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






2. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






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






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






9. An ionic compound that resists changes in its pH






10. Named after their cation and anion






11. 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






12. The lowest allowable energy state of an atom






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






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






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






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






17. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






18. Slightly less reactive than alkali metals - comprise group II






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






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






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






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






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






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






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






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






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






29. A solution in which water is the solvent






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






31. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






32. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






33. 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.






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






35. E=hc/?






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

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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. Having characteristics of both an acid and a base and capable of reacting as either






39. 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






40. 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.






41. 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-






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






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






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






45. 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






46. 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.






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






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






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






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