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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. 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.






2. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






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






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






10. 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






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






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






13. Two or more atoms held together by covalent bonds






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






15. 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






16. 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






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






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






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






20. 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






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






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






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






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






25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






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






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






30. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






31. 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.






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






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






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






36. 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






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






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






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






40. 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-






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






42. Simplest whole # ration of atoms in a compound






43. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






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






47. 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






48. Chalcogens - - Oxide O






49. The lowest allowable energy state of an atom






50. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water