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






2. The lowest allowable energy state of an atom






3. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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






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






6. 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






7. Named after their cation and anion






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






9. The percent by mass of each element in a compound






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






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






12. 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






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






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






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






16. 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.






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






18. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






19. 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






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






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






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






23. 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






24. 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


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






26. 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






27. 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.






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


30. Small discrete increments of energy.






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






32. 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.






33. The slowest elementary step which is the limit for the rate of the other steps






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






35. An atom or group of atoms that has a positive or negative charge






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






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






38. Two or more atoms held together by covalent bonds






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






40. 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






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






42. 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.






43. 2.18 x 10^-18 J/electron






44. 5 valence electrons -3 ions - Nitride N






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






47. 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.






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






49. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin


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