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






2. 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






3. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






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






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






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






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






10. 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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11. The lowest allowable energy state of an atom






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






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






14. A solid made up of particles that are not arranged in a regular pattern.






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






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






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. In a solution - the substance that dissolves in the solvent






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

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






22. 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






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






24. 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.






25. Named after their cation and anion






26. 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






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






28. The average distance between the nuclei of two bonded atoms






29. 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






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






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






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






33. 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-






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






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






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






38. 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.






39. 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






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






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






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






43. 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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44. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






46. 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






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






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






49. 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






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