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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 weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






3. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






4. Simplest whole # ration of atoms in a compound






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






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






7. 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






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






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






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






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






12. 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.






13. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






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






16. 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






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






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






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






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






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






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






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






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






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






26. 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.






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






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






29. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






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






32. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






34. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






35. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






36. 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






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






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






39. Named after their cation and anion






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






41. An ionic compound that resists changes in its pH






42. 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.






43. 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-






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






45. 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






46. 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






47. The process of decomposing a chemical compound by the passage of an electric current.






48. Chalcogens - - Oxide O






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






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







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