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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






2. 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.






3. 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






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






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






6. 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






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






8. 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.






9. Two or more atoms held together by covalent bonds






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






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






12. The lowest allowable energy state of an atom






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






14. 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-






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






16. Common definition of acids as proton (H+) donors and bases as proton acceptors






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






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






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






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






21. 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.






22. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






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






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






26. 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






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






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






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






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






31. 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






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






33. A horizontal row of elements in the periodic table






34. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






35. 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






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






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






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






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






40. 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






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






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






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






44. 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

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45. 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






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






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






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






49. The slowest elementary step which is the limit for the rate of the other steps






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