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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. 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.






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






3. The lowest allowable energy state of an atom






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






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






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






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






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






9. 2.18 x 10^-18 J/electron






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






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






13. PH of a molecule at which it contains no net electric charge - isoelectric point.






14. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






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






18. Named after their cation and anion






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






20. 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






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






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






23. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






24. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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25. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






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






28. 5 valence electrons -3 ions - Nitride N






29. 5 different orbitals shaped like clover leaves and max electrons is 10






30. 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.






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






32. Small discrete increments of energy.






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






34. 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.






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






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






37. 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.






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






39. Two or more atoms held together by covalent bonds






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






41. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






42. 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.






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






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






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






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






47. 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






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






49. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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