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






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






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






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






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

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6. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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7. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






9. 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






10. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






11. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






13. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






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






16. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






17. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






19. 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.






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






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






22. 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-






23. 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






24. 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






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. 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






27. The lowest allowable energy state of an atom






28. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






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






32. 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.






33. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






35. The process of decomposing a chemical compound by the passage of an electric current.






36. 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.






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






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






39. 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






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






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






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






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






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






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






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






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






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






49. 2.18 x 10^-18 J/electron






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