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






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






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






4. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






5. 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






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






7. Simplest whole # ration of atoms in a compound






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






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






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






11. 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






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






13. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






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






15. 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






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






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






18. An ionic compound that resists changes in its pH






19. 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






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






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






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






23. 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






24. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






26. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






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






29. 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






30. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






31. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






32. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






34. Chalcogens - - Oxide O






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






36. The lowest allowable energy state of an atom






37. 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.






38. A solution in which water is the solvent






39. Small discrete increments of energy.






40. 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






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






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






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






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






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






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






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






48. E=hc/?






49. 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.






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