Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Chem Final
FCA Chemistry Final
| Question | Answer |
|---|---|
| mr. misko put 54g of whiter into a beaker. how many moles of water did he place in the beaker? | 3.0 mol |
| a 2.000 mol sample of acetic acid has a mass of how many grams (acetic acid is CH3COOH) | 120g |
| the mole is a unit of | quantity |
| avogadro's number represents the number of _____ in a _____ | particles; mole |
| what is accuracy? | is a measure of how close a value is to the true value |
| what is precision? | is a measure of how close a series of value are to each other |
| which is a physical property? | mass, electrical conductivity, boiling point (NOT heat of combustion) |
| which is an intensive property? | density, melting point, malleability (NOT volume) |
| which is a pure substance? | diamonds, iron (III) sulfate, distilled water (NOT milk) |
| which is a type of mixture? | solution, suspension, colloid (NOT isotope) |
| how many protons, neutrons, & electrons does the isotope of carbon known as Carbon-14 have | 6-proton, 8-neutrons, 6-electrons |
| the atomic number of carbon is | 6 and equals the number of protons |
| 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 |
| who said: "by convention sweet, by convention bitter, by convention hot, by convention cold, by convention color: but in reality atoms and void" | democritus |
| who is credited for making the periodic table of the elements? | dmitri mendeleev |
| which group of the periodic table contains highly reactive elements that all form cations? | alkali metals |
| which group of the periodic table all form negative one anions? | halogens |
| which group of the periodic table contains elements that are fairly reactive and all form positive two cations? | alkaline earth metals |
| which group of the periodic table contains elements that are very stable and unreactive? | noble gases |
| what is the measure of the ability of an atom to attract electrons in a molecule | electronegativity |
| what is the most electronegative element? | fluorine |
| a bond that results from the electrostatic attraction between oppositely charged particles is | ionic bond |
| a bond that results from the sharing of valence electrons is | covalent bond |
| a bond that exists when electrons are delocalized and have an electrostatic attraction for the nuclei of different atoms called | a metallic bond |
| a pi bond is formed from the sharing of electrons between what types of orbitals? | p orbitals |
| according to VSEPR theory, what is the geometry of methane? | tetrahedral |
| according to VSEPR theory, what is the geometry of water? | bent |
| according to VSEPR theory, what is the geometry of carbon dioxide? | linear |
| what is an intermolecular force of attraction between 2 polar molecules | dipole-dipole |
| the intermolecular force that results from the synchronized movement of electrons in non-polar molecules | london dispersion forces |
| 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 |
| nitrogen dioxide has the formula: | NO2 |
| iron (III) sulfate has the formula: | Fe2(SO4)3 |
| what is KBr? | potassium bromide |
| ammonium nitrate has the formula: | NH4NO3 |
| hydroxide has a charge of | positive 1 |
| NaOH + CaCl2 -> NaCl + Ca(OH)2 is what type of reaction? | double displacement |
| C8H18 + O2 -> H2O + CO2 + heat is what type of reaction? | combustion |
| the ability of a substance to resist flowing | viscosity |
| the intermolecular force of attraction between particles of the same substance | cohesion |
| a solid whose particles are arranged in a random manner | an amorphous solid |
| graphite & diamond are examples of 2 | allotropes of an element |
| 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 |
| the process of a gas becoming a liquid is called | condensation |
| the process of a solid becoming a gas is called | sublimation |
| 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 |
| how much energy is required to completely melt a 36g sample of water that was initially at -25 degrees celsius? | 14KJ |
| 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 |
| 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 |
| a balloon with a volume of 1.5L at 298K is slowly heated to 400K. what is the new pressure | 2.0L |
| 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 |
| how many moles of gas are present in a 2.9L container at 1.0 atm and 298K? | .12mol |
| the component that is dissolved into a solvent in order to form a solution | solute |
| any substance that ionizes into cations and anions when dissolved | electrolyte |
| a substance that only partially ionizes when dissolved in a solution | weak electrolyte |
| liquids that are not soluble in one another/ not able to be mixed | immiscible |
| a solution that has reached the equilibrium where the rate of dissolution = the rate of recrystallization | saturated solution (supersaturated- saturated to the maximum) |
| a unit for concentration that expresses the number of moles of solute per leader of solution | molality |
| a unit for concentration that expresses the number of moles of solute per liter of solution | molarity |
| any substance that increases the concentration of hydrogen ions in aqueous solution | arrhenius acid |
| any substance that increases the concentration of hydroxide ions in aqueous solution | arrhenius base |
| proton donor | bronsted-lowry acid |
| proton acceptor | bronsted-lowry base |
| formed when bronzed lowry base accepts a proton | conjugate acid |
| remains after a bronzed-lowry acid donates a proton | conjugate base |
| a substance that can be either an acid or base | amphoteric |
| acid that can only date one proton | monoprotic acid |
| an acid that ionized when dissolved in solution | strong acid |
| 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 |
| the rule of polarity in solubility. only positives with positives and negatives with negatives | like dissolves like |
| unsaturated | less than saturated |
| are properties that depend on concentration of solute but not on the identity of the solute. explains why rock salt melts ice | colligative properties |
| sour taste, change color of acid & base indicatiors, react with bases to form salt & water and feel slippery | properties of acids |
| bitter taste, change color of acid/base indicators, react with bases to form salt & water, feel slippery | properties of bases |
| provides a surface that makes correct collisions between reactants easier | a catalyst |
| is a tool that is used in order to determine if a reaction will be spontaneous | gibbs free energy |
| 4 factors that influence reaction rates | surface area, concentration, temp, catalyst |
| the energy required or releases during the chemical reaction of substances in their standard state | standard molar enthalpy of reaction |
| a device used to measure the enthalpy of change fir a reaction | calorimeter |
| a measure of the energy that is not able to do work | entropy |
| the total amount of energy in a thermodynamic system | enthalpy |
| the energy level that must be overcome by the reactants in a chemical reaction in order for the reaction to occur | activation energy |
| 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 |
| one half the distance between the nuclei and the radius | atomic radii |
| the energy required to remove an electron | ionization energy |
| the ability of an element to attract the electrons of another element | electronegativity |
| electrons in the highest energy level (outermost) | valence electrons |
Created by:
bgpalmers
Popular Chemistry sets