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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. 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.






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

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






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






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






6. A definite stable energy that a physical system can have






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






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






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






10. 2.18 x 10^-18 J/electron






11. 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






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






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






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






15. 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






16. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






17. 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.






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






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






20. 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






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






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






23. 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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24. 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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25. 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.






26. 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






27. 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






28. 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






29. The maximum amount of product that can be produced from a given amount of reactant






30. Common definition of acids as proton (H+) donors and bases as proton acceptors






31. The lowest allowable energy state of an atom






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






33. An elementary particle with 0 charge and mass about equal to a proton






34. 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






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






36. 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.






37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






39. 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.






40. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






41. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






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






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






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






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






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

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49. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






50. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.