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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. An atom or group of atoms that has a positive or negative charge






2. 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






3. 5 valence electrons -3 ions - Nitride N






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






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






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






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






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






9. Small discrete increments of energy.






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






11. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






12. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






13. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






15. 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






16. Chalcogens - - Oxide O






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






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






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






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






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






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






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






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

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






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






27. 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-






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






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






30. 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.






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






32. 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






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






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






35. 2.18 x 10^-18 J/electron






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






37. 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






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






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






40. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






42. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






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






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






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






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






48. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






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






50. E=hc/?