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






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






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






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






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






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






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






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






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






10. 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






11. 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






12. An ionic compound that resists changes in its pH






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






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






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






16. 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






17. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






18. 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.






19. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






21. 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






22. 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






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






24. The process by which one or more substances change to produce one or more different substances






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






26. 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-






27. Named after their cation and anion






28. E=hc/?






29. 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






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






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






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






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






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






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






36. 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






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






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






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






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






42. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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






44. 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






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






46. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






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






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






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