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






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






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

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






5. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






6. The process of decomposing a chemical compound by the passage of an electric current.






7. Small discrete increments of energy.






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






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






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






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






12. An ionic compound that resists changes in its pH






13. 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-






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

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






16. 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






17. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






18. 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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19. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






20. 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






21. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






23. 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.






24. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






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






27. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






28. Redox reaction - in which the same species is both oxidized and reduced.






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






30. 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






31. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






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






33. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






34. 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






35. 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






36. 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.






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






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






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






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






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






43. The energy required to break a chemical bond and form neutral isolated atoms






44. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






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






47. The percent by mass of each element in a compound






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






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






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