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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. A horizontal row of elements in the periodic table






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






3. Having characteristics of both an acid and a base and capable of reacting as either






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






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






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






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






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






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






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






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






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






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






14. 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






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






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






17. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






18. 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.






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






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






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






22. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






23. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






24. Substance in which a solute is dissolved to form a solution






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






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






27. E=hc/?






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






29. 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






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






31. A substance that - when dissolved in water - results in a solution that can conduct electricity






32. 2.18 x 10^-18 J/electron






33. Chalcogens - - Oxide O






34. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






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






37. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






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






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






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






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






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






43. 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






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






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






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. 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






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






50. Small discrete increments of energy.