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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.
  • 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. 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






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






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






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

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






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






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






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






9. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






11. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






12. Common definition of acids as proton (H+) donors and bases as proton acceptors






13. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






14. A horizontal row of elements in the periodic table






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






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






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






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






19. Named after their cation and anion






20. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






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






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






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






25. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






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






27. 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.






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






29. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






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






31. 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.






32. 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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33. 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.






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

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35. 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






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






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






38. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






39. 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.






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






41. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






42. 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.






43. 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






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






45. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






48. 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






49. 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






50. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.