Test your basic knowledge |

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 substance that - when dissolved in water - results in a solution that can conduct electricity






2. 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






3. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


4. Simplest whole # ration of atoms in a compound






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






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






7. 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-






8. 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.






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






10. 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






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






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






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






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






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






16. Chalcogens - - Oxide O






17. 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






18. 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.






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






21. 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






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






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






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


25. 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.






26. 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






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






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






29. 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






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






31. 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.






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






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






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






35. 2.18 x 10^-18 J/electron






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






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






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






39. 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






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






41. 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






42. 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






43. The lowest allowable energy state of an atom






44. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






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






47. 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.






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






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






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