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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • 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. An ionic compound that resists changes in its pH






2. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






4. 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






5. 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






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






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

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9. 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






10. 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






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






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






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






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






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






16. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






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






19. E=hc/?






20. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






21. 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.






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






23. 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.






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






25. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






26. 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






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






28. 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.






29. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






30. Rare earth element group (elements 58-71)






31. Small discrete increments of energy.






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






33. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






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






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






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






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






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






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






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






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






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






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






45. Chalcogens - - Oxide O






46. 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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47. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






48. 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






49. 5 different orbitals shaped like clover leaves and max electrons is 10






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