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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.
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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. 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






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






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






4. 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.






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






6. 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.






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






8. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






9. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






10. 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






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






12. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






13. 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






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






15. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






16. 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






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






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






19. 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






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






21. The lowest allowable energy state of an atom






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






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






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






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






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






27. 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.






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






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






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






31. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






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






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






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






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






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






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






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






40. 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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41. E=hc/?






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






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






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






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






46. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






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






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






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