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






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






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






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






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






6. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






8. 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.






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






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






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






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






13. 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






14. 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






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






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






17. 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






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






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






20. The lowest allowable energy state of an atom






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






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






23. Small discrete increments of energy.






24. 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.






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






26. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






27. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






29. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






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






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






33. 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






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






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






36. Numbers that specify the properties of atomic orbitals and of their electrons






37. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






38. 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






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






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






41. In a solution - the substance that dissolves in the solvent






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






43. 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






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






45. 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






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






47. Gram equivalent weight of solute per liter of solution - often denoted by N.






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






49. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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