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






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






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






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






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






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






7. 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.






8. 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






9. 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






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






11. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






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






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






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






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






16. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






17. 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






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

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19. An ionic compound that resists changes in its pH






20. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






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






23. 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






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






25. Small discrete increments of energy.






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






27. The average distance between the nuclei of two bonded atoms






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






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






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






31. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






33. 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.






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






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






36. A reaction where a compound does Not change its molecular structure.






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






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






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






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






41. 5 valence electrons -3 ions - Nitride N






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






43. 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






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






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






46. 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.






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






48. 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






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






50. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






Can you answer 50 questions in 15 minutes?



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