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






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






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






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

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


5. A horizontal row of elements in the periodic table






6. An ionic compound that resists changes in its pH






7. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






8. 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






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






10. 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-






11. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






13. 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






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. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






16. 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.






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






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






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






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






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






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






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






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






25. 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






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






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






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






29. Named after their cation and anion






30. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






31. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






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






33. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






36. 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






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






38. 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






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






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






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






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






43. Elements in the middle of the periodic table - in groups 3-12.






44. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






45. 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






46. Any sample of a given compound will contain the same elements in the identical mass ratio.






47. Small discrete increments of energy.






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






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






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