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






2. The lowest allowable energy state of an atom






3. 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.






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






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






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






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






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






9. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






10. 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.






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






12. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






13. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






14. 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






15. 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






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






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






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






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






20. 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-






21. 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






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






23. 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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24. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






25. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






29. Named after their cation and anion






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






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






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






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






34. A solution in which water is the solvent






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






36. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






37. 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






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






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






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






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






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






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

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44. A horizontal row of elements in the periodic table






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






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






47. Two or more atoms held together by covalent bonds






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






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






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







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