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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. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






3. The lowest allowable energy state of an atom






4. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






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

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






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






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






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






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






12. 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






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






14. 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.






15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






16. Two or more atoms held together by covalent bonds






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






18. 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






19. 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.






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






21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






23. 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






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






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






26. 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






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






28. 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






29. 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






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






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






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






33. Named after their cation and anion






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






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






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






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






38. 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.






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






40. Small discrete increments of energy.






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






42. 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






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






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






45. 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






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






47. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






49. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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