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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. 2.18 x 10^-18 J/electron






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






3. Property of the elements that can be predicted from the arrangement of the periodic table






4. In a solution - the substance that dissolves in the solvent






5. 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.






6. 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






7. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






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






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






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






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






13. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






14. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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15. 5 valence electrons -3 ions - Nitride N






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






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






18. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






20. 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.






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






23. 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.






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






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






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






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






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

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






30. Numbers that specify the properties of atomic orbitals and of their electrons






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






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






33. 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






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






35. A solution in which water is the solvent






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






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






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






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






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






41. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






43. 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






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






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






46. 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.






47. Named after their cation and anion






48. Two or more atoms held together by covalent bonds






49. 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






50. The lowest allowable energy state of an atom