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






2. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






3. 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






4. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






5. A reaction in which atoms of one element take the place of atoms of another element in a compound






6. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


7. Slightly less reactive than alkali metals - comprise group II






8. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






10. 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






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






12. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






13. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






15. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






16. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






17. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






19. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






21. Having characteristics of both an acid and a base and capable of reacting as either






22. 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






23. An atom or group of atoms that has a positive or negative charge






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






25. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






27. Chalcogens - - Oxide O






28. 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.






29. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






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






32. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






33. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






34. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






35. Property of the elements that can be predicted from the arrangement of the periodic table






36. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






37. An elementary particle with 0 charge and mass about equal to a proton






38. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






39. 2.18 x 10^-18 J/electron






40. Redox reaction - in which the same species is both oxidized and reduced.






41. E=hc/?






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






43. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






44. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






45. The maximum amount of product that can be produced from a given amount of reactant






46. 5 valence electrons -3 ions - Nitride N






47. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






48. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






49. 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






50. (chemistry) a substance that changes color to indicate the presence of some ion or substance