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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. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






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






3. 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.






4. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






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






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






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






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






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






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






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






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






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






15. PH of a molecule at which it contains no net electric charge - isoelectric point.






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






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






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






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






20. A reaction where a compound does Not change its molecular structure.






21. Chalcogens - - Oxide O






22. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






23. 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






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






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






26. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






27. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






28. 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






29. 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.






30. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






32. 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






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






34. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






35. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






36. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






38. 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.






39. 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






40. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






43. 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.






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






45. A horizontal row of elements in the periodic table






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






47. 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






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






49. 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






50. Rare earth element group (elements 58-71)