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






2. 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






3. Simplest whole # ration of atoms in a compound






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






5. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






6. 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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7. (chemistry) p(otential of) H(ydrogen)






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






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






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






11. 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.






12. 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






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






14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






15. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






16. 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.






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






18. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






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






21. 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






22. 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.






23. 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.






24. Small discrete increments of energy.






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






26. A solid made up of particles that are not arranged in a regular pattern.






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






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






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






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






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






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






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






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






36. Named after their cation and anion






37. 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.






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






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






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






41. 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






42. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






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






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






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






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






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






49. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






50. The maximum amount of product that can be produced from a given amount of reactant