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






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






3. An ionic compound that resists changes in its pH






4. 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






5. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






7. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






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 percent by mass of each element in a compound






11. 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.






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






13. E=hc/?






14. 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






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






16. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






18. 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






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






20. 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






21. Two or more atoms held together by covalent bonds






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






23. 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






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






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






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






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






28. 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






29. 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






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






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






32. 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.






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






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






35. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






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






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






39. The lowest allowable energy state of an atom






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






41. 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.






42. 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






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






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






45. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






48. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






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