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






2. 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






3. PH of a molecule at which it contains no net electric charge - isoelectric point.






4. 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






5. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






6. 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.






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






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






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






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






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






12. Two or more atoms held together by covalent bonds






13. Small discrete increments of energy.






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






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


16. 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






17. 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






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






19. 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.






20. 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






21. 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






22. 5 valence electrons -3 ions - Nitride N






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






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






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






26. Named after their cation and anion






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






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






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






30. Sum of the protons and neutrons in an element often denoted by the letter A






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






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






33. 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.






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






35. A subdivision of an energy level in an atom. They are divided into orbitals.






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






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






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






39. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






41. 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






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






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






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






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






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


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






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






50. The average distance between the nuclei of two bonded atoms