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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.
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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. 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.






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






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






4. 2.18 x 10^-18 J/electron






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






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






7. 5 valence electrons -3 ions - Nitride N






8. A solution in which water is the solvent






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






10. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






11. 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.






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






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






14. 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






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






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






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






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






19. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






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






22. A subdivision of an energy level in an atom. They are divided into orbitals.






23. 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.






24. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






25. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






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






31. 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.






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






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






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






35. 5 different orbitals shaped like clover leaves and max electrons is 10






36. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






37. 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.






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






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






40. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






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






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






46. 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






47. Redox reaction - in which the same species is both oxidized and reduced.






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






49. E=hc/?






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