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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. E=hc/?






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






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






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






6. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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






8. Two or more atoms held together by covalent bonds






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






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






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






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






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






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






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






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






17. 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






18. Chalcogens - - Oxide O






19. A solid made up of particles that are not arranged in a regular pattern.






20. Slightly less reactive than alkali metals - comprise group II






21. 5 valence electrons -3 ions - Nitride N






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






23. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






26. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






27. Simplest whole # ration of atoms in a compound






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






29. The process by which one or more substances change to produce one or more different substances






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






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






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






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






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






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






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






38. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






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. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






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

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42. 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






43. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






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






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






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

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






48. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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






50. 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