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






2. 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






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






4. 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.






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






6. 5 different orbitals shaped like clover leaves and max electrons is 10






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






8. 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-






9. 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






10. 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.






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






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






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






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






15. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






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






18. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






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






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






22. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






23. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






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






25. Acids defined as electron - pair acceptors and bases as electron - pair donors.






26. Chalcogens - - Oxide O






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

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28. Named after their cation and anion






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






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






31. 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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32. 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






33. 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






34. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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






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






37. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






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






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






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






42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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

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44. 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.






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






46. 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.






47. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






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






49. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






50. The lowest allowable energy state of an atom