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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. 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

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






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






4. 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






5. 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.






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






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






8. 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.






9. 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






10. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






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






12. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






13. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






14. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






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






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






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






21. 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






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






23. Gram equivalent weight of solute per liter of solution - often denoted by N.






24. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






26. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






27. 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






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






29. Chalcogens - - Oxide O






30. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






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






32. Two or more atoms held together by covalent bonds






33. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






35. 2.18 x 10^-18 J/electron






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






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. 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-






39. 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.






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






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






42. Tells you how much solute is present compared to the amount of solvent






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






44. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






45. Small discrete increments of energy.






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






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






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






49. 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






50. 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