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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. An elementary particle with 0 charge and mass about equal to a proton






2. Small discrete increments of energy.






3. 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






4. Named after their cation and anion






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






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






7. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






9. 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






10. A horizontal row of elements in the periodic table






11. 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






12. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






14. 2.18 x 10^-18 J/electron






15. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






17. 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






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






19. Sum of the protons and neutrons in an element often denoted by the letter A






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






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






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






24. 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






25. 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.






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






27. 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






28. 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






29. 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






30. 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






31. 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






32. Simplest whole # ration of atoms in a compound






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






34. 5 valence electrons -3 ions - Nitride N






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






36. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






38. 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






39. 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.






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






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






42. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






43. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






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






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






46. 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






47. 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.






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






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






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