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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. 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.






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






3. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






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






5. 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.






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






7. 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.






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






9. 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






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






11. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






13. The slowest elementary step which is the limit for the rate of the other steps






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






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






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






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






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






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






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






21. An ionic compound that resists changes in its pH






22. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






23. Small discrete increments of energy.






24. 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






25. 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






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






28. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






30. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






32. 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.






33. 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






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






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






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






37. E=hc/?






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






39. An atom or group of atoms that has a positive or negative charge






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






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






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






43. 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.






44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






45. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






46. 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






47. 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.






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






50. 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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