Test your basic knowledge |

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






2. 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-






3. 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.






4. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






6. Tells you how much solute is present compared to the amount of solvent






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






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






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






10. 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






11. An ionic compound that resists changes in its pH






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






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






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






15. 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.






16. Two or more atoms held together by covalent bonds






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






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






19. 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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


23. 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






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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






26. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






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






28. Named after their cation and anion






29. 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.






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






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. Slightly less reactive than alkali metals - comprise group II






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






34. 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






35. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






36. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






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






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






40. 5 different orbitals shaped like clover leaves and max electrons is 10






41. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






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






44. 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






45. E=hc/?






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






47. Property of the elements that can be predicted from the arrangement of the periodic table






48. 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






49. A substance that - when dissolved in water - results in a solution that can conduct electricity






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