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






2. 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.






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






4. 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






5. 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






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






7. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






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






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






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






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






13. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






14. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






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






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






18. 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.






19. 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






20. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T


21. 2.18 x 10^-18 J/electron






22. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






23. 5 different orbitals shaped like clover leaves and max electrons is 10






24. 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


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






26. 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-






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






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






29. 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






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






31. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


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






33. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






34. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






35. An ionic compound that resists changes in its pH






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






37. 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


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






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






40. Temperature is constant; effusion and temperature are proportional to the square root of their masses


41. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






43. 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.






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






45. 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






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






47. E=hc/?






48. Two or more atoms held together by covalent bonds






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






50. The pressure exerted by a vapor in equilibrium with its liquid or solid phase