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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. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






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






3. 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






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






5. 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






6. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






7. 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






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






9. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






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






11. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






13. A dynamic condition in which two opposing changes occur at equal rates in a closed system






14. The maximum amount of product that can be produced from a given amount of reactant






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






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






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






18. 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.






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






20. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






24. 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.






25. 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






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






27. Two or more atoms held together by covalent bonds






28. 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.






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






30. 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.






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






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






33. A base that can accept two moles of H+ per mole of itself (ex: SO4






34. 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.






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






36. 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






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. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






39. 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






40. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






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






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






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






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






45. Simplest whole # ration of atoms in a compound






46. 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






47. Chalcogens - - Oxide O






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






49. 5 valence electrons -3 ions - Nitride N






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