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






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






3. The lowest allowable energy state of an atom






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






5. Redox reaction - in which the same species is both oxidized and reduced.






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






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. 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.






9. 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






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






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






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






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






14. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






16. Small discrete increments of energy.






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






18. 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






19. Chalcogens - - Oxide O






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






21. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






23. 5 valence electrons -3 ions - Nitride N






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






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






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






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






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






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






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






31. 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.






32. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






35. 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






36. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






37. A solution in which water is the solvent






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






39. 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.






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






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






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






44. 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






45. Named after their cation and anion






46. 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






47. Simplest whole # ration of atoms in a compound






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

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






50. 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