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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. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






2. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






5. 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






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






7. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






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






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






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






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






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






14. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






16. 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-






17. A solid made up of particles that are not arranged in a regular pattern.






18. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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






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






21. Rare earth element group (elements 58-71)






22. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






24. 2.18 x 10^-18 J/electron






25. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






27. 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

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






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






31. 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.






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

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33. 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






34. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






35. 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.






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

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






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






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






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






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






42. 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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43. Chalcogens - - Oxide O






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






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






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






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






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






49. An ionic compound that resists changes in its pH






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