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






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






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






4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






6. The lowest allowable energy state of an atom






7. 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.






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






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






10. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






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






13. 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






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






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






16. The energy required to break a chemical bond and form neutral isolated atoms






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






18. Numbers that specify the properties of atomic orbitals and of their electrons






19. 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






20. Small discrete increments of energy.






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






22. 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






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






24. Named after their cation and anion






25. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






26. A reaction where a compound does Not change its molecular structure.






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






28. 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






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






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






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






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






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






35. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






36. 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






37. E=hc/?






38. 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






39. 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






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






41. The maximum amount of product that can be produced from a given amount of reactant






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






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






44. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






45. 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.






46. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






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






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






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