Test your basic knowledge |

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 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






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






3. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






4. 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






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






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






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






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






9. 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.






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






11. Simplest whole # ration of atoms in a compound






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






13. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






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






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






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






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






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






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






22. 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.






23. 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.






24. 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.






25. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






26. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






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






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






29. 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






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






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






32. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






34. E=hc/?






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






36. Slightly less reactive than alkali metals - comprise group II






37. 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






38. 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






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


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






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






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






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






44. A horizontal row of elements in the periodic table






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






46. Common definition of acids as proton (H+) donors and bases as proton acceptors






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






48. 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






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






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