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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 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






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






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






4. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






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






7. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






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






10. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






11. 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






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






13. 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






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


15. The average distance between the nuclei of two bonded atoms






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






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






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






19. 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.






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






21. 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






22. 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






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






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






25. 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.






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






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






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






29. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






30. 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






31. The Percent by mass of each element in a compound.






32. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T


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






34. Substance in which a solute is dissolved to form a solution






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






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






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






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






39. A solid made up of particles that are not arranged in a regular pattern.






40. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






41. 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.






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






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






44. 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-






45. Property of the elements that can be predicted from the arrangement of the periodic table






46. 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.






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






48. 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






49. A definite stable energy that a physical system can have






50. 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