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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • 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 chemical bond that involves sharing a pair of electrons between atoms in a molecule






2. 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






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






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






6. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






8. The lowest allowable energy state of an atom






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






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






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






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






13. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






14. A subdivision of an energy level in an atom. They are divided into orbitals.






15. 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






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






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






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






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






20. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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21. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






22. Simplest whole # ration of atoms in a compound






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






24. A dynamic condition in which two opposing changes occur at equal rates in a closed system






25. 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






26. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






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






29. 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






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






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






32. 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






33. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






34. 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






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






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






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






38. 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.






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






40. 5 valence electrons -3 ions - Nitride N






41. 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






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

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43. 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






44. 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






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






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






47. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






48. 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






49. 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.






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







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