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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. An ionic compound that resists changes in its pH






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






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






4. 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.






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






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






7. 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






8. A horizontal row of elements in the periodic table






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






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






11. 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






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

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13. Chalcogens - - Oxide O






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






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






16. 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






17. 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






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






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






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






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






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






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






24. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






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






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






28. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






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






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






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






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






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






34. 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.






35. 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






36. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






37. 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






38. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






39. The lowest allowable energy state of an atom






40. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






41. Simplest whole # ration of atoms in a compound






42. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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






45. 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






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






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






48. The percent by mass of each element in a compound






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






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