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247 Cards in this Set
- Front
- Back
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Celcius to kelvin
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C + 273
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proton
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Atomic #
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mass #
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protons + neutrons
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electrons
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= to proton #
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cation
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positive ion
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anion
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negative ion
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cathode
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negative electrode
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anode
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positive electrode
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isotope
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same element different mass #
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hydroxide
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oh-1
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cyanide
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cn-
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sulfate
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so4-2
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phosphate
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po4-3
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nitrate
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no3-1
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perchlorate
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clo4-
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chlorite
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clo2-
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carbonate
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co3-2
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bicarbonate
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hco3-
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peroxide
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o2-2
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permanganate
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kmno4-
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ammonium
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nh4+
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chlorate
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clo3-
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hypochlorite
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clo-
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-ite
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1 less oxygen
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-hypo
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2 less oxygen
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-per
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1 more oxygen
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-ous
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less cations
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-ic
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more cations
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electronic configuration
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n- shell electron is in (1s, 2s)
l- subshell electron is in (s, p) m1- orbital (1, 3, 5) ms- spin (+ or -) |
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max electrons in s shell
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2
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max electrons in p shell
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6
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max electrons in d shell
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10
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max electrons in f shell
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14
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valence electrons
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electrons in the outer most shell
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diamagnetic
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an element with 2 electrons in all of its occupied orbitals
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paramagnetic
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an element that has atleast one orbital with only one electron in it
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row
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period
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column
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family
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max # of electrons per row
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2n^2
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Halogens (Lightest to Heaviest)
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flourine, chlorine, bromine, iodine
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noble gases (Lightest to Heaviest)
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He, Ne, Ar, Kr, Xe, R
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ideal gas law
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pv=nrt
p-atm v-liters n-mol r-.0821 t-k |
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P&V
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directly proportional
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P or V and T
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inversely proportional
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torr/760=
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atm
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Avogadros Law
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v/n=v/n
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Daltons Law
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partial pressure
P=p1+p2+p3 |
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STP
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22.4 L, 273K, 1 atm, 1 mole
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Gas properties
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individual molecules widely dispersed
avg KE is direcly proportional to the absolute temperature It is elastic and therefore no momentum is lost Pressure of a gas is due to collisions Gas molecules do not attract eachother |
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intermolecular
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between molecules
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intramolecular
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within a molecule
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EN
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capacity of the atoms of an element to attact bonded electrons
non metals have greater En than metals Fl has greatest EN Cesium the least increases from left to right bottom to up |
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non-polar covalent
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less than .5
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polar covalent
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.5-1.9
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ionic bond
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greater than 1.9
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dipole moment
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molecule is polar
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symmetric
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non polar
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non symmetric
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polar
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dipole moment of zero
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non polar
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london forces
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neutral nonpolar molecules attract eachother. weakest intermolecular attraction
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hydrogen bonding
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very stron dipole dipole.
H is bonded to F, O or N |
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Diatomics
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AX polar
X2 non polar |
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Bent
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2 bonds and an lp
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linear
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2 bonds
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trigonal planar
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3 bonds
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pyramidal
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3 bonds and an lp
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tetrahedral
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4 bonds
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octahedral
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6 bonds
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ionic compounds
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metal/non metal
polyatomic strongest intermolecular force |
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strength of intermolecular force
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ion-ion>H-Bonding>Dipole-Dipole>London Forces
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The stronger the intermolecular attraction, the ______
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higher the MP and BP will be
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For polar molecules, the smaller the molecule
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the stronger the attraction
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For non-polar molecules, the larger the molecule
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the stronger the attraction
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To determine bond polarity, mp and bp use:
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type of bond or weight. the higher the weight the greater the bp, the stronger the bond the greater the bp
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empirical formula
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simplest whole number ratio
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molecular formula
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actual # of atoms
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percent composition
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n*gE*(100/gF)=%E
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percent composition to empirical formula
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(%/100)/gE=amount of moles
if it is not a whole # divide by smallest # of moles |
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denisty
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m/v
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specific gravity
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(d of x)/(d of water)
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homogenous
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completely uniform
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solute
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the one being dissolved
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solvent
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the one doing the dissolving
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concentration
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quantity of solute/ quantity of solvern or solution as a whole
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Molarity (M)
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moles of solute/ L of solution
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# of moles
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M*L
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% by mass
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(mass of solute*100)/mass of solution
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% by mass/volume
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(mass of solute*100)/volume of solution in mL
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Molality (m)
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moles of solute/ mass of solvent in kg
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Mole fraction =1
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moles of i/ total moles
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Raolt's Law
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mole fraction/ vapor pressure
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BP elevation
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kb*m
kb (constant) m (molality of solute) |
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FP Depression
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kf*m
kf (constant) m (molality of solute) |
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osmosis
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flow of solvent to equalize concentrations
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dialysis
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the flow of solute through a membrane
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osmotic pressure
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pressure exerted to stop flow of osmosis
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the greatest colligative effect would be
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the lowest vp, highest bp, lowest fp, or largest osmotic pressure
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strong electrolyte solutes
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water soluble strong acids (HCl, HNO3, H2SO4)
water soluble strong bases (NaOH, KOH) water soluble salts (NaCL, KNO3, K2SO4) |
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weak electrolyte solutes
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water soluble weak acid (CH3COOH)
water soluble weak base (NH3) |
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non-electrolyte solutes
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water soluble sugars (glucose, sucrose)
water soluble alcohols (CH3OH, C2H5OH) |
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Dilution
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Mi * Vi=Mf * Vf
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limiting reactant
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calculate the qty of product separately for each reactant. Then choose the least amount of product calculated as the correct choice.
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Acid properties
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taste sour
turns litmus red yield pH less than 7 completely ionize |
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base properties
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taste bitter and have a slippery feel
turn litmus blue yield pH greater than 7 |
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Arrhenius definition
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acid generates H+
base yields OH- |
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Bronsted-Lowry Definition
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acid is a (H+) proton donor
base is a proton acceptor |
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Lewis Definition
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acid is an electron pair acceptor
base is an electron pair donor |
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strong acids react ____
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completely
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weak acids react ______
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incompletely
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a strong electrolyte is _______ ionized
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completely
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a weak electrolyte is ________
ionized |
partially
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strong acids
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hcl, hno3, h2so4,
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weak acid
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ch3cooh, hf, h2co3, h3po4
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strong base
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IA and IIA hydroxides
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weak base
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ammonia
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pH=
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-log[H]
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pOH
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-log[OH]
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calculating pH or pOh with out calculator
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take molarity and count the number of times u need to move the decimal to make it 1.
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calculating molarity from ph or pOH without calculator
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1x10-(ph or pOH)
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kw
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[h3o][oh]= 1 x 10 -14
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pH + pOH=
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14
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buffer
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weak acid and weak base
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acid/base stoichiometric
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Nb * Mb *Vb = Na * Mb * Vb
n= # of h donated/accepted |
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oxidation # of IA
(Li, Na, K,Rb, Cs) |
+1
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oxidation # of F
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-1
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oxidation # of IIA
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+2
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Group II A elements
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(Be, Mg, Ca,Sr, Ba)
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Group IA elements
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(Li, Na, K,Rb, Cs)
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oxidation # of Al
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+3
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oxidation # of H
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+1 with non metal
-1 with metal |
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oxidation # of O
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-2
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oxidation # of cl, br, I
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-1
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oxidation # for an unknown element
ex. cr2o7-2 find On for CR |
2(x)+7(-2)=-2
x=+6 |
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reduction reaction
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decrease cation
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OXIDATION REACTION
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increase cation
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reducing agent
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the one that is being increased
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oxidizing agent
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the one that is being decreased
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redox reaction
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create half reaction
balance oxidation by adding e- |
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specific heat
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q=m*sh*delta t
q= heat |
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heat of fusion
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m*q
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heat of vaporation
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m*q
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entropy
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disorder
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spontaneous reaction
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incr in disorder
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1st law of thermodynamics
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conservation- mass n energy is conserved
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2nd law of thermodynamics
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disorder- spontaneous incr disorder
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3rd law of thermodynamics
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pure solid at absolute 0 has 0 disorder
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disorder increase
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positive s
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disorder decrease
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negative s
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delta s
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s prod- s reactants
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enthalpy, h
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heat change
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h is negative
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exothermic
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h is positive
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endothermic
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gibbs free energy, g
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=h-ts
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g is negative
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reaction spontaneous
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g is positive
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reaction non spontaneous
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g is 0
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equilibrium
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overall order
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x+y+z
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rate
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k[a]^x[b] ^y[c]^z
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the larger the value of k_______
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the faster the reaction
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g=
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Ea(for)-Ea(rev)
or e of prod - e of reac |
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Ea (for)=
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TS-react
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Ea(rev)=
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TS-prod
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transition state
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short lived max energy
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activation energy
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the larger the value of Ea the slower the reaction will be
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spontaneous reactions
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products above reactants
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non spontaneous reactions
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reactants above products
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equilibrium reactions
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reactants = products
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catalyst
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lowers TS
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equilibrium constant, k
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prod/react
(only for gases) |
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pure solids, pure liquids and water ________
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are not included in the equilibrium expression
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changes in concentration
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add reactant - shift to right
remove reactant- shift to left add product- shift to left remove product- shift to right |
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changes in pressure
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decrease in pressure- increase in volume more moles
increase in pressure- decrease in volume less moles |
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changes in temp
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endothermic- remove product
exothermic- add product |
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tetrahedral angle
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109*
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trigonal planar angle
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120*
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linear angle
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180*
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saturated
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single bond
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unsaturated
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multiple bond
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saturated hydrocarbons
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alkane
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unsaturated hydrocarbons
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alkene or alkyne
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methane
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ch4
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ethane
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ch3-ch3
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propane
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ch3-ch2-ch3
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butane
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ch3-ch2-ch2-ch3
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pentane
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c5h12
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hexane
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c6h14
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heptane
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c7h16
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octane
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c8h18
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nonane
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c9h20
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decane
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c10h22
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methyl
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-ch3
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ethyl
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-ch2-ch3
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propyl
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-ch2-ch2-ch3
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isopropyl
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-ch-(ch3)2
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naming
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identify the longest carbon chain
give the smallest number list in abc order |
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naming alcohols
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state number of OH group and end in -ol
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naming esters
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2 word name.. first from alcohol
2nd from acid end in -ate |
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aldehyde
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r-c-h
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ketone
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r-c-r
|| o |
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naming aldehyde
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end in -al
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naming ketone
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end in -one
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carboxylic acid
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r-c-oh
|| o |
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naming carboxylic acid
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end in -ic acid
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ester
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r-c-or
|| o |
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ether
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r-o-r
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naming ether
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add ether as 2nd word
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naming amine
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add amine as 2nd word
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amine
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r-nh2
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ammino acids
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nh2-c-c-oh
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isomers
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same molecular formula but possess some structural difference
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geometric isomers
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cis and trans
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optical isomers
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non superimposable mirror images
have four different groups bonded 2 carbon |
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aromatic compounds
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conjugated ring system
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huckels law
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4N+2=# of bonds
n should be 0, 1, 2, 3, 4 |
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formation of an ester
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reaction of cooh and an alcohol
with h+ |
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markonikovs rule
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adds h to alkene with more h and x to c with less h
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anti-markonikovs rule,
h2o2/hbr |
adds h to alkene with less h and x to c with more h
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1* carbon
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alcohol, aldehyde or cooh attached to c thats attached to 1 r
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2* carbon
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alcohol or ketone attached to c thats attached to 2 r's
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1* carbon oxidation sequence
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ethane>alcohol>aldehyde>COOH
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2* carbon oxidation sequence
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propane>alcohol>ketone
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oxidizing agents
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h2cro4, kmno4, na2cr2o7/h2so4
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reducing agent
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lialh4
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stability of a carbocation
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3>2>1
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sn1
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3>2>1
carbocation |
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sn2
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1>2>3
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acid catalyzed dehydration for alcohols
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yields 2 products
major- loss of h on right minor- loss of h on left |
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hydration reactions
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alkene + h2o -> alcohol
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two amino acids form _____
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a peptide bond
(-h20) |
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anhydride
|
removal of h2o
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triple pt
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where all states coexist
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sublimation
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solid to gas
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deposition
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gas to solid
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last point on line in phase diagram
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critical point
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phase diagram
|
left to right solid to liquid and on bottom gas
between solid and liquid m/f pt between liquid and gas bp |
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ksp=
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[m^n+][x^n-]
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the smaller the value of ksp
|
the less soluble the salt will be
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solubility
|
sqrt of ksp
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oxidation occurs at the
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anode
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reduction occurs at the
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cathode
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optically active
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a molecule that has a non superimposable mirror image
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chiral
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carbon bonded 2 four different groups
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addition of br2
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adds 2 br's
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br2/ccl4
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colorless
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sp3 hybridized
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4 single bonds
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sp2 hybridized
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1 double 3 singles
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sp hybridized
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linear
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