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






2. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






3. 2.18 x 10^-18 J/electron






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






5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






6. 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.






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






8. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


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






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






11. 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


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


13. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






15. 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


16. 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.






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






18. 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






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






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






21. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






22. 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






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






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






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






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






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






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






29. 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






30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






32. 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.






33. 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






34. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






35. 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.






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






37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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






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






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






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






44. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






45. A solution in which water is the solvent






46. 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






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






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






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






50. 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