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






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






3. 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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4. 2.18 x 10^-18 J/electron






5. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






7. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






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

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






11. The process of decomposing a chemical compound by the passage of an electric current.






12. 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






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






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






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






16. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






17. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






22. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






25. 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






26. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






28. 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.






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






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






31. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






32. 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






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






34. 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






35. 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






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






37. 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.






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






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. 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.






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






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






43. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






44. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






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






47. 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.






48. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






50. 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