FCA Chemistry Final
Quiz yourself by thinking what should be in
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on it to display the answer.
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| mr. misko put 54g of whiter into a beaker. how many moles of water did he place in the beaker? | 3.0 mol
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| a 2.000 mol sample of acetic acid has a mass of how many grams (acetic acid is CH3COOH) | 120g
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| the mole is a unit of | quantity
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| avogadro's number represents the number of _____ in a _____ | particles; mole
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| what is accuracy? | is a measure of how close a value is to the true value
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| what is precision? | is a measure of how close a series of value are to each other
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| which is a physical property? | mass, electrical conductivity, boiling point (NOT heat of combustion)
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| which is an intensive property? | density, melting point, malleability (NOT volume)
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| which is a pure substance? | diamonds, iron (III) sulfate, distilled water (NOT milk)
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| which is a type of mixture? | solution, suspension, colloid (NOT isotope)
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| how many protons, neutrons, & electrons does the isotope of carbon known as Carbon-14 have | 6-proton, 8-neutrons, 6-electrons
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| the atomic number of carbon is | 6 and equals the number of protons
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| the scientist antoine lavoisier is known as the father of modern chemistry. one of his major accomplishments was to ________ | write a book on chemical nomenclature
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| who said: "by convention sweet, by convention bitter, by convention hot, by convention cold, by convention color: but in reality atoms and void" | democritus
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| who is credited for making the periodic table of the elements? | dmitri mendeleev
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| which group of the periodic table contains highly reactive elements that all form cations? | alkali metals
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| which group of the periodic table all form negative one anions? | halogens
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| which group of the periodic table contains elements that are fairly reactive and all form positive two cations? | alkaline earth metals
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| which group of the periodic table contains elements that are very stable and unreactive? | noble gases
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| what is the measure of the ability of an atom to attract electrons in a molecule | electronegativity
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| what is the most electronegative element? | fluorine
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| a bond that results from the electrostatic attraction between oppositely charged particles is | ionic bond
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| a bond that results from the sharing of valence electrons is | covalent bond
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| a bond that exists when electrons are delocalized and have an electrostatic attraction for the nuclei of different atoms called | a metallic bond
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| a pi bond is formed from the sharing of electrons between what types of orbitals? | p orbitals
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| according to VSEPR theory, what is the geometry of methane? | tetrahedral
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| according to VSEPR theory, what is the geometry of water? | bent
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| according to VSEPR theory, what is the geometry of carbon dioxide? | linear
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| what is an intermolecular force of attraction between 2 polar molecules | dipole-dipole
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| the intermolecular force that results from the synchronized movement of electrons in non-polar molecules | london dispersion forces
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| the intermolecular forces that exist between ethanol molecules are somewhat weaker than those that exist between water molecules, consequently: | water has a higher boiling point because it is harder for molecules to leave the liquid phase
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| nitrogen dioxide has the formula: | NO2
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| iron (III) sulfate has the formula: | Fe2(SO4)3
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| what is KBr? | potassium bromide
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| ammonium nitrate has the formula: | NH4NO3
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| hydroxide has a charge of | positive 1
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| NaOH + CaCl2 -> NaCl + Ca(OH)2 is what type of reaction? | double displacement
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| C8H18 + O2 -> H2O + CO2 + heat is what type of reaction? | combustion
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| the ability of a substance to resist flowing | viscosity
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| the intermolecular force of attraction between particles of the same substance | cohesion
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| a solid whose particles are arranged in a random manner | an amorphous solid
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| graphite & diamond are examples of 2 | allotropes of an element
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| all matter is made up of tiny particles called atoms, ions, or molecules, particle motion -- particle motion is least in solids, greater in liquids, and greatest in gases -- particles in motion possess kinetic energy, which is greatest in gases --these r? | tenants of the kinetic molecular theory
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| the process of a gas becoming a liquid is called | condensation
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| the process of a solid becoming a gas is called | sublimation
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| how much energy is required to completely melt a 36g sample of ice (solid water) that has just previously warmed up to 0.00 degrees celsius | 12KJ
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| how much energy is required to completely melt a 36g sample of water that was initially at -25 degrees celsius? | 14KJ
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| how much energy is required to heat a 36.0g sample of solid water from -25.0 degrees celsius to 50.0 degrees celsius? | 21.4KJ
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| a plastic water bottle with an initial volume of .50L and a pressure of 1.0atm is crushed to .20L. what is the new pressure | 2.5atm
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| a balloon with a volume of 1.5L at 298K is slowly heated to 400K. what is the new pressure | 2.0L
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| A gas takes up a volume of 20.0L, has a pressure of 1.00atm, and a temperature of 298K. if the temperature was increases to 352K and the pressure was dropped to .500atm, what is the new volume? | 47.2L
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| how many moles of gas are present in a 2.9L container at 1.0 atm and 298K? | .12mol
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| the component that is dissolved into a solvent in order to form a solution | solute
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| any substance that ionizes into cations and anions when dissolved | electrolyte
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| a substance that only partially ionizes when dissolved in a solution | weak electrolyte
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| liquids that are not soluble in one another/ not able to be mixed | immiscible
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| a solution that has reached the equilibrium where the rate of dissolution = the rate of recrystallization | saturated solution (supersaturated- saturated to the maximum)
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| a unit for concentration that expresses the number of moles of solute per leader of solution | molality
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| a unit for concentration that expresses the number of moles of solute per liter of solution | molarity
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| any substance that increases the concentration of hydrogen ions in aqueous solution | arrhenius acid
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| any substance that increases the concentration of hydroxide ions in aqueous solution | arrhenius base
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| proton donor | bronsted-lowry acid
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| proton acceptor | bronsted-lowry base
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| formed when bronzed lowry base accepts a proton | conjugate acid
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| remains after a bronzed-lowry acid donates a proton | conjugate base
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| a substance that can be either an acid or base | amphoteric
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| acid that can only date one proton | monoprotic acid
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| an acid that ionized when dissolved in solution | strong acid
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| the point in a titration where the number of moles of the substance being titrated equals the number of moles of acid/base added | equivalence point
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| the rule of polarity in solubility. only positives with positives and negatives with negatives | like dissolves like
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| unsaturated | less than saturated
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| are properties that depend on concentration of solute but not on the identity of the solute. explains why rock salt melts ice | colligative properties
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| sour taste, change color of acid & base indicatiors, react with bases to form salt & water and feel slippery | properties of acids
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| bitter taste, change color of acid/base indicators, react with bases to form salt & water, feel slippery | properties of bases
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| provides a surface that makes correct collisions between reactants easier | a catalyst
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| is a tool that is used in order to determine if a reaction will be spontaneous | gibbs free energy
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| 4 factors that influence reaction rates | surface area, concentration, temp, catalyst
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| the energy required or releases during the chemical reaction of substances in their standard state | standard molar enthalpy of reaction
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| a device used to measure the enthalpy of change fir a reaction | calorimeter
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| a measure of the energy that is not able to do work | entropy
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| the total amount of energy in a thermodynamic system | enthalpy
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| the energy level that must be overcome by the reactants in a chemical reaction in order for the reaction to occur | activation energy
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| a reaction in which the reactants are converted to products without the constant addition of energy from outside the thermodynamic system to sustain the reaction | spontaneous reaction
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| one half the distance between the nuclei and the radius | atomic radii
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| the energy required to remove an electron | ionization energy
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| the ability of an element to attract the electrons of another element | electronegativity
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| electrons in the highest energy level (outermost) | valence electrons
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