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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. Simplest whole # ration of atoms in a compound






2. Property of the elements that can be predicted from the arrangement of the periodic table






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






4. 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






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






6. 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






7. 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-






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






9. E=hc/?






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






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






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






13. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






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






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






16. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






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






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






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






20. Numbers that specify the properties of atomic orbitals and of their electrons






21. 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.






22. 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.






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






25. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






26. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






27. 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






28. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






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






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






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






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






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






35. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






36. 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






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






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






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






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






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






42. An atom or group of atoms that has a positive or negative charge






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






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






45. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






46. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






47. Chalcogens - - Oxide O






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






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






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