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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. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






2. 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.






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






4. An ionic compound that resists changes in its pH






5. 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.






6. 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






7. Small discrete increments of energy.






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






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






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






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


12. 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.






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






14. An elementary particle with 0 charge and mass about equal to a proton






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






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






17. 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






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






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






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






21. Simplest whole # ration of atoms in a compound






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






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






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






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






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






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






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






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






30. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






31. A reaction where a compound does Not change its molecular structure.






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






33. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






35. 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






36. 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






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






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


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






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






41. E=hc/?






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






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






44. The energy required to break a chemical bond and form neutral isolated atoms






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






46. 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






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






48. 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.






49. 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






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