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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • 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. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






3. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






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






6. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






7. 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.






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






9. 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






10. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






12. 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.






13. 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-






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






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






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






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






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






19. 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






20. A solution in which water is the solvent






21. 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






22. 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






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






24. 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






25. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






26. (chemistry) p(otential of) H(ydrogen)






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






28. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






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






30. 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






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






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






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






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






35. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






36. 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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37. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






38. 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






39. 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






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






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






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






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






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






46. An ionic compound that resists changes in its pH






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






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






49. 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.






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