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






2. 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






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






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






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






6. 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






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


8. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






9. 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






10. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






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






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






13. Chalcogens - - Oxide O






14. 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






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






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






17. 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.






18. 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






19. 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






20. 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






21. 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.






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






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






24. 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






25. A horizontal row of elements in the periodic table






26. 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.






27. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






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






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






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






36. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






37. The lowest allowable energy state of an atom






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






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






40. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






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






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






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






45. 2.18 x 10^-18 J/electron






46. 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






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






48. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






50. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight