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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. 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






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






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






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






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

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6. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






7. Simplest whole # ration of atoms in a compound






8. 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






9. 5 different orbitals shaped like clover leaves and max electrons is 10






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






11. 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






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

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






14. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






15. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






16. 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






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






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






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






20. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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






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






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






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






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






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






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






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






31. 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






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






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






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






35. 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.






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






37. 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






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






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






40. 5 valence electrons -3 ions - Nitride N






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






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






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






44. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






45. A subdivision of an energy level in an atom. They are divided into orbitals.






46. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






47. 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






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






49. The lowest allowable energy state of an atom






50. 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.