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






2. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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






6. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






7. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






9. 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






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






11. Elements in the middle of the periodic table - in groups 3-12.






12. Common definition of acids as proton (H+) donors and bases as proton acceptors






13. 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






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






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






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






17. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






18. 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






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






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






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






22. 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






23. 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






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






25. Gram equivalent weight of solute per liter of solution - often denoted by N.






26. E=hc/?






27. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






28. 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






29. 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






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






31. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






34. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






35. 5 different orbitals shaped like clover leaves and max electrons is 10






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






37. Simplest whole # ration of atoms in a compound






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






39. In a solution - the substance that dissolves in the solvent






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






41. A solution in which water is the solvent






42. 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.






43. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






44. 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






45. 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-






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






47. 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






48. 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.






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






50. 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