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






2. Simplest whole # ration of atoms in a compound






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






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






5. 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.






6. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






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






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






11. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






15. 2.18 x 10^-18 J/electron






16. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






17. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






18. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






19. 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






20. 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.






21. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






22. 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






23. 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






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






25. 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






26. 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






27. 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






28. Named after their cation and anion






29. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






30. 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.






31. 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






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






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






34. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






35. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






36. 5 valence electrons -3 ions - Nitride N






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






38. 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






39. Two or more atoms held together by covalent bonds






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






41. 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






42. The lowest allowable energy state of an atom






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






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






45. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






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






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






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






50. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers







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