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






2. 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






3. 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.






4. 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






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






7. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






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






10. The lowest allowable energy state of an atom






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






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






13. 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.






14. 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.






15. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






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






17. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






19. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






20. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






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






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






24. 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.






25. 2.18 x 10^-18 J/electron






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






27. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






28. 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






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






30. 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.






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






32. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






33. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






34. 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






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






36. Chalcogens - - Oxide O






37. 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






38. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






41. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






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






44. 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.






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






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

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47. 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






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






49. 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






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







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