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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






2. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






3. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






4. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






5. Tells you how much solute is present compared to the amount of solvent






6. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






7. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






8. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






9. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






10. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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11. A substance that - when dissolved in water - results in a solution that can conduct electricity






12. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






13. 5 valence electrons -3 ions - Nitride N






14. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






15. Acids defined as electron - pair acceptors and bases as electron - pair donors.






16. The Percent by mass of each element in a compound.






17. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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18. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






19. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






20. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






21. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






23. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






24. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






25. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






26. The process of decomposing a chemical compound by the passage of an electric current.






27. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






28. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






29. The process by which one or more substances change to produce one or more different substances






30. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






31. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






32. The percent by mass of each element in a compound






33. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






34. A solution in which water is the solvent






35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






36. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






37. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






38. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






39. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






40. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






42. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






43. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






44. An ionic compound that resists changes in its pH






45. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






46. The average distance between the nuclei of two bonded atoms






47. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






48. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






49. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






50. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.







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