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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 30 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. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






2. 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-






3. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total


4. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






5. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






6. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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


8. 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






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






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






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






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






13. 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.






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






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






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






17. A horizontal row of elements in the periodic table






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






19. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






20. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






21. 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.






22. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






25. Small discrete increments of energy.






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






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






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






29. E=hc/?






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






31. 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






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






33. 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.






34. 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






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






36. 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






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


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






39. 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.






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






41. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






42. 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






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






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






45. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






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






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






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






50. Chalcogens - - Oxide O