical energy |
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Term
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Definition
solute gets dissolved
solvent does the dissolving |
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Term
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Definition
| different particles not evenly spread out |
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Term
|
Definition
Solutions
if in water, aqueous |
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Term
SEPARATE BY SIZE
LIKE HETEROGENEOUS MIXTURES |
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Definition
| filtration (like sand and water) |
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Term
| SEPARATE INKS DYES, COLORS |
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Definition
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Term
| SEPARATE BY BOILING POINT |
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Definition
distillation
like crude oil (fractional distillation) |
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Term
|
Definition
dissolved solids in water/liquids
like salt water |
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Term
| ADDING MORE PARTICLES MAKE THE |
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Definition
freezing point go down
boiling point go up
vapor pressure go down
osmotic pressure go up |
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Term
| SUPERSATURATED, SATURATED, UNSATURATED |
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Definition
supersaturated= above the accepted value,
saturated = equal to the accepted value
unsaturated = less than the accepted value |
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Term
|
Definition
Solid in solution,
occurs when something is insoluble |
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Term
| What has a fixed ratio or proportion? |
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Definition
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|
Term
If a substance has a high boiling point what kind of intermolecular forces does it have?
Conversely, low boiling point? |
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Definition
strong or high
Low boiling point means lower intermolecular forces |
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Term
| Which two subatomic particles have the same quantity of charge but opposite signs? |
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Definition
| proton +1, and electron -1 |
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|
Term
| Which subatomic particle holds the nucleus together? |
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Definition
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|
Term
| Which subatomic particle is equal to the atomic number? |
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Definition
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|
Term
| Which two subatomic particles have the same quantity of charge but opposite signs? |
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Definition
| proton +1, and electron -1 |
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|
Term
| Which subatomic particle holds the nucleus together? |
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Definition
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|
Term
| Which subatomic particle is equal to the atomic number? |
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Definition
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|
Term
| Which subatomic particle has no charge? |
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Definition
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|
Term
| Which subatomic particle has a charge of -1? |
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Definition
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|
Term
| What does NOT change during excited state? |
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Definition
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|
Term
| How do we calculate atomic mass of isotopes? |
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Definition
| take the weighted average of all the naturally occurring isotopes |
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Term
|
Definition
|
|
Term
| chemical energy into electrical |
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Definition
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|
Term
| electrical energy into chemical energy |
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Definition
|
|
Term
| How do the boiling points of water and a solution compare? |
|
Definition
the solution will have a higher boiling point and lower freezing point
(boiling pt elevation and freezing pt depression) |
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Term
| How are C graphite and C diamond different? |
|
Definition
| different structures so different properties |
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Term
| How are allotropes different? |
|
Definition
| different structures and different properties |
|
|
Term
| What makes something organic? |
|
Definition
|
|
Term
| What elements are in a hydrocarbon? |
|
Definition
|
|
Term
| What is a saturated molecule? |
|
Definition
| all single bonds = alkanes |
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|
Term
| What is an unsaturated molecule? |
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Definition
| contains at least 1 multiple bond (double or triple) |
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Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| What reaction produces polymers? |
|
Definition
|
|
Term
| What reaction produces esters? |
|
Definition
|
|
Term
| What reaction produces alcohol? |
|
Definition
|
|
Term
| CH4 + Cl2 ==> CH3Cl + HCl |
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Definition
|
|
Term
| What are esters made from? |
|
Definition
|
|
Term
| What element can make long chains, rings and networks? |
|
Definition
|
|
Term
| How many electrons are shared in a triple bond? |
|
Definition
|
|
Term
|
Definition
| when forward and reverse reaction rates are equal and the concentration of the reactants and the products remains constant |
|
|
Term
| What is Le Chatelier's Principle? |
|
Definition
| that a system in equilibrium , when disturbed, will shift and return to equilibrium |
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|
Term
| What type of bonding gives water an unusually high boiling point? |
|
Definition
|
|
Term
| What are the 3 types of hydrogen bonds? |
|
Definition
H-N H-O H-F
because of high EN |
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|
Term
| A system in equilibrium, when pressure is increased will shift towards ________ |
|
Definition
| the side with less moles of gas |
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Term
| A system in equilibrium, when pressure is decreased will shift towards ________ |
|
Definition
| the side with more moles of gas |
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