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85 Cards in this Set
- Front
- Back
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Flame test: lithium, strontium
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Red
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Flame test: Calcium
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Orange
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Flame test: Sodium
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Yellow
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Flame test: Barium
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Green
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Flame test: Potassium
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Violet
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Device used to measure amount of gas evolved in a reaction
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Manometer
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How we determine how much heat is produced or absorbed by a reaction
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Calorimetry
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Formula to calculate amount of heat produced or absorbed by a reaction
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Q=mc deltaT
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Test to see if solution contains ions or not
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Conduction, check for electricity
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Solids are separated from liquids in a mixture and passed through a filter
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Filtration
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Differences in boiling points of liquids can be used to separate substances
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Distillation
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Substances are separated by differences in degree of affinities to which they are adsorbed onto the surface
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Chromatography
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Compounds that have the same chemical formula but different geometrical arrangement of atoms
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Isomers
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Hydrocarbon is made of...
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Hydrogen + Carbon
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Alkanes
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Hydrocarbones with single bonds
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Alkenes
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Hydrocarbons with at least one double bond
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Alkynes
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Hydrocarbons with at least one triple bond
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Aromatic hydrocarbons
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Six carbon rings with alternating double bonds; ex. benzene
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Functional group: alcohol
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-OH
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Functional group: amine
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-NH2
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Functional group: halide
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-F/Cl/Br/I
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Functional groups: carboxylic acids
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COOH
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Functional group: aldehydes and ketones
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C=O
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Functional group: ether
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C-O-C
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Functional group: ester
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COO
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Four major biomolecules
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Lipids, carbohydrates, proteins, nucleic acids
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Product of H+ and OH- concentrations at 25 C
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1x10^-14
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pH + pOH
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14
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Arrhenius acid produces...
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H+
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Arrhenius base produces...
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OH-
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To calculate pH of a strong acid, simply calculate...
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Molarity of the solution
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Solution of weak acid/base conjugate pair that resists change in pH when other acids or bases are added
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Buffer
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Equivalence point of a titration of a strong acid or base
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is always at pH 7
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Bronsted-Lowry acid
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Proton donor
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Bronsted-Lowry base
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Proton acceptor
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How quickly reactants are converted into products
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Rate of reaction
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Factors that affect rate of reaction
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Concentration of reactants in solution, surface area of solid reactants, temperature, type of reactants involved, presence of catalyst
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What is never consumed during a reaction?
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A catalyst
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The fact that reactants can be converted to products and vice versa
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Dynamic equilibrium
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The system is in equilibrium when...
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the rate of the forward reaction equals the rate of the reverse reaction
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Adding more reactants, or removing products, will...
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Shift the equilibrium to the right
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Adding products, or removing reactants, will...
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Shift the equilibrium to the left
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What has no effect on equilibrium?
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Catalysts
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A system at equilibrium causes the system to shift to relieve the stress
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Le Chatelier's principle
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What does a catalyst do?
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Lowers activation energy
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What is activation energy?
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Amount of energy each reactant molecules needs to be converted into a product
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Molality
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moles / kilograms
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Increasing the temperature causes _____ in solubility of solids
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increase
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Increasing temperature causes _______ in solubility of gases
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decrease
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More pressure, _____ solubility in water
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greater
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Formula for boiling point elevation and freezing point depression
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delta T = kmi (where k is a constant, m is molality)
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Boiling point elevation depends on....
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Number of solute particles and type of solvent, but not type of solute particles
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Ideal gas law
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PV=nRT (P=pressure, V=volume, n=moles of gas, R=gas constant, T=temp kelvin)
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Ideal gas assumptions
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1) Molecules of an ideal gas occupy zero volume, 2) Molecules of an ideal gas do not attract or repel each other
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Molecular shapes: 4, 0
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tetrahedral, ex. CCl4
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Molecular shapes: 4, 1
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trigonal pyramidal, ex. NH3
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Molecular shapes: 4, 2
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bent, ex. H2O
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Molecular shapes: 3, 0
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trigonal planar, ex. NO3-
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Molecular shapes: 3, 1
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bent, ex. SO2
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Molecular shapes: 2, 0
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linear, ex. CO2
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Diatomic molecules are polar or nonpolar?
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Nonpolar
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Bonds with great electronegative differences are...
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polar
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Unequal sharing of electrons to form a stable octet
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Polar covalent bond
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Bond formed between nonmetals with different electronegativities
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Polar covalent bond
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Bond formed between metals
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Metallic bond
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Bond formed between metal and nonmetal
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Ionic bond
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A device used to produce an electronic current from a spontaneous redox reaction
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Electrochemical cell (voltaic cell)
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Where reduction takes place in voltaic cell
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Cathode
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Where oxidation occurs in voltaic cell
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Anode
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A device that measures the voltage (electric potential) of the electrochemical cell
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Voltmeter
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Process by which electrical energy is put into a nonspontaneous redox reaction to force it to occur
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Electrolysis
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A useful way to separate ionic compounds into constituent elements
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Electrolysis
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Neutralizes excess charge buildup in voltaic cell
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Salt bridge
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Change in potential energy when a given element is reduced or oxidized
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Standard electrode potential E^0
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Alpha decay
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Alpha particle emitted, atomic number decreases by 2, mass number decreases by 4
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Beta decay
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Neutron --> proton, beta particle is emitted, atomic number increases by 1
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Positive beta decay (positron emission)
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Proton --> neutron, positron is emitted, atomic number decreases by 1
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Gamma decay
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Nucleus becomes more stable
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Incorrect idea that electrons orbit the nucleus like planets orbit the sun
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Bohr model
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Electrons have properties of particles and waves
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De Broglie hypothesis
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Ionization energy and electronegativity...
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Increase towards F on periodic table
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Atomic radius and metallic character...
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Increase towards Cs on periodic table
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Metallic character
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How easily an atom gives up an electron in a bond
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Ionization energy
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Energy requierd to move remove an electron from an atom
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Electronegative
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How much an atom "pulls" on electrons in a bond
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