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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. 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.






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






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






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






6. 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






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






8. 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






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






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






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






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






13. 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






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






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






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






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






18. 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






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






20. Chalcogens - - Oxide O






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






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






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






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






25. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






26. 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.






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






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






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






30. 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






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






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






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






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






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






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






37. 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






38. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






40. Small discrete increments of energy.






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






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






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






44. Two or more atoms held together by covalent bonds






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






46. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






47. 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






48. 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.






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






50. The slowest elementary step which is the limit for the rate of the other steps