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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 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.






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






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






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






5. 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






6. 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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7. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






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






10. 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






11. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






12. 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






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






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

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






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






17. 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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18. 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.






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






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






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






23. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






24. 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.






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






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






27. 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






28. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






29. 2.18 x 10^-18 J/electron






30. 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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31. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






32. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






35. 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






36. A base that can accept two moles of H+ per mole of itself (ex: SO4






37. The lowest allowable energy state of an atom






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






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






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






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






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






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






44. 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






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






46. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






48. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






49. 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






50. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge