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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. A definite stable energy that a physical system can have






2. 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






3. 2.18 x 10^-18 J/electron






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






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






6. 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.






7. The lowest allowable energy state of an atom






8. 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


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






10. 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






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






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






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






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






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






16. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






17. 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.






18. Simplest whole # ration of atoms in a compound






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






20. Named after their cation and anion






21. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






22. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






25. 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






26. E=hc/?






27. A solid made up of particles that are not arranged in a regular pattern.






28. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






30. 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






31. 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






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






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






34. 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






35. 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






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






37. 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






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. Rare earth element group (elements 58-71)






40. The Percent by mass of each element in a compound.






41. 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.






42. 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.






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






44. 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






45. 5 valence electrons -3 ions - Nitride N






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






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






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






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






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