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






2. 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.






3. 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.






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






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






6. A definite stable energy that a physical system can have






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






8. 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






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






10. PH of a molecule at which it contains no net electric charge - isoelectric point.






11. Chalcogens - - Oxide O






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






13. 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






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






15. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






19. 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






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






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






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






23. 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.






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






25. A horizontal row of elements in the periodic table






26. 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






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






28. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






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






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






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






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






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






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






35. 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.






36. 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






37. 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






38. 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






39. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






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






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






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






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






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






46. 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.






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






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






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






50. The lowest allowable energy state of an atom