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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 30 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. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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


3. Chalcogens - - Oxide O






4. 5 valence electrons -3 ions - Nitride N






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






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






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






8. 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






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






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






11. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






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






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






14. 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






15. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






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






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






18. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






19. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






20. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






21. 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.






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






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






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






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






26. 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






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






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






29. A base that can accept two moles of H+ per mole of itself (ex: SO4






30. 5 different orbitals shaped like clover leaves and max electrons is 10






31. Small discrete increments of energy.






32. Numbers that specify the properties of atomic orbitals and of their electrons






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






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






35. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






37. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total


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






39. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






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






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






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






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






45. PH of a molecule at which it contains no net electric charge - isoelectric point.






46. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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


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






49. The energy required to break a chemical bond and form neutral isolated atoms






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