AP Chemistry

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Chemistry

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395 Terms

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Electron Config
The atoms orbital config
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Chemistry
study of what is in stuff reacting with other stuff
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Matter
The stuff
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Elements
pure substances that is a single element
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Compounds
pure substances that is two or more element
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Homogeneous
evenly distributed different mixture
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Heterogeneous
chemically bonded elements not evenly distributed
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protons or atomic number
How does the periodic table distribute its elements
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P+\>e-
cation
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P+
anion
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isotopes
difference of neutrons in the same elements
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What is most helpful when determining if a substance is pure?
Mass percent of the element
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avagadro's number
6.022x10²³\=1mole
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mass spectrometry
A bar graph showing the different isotopes of an element. The total equals the element on the periodic table.
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percent composition
summing atoms weight and dividing each individual by the sum.
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empirical formula
Finding the ratio of atoms by making percents to equal grams by 100%\=100g then turn to moles by timing m/g then dividing by the lowest atom and rounding others to nearest atom
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molecular formula
the actual composition of a compound by taking empirical formula with actual mass
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sig figs
The number of numbers that are relevant for a solution. (no leading zeros, sandwiched zeros are sig, yes trailing zeros if zero, yes none zeros)
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proton
+in the nucleus with a weight of 1.00727
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neutron
0in the nucleus with a weight of 1.00866
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electron
-in the ion cloud with a weight of .00055
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coulombs law (q\=attraction)(r\=distance)
(q_1q_2)/r^2
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S config
first config of a layer a circle 2
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P config
starts 2nd layer and second config of the layer a figure eight 3
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D config
third level of atom a d shape 2
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F config
last level of atom a shape
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photoelectron spectroscopy
peaks showing the number of electrons from shells and energy use
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Ionization energy (IE)
energy to remove an electron the (increase right and up)
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electronegativity
ability to attract electrons ( increase right and up)
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atomic radius/ radii
The distance of an electron from the nucleus (increase left and down)
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ionic bond
metal and a nonmetal strongest bond ∆en 1.7-4.0
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covalent bond
2 non metals
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metalic
2 metals
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hun's law
if atoms can fill out they would
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polar covalent
∆en.3-1.7
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non polar covalent
∆En0-.3
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intra molecular forces
forces that impact bonding
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perfect bond length
attractive forces \= repulsive forces
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determining strength of bonds
1 coulomb's law, 2 bond energy, 3 bond length, 4 atom size, 5 \# of bonds
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coulomb's law
(q1*q2)/r^2
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bond energy
Kj of energy (higher \= harder)
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bond length
distance of atoms (closer\=harder)
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atom size
size of atom (smaller\=harder)
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\# of bonds
1-3 bonds of an atom (more\=harder)
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crystal lattice
alternating repeating atoms that are ionic
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metal
sea of electrons (made of same element)
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alloy
substitutional and interstitial (made of a mix of metals)
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substitutional
Two compound of relatively similar size switch atoms.
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interstitial
Two compound of different sizes combine between bigger atoms.
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formal charge (FC)
V-NB-b/2\=FC determines which element is more neutral. (valence, non-bonding, bond e-,)
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VESPR
used to determine 3d aspects of an atom (valence, shell, electron, pair, repulsion)
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2 domains
linear sp 180˚
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3 domain
trigonal planar 120˚ or lp bent
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4 domain
trigonal planar 109.5˚, or lp trigonal pyramid
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resonance structures
structures that can change orientation while being the same compound. Usually carbon and is due to equal lengths.
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intramolecular forces
attractions within molecules
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polarity of intermolecular forces
The high difference in electronegativity for covalent and ionic compounds (ionic always)
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dipole
the attractions of a positive and negative polarity (greater difference \= stronger dispersion forces)
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London dispersion forces (LDF)
In temporary fluctuating dipoles, electrons are unevenly distributed to one side. (Changes are dependent on temp decrease \= greater IMF)
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dipole-dipole
attractions between oppositely charged regions of polar molecules
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dipole-induced dipole
The partial charge on a polar molecule induces a temporary partial charge on a neighboring non polar molecule or atom
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ion-dipole
the charge of an ion is attracted to the partial charge on a polar molecule.
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hydrogen bonding
strongest of the bonds (hydrogen is always positive)(N, O, F)
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Increasing IMF
Closer contact by greater size or bigger charge difference.
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Effects of greater IMF
greater Breaking point, higher melting point, greater surface tension, lower vapor pressure.
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Vapor pressure
The amount of free floating atoms based on temp.
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pv\=nRt
Pressure x Volume \= \# of moles x Gas Constant x Temperature
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Pressure (P)
Measured in atmospheres STP 1 (KPA .00987 \= atm 1)
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volume (L)
Measured in Liters (L) STP 22.4
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moles (n)
6.023*10^23 represented by mol The number of atoms present.
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constant (R)
.08206 atm
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temperature (T)
Measured in kelvin (K) average speed of atoms. (atoms can be going different speed)
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boil's law
as P increases V decrease p*v\=p*v
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Charles' law
as v increase T increases. v/t\=v/t
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Gay-Lussac's Law
as P increase T increases. p/t\=p/t
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Avagadro's Law
as V/n \= constant
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Dalton's law
total pressure\= p1+p2+p3+...
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Assumptions of Kinetic molecular theory
gas particles have "no" volume
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gas particle feel no attractions

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constant motion

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Kinetic energy (Ke)
Speed of atoms
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mass
weight of an atom (different element and isotopes)
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velocity (Ve)
energy an atom contains. (temp changes)
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Ke\= 1/2m*Ve^2
Mass decreases speed more velocity (increases by heat) making the atom go faster.
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Grahm's Law of Effusion
smaller things diffuse faster out of membranes.
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molar mass (MM)
grams / mol
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ideal gas deviations
an increase in deviation. Less volume(L) lowers pressure, bigger molecules (MM) higher pressure.
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ideal gas deviations
an increase in deviation. Low Temp, High IMF both decrease pressure
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molarity (M)
mol/L
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concentration
molarity is one way to calculate concentration (some \#/ L)
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Miscible
completely soluble
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Imiscible
not fully soluble (ratios)
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solvation
break solute-solute and solvent-solvent interactions forming solute-solvent interaction
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exo
release energy
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endo
take in energy
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chromatography
separates two liquids with different polarity with paper and a liquid being polar (polar paper, higher is less polar)(nonpolar, higher is polar)
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filtration
The separation of a liquid and a solid through a medium.
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distillation
separating a liquid and liquid through evaporating (the end liquid is the distillate)
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larger molecules
larger \= more polarizable, high IMF, higher Bp (c-c-c-c) smaller than (c-c-c-c-c)
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limits of models
Must assume some simplifications of complex issues. Some boundaries or limits identify. Not applicable to all situations.