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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. E=hc/?






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






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






4. 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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5. An elementary particle with 0 charge and mass about equal to a proton






6. 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






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






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






9. 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






10. 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.






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






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






13. 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






14. 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






15. 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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16. The percent by mass of each element in a compound






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






18. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






19. 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






20. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






21. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






23. 5 valence electrons -3 ions - Nitride N






24. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






25. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






26. 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






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






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






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

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






31. 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






32. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






33. 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-






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






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






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






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






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






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






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






41. Small discrete increments of energy.






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






43. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






44. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






45. (chemistry) p(otential of) H(ydrogen)






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






47. 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.






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






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






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







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