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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. Two or more atoms held together by covalent bonds






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






3. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






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






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






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






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






9. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






10. The lowest allowable energy state of an atom






11. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






12. 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






13. (chemistry) p(otential of) H(ydrogen)






14. 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.






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






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






17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






18. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






19. 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






20. The slowest elementary step which is the limit for the rate of the other steps






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






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






23. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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24. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






25. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






26. A definite stable energy that a physical system can have






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






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






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






30. Substance in which a solute is dissolved to form a solution






31. 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






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






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






34. 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.






35. Any sample of a given compound will contain the same elements in the identical mass ratio.






36. Simplest whole # ration of atoms in a compound






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






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






39. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






40. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






41. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






43. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






44. 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






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






46. 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.






47. Small discrete increments of energy.






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






49. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






50. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu







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