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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. 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






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






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






4. Named after their cation and anion






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






6. 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.






7. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






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






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






11. 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.






12. 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






13. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






14. A horizontal row of elements in the periodic table






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






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






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. Rare earth element group (elements 58-71)






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






20. Any sample of a given compound will contain the same elements in the identical mass ratio.






21. 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.






22. 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.






23. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






24. E=hc/?






25. 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.






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






27. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






28. 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.






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






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






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






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






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






34. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






35. 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






36. Chalcogens - - Oxide O






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






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






40. The lowest allowable energy state of an atom






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






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






43. 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






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






45. Small discrete increments of energy.






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






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






48. The process of decomposing a chemical compound by the passage of an electric current.






49. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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