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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.
  • 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 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.






2. An atom or group of atoms that has a positive or negative charge






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






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






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






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






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






8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






9. A reaction where a compound does Not change its molecular structure.






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






11. Rare earth element group (elements 58-71)






12. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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






14. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






15. 5 different orbitals shaped like clover leaves and max electrons is 10






16. 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.






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






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






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






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






21. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






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






25. 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.






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






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






28. Chalcogens - - Oxide O






29. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






31. 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






32. A solution in which water is the solvent






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






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






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






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


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






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






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






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






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






42. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






43. 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.






44. 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.






45. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






46. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






48. 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






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






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