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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 Percent by mass of each element in a compound.






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






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






4. A definite stable energy that a physical system can have






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






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






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






8. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






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






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






11. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






14. 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.






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






16. 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


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






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






19. 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






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


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






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


23. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






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






26. 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






27. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






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






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






31. 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






32. 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.






33. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






34. 2.18 x 10^-18 J/electron






35. E=hc/?






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






38. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






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






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






42. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






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






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






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






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






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


49. 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






50. 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.