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. Substance in which a solute is dissolved to form a solution






2. 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






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






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






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






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






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






8. 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.






9. 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






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






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






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






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






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






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






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






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






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






22. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






24. 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






25. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






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






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


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






30. 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






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






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


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






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






36. 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.






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






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






39. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






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






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






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






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


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






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






46. 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






47. 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






48. The area of chemistry that is concerned with reaction rates and reaction mechanisms






49. A solution in which water is the solvent






50. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.