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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. 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






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






3. 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






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






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






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






7. 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.






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






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






10. 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.






11. 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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12. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






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






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






15. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






16. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






18. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






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






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

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






22. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






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






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






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






26. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






27. 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.






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






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






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






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






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






33. 2.18 x 10^-18 J/electron






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






35. 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.






36. 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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37. 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






38. 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






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






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






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






42. (chemistry) a substance that changes color to indicate the presence of some ion or substance






43. Small discrete increments of energy.






44. 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.






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






46. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






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






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






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






Can you answer 50 questions in 15 minutes?



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