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






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






3. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






4. 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.






5. 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






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






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






8. 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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9. 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






10. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






16. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






17. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






19. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






20. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






21. A horizontal row of elements in the periodic table






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






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






24. 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.






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






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






27. 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






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






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






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






31. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






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






34. 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






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






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






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






39. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






40. 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.






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






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






43. 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.






44. 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






45. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






46. Tells you how much solute is present compared to the amount of solvent






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






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






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






50. 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







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