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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. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






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






4. 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






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






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






7. Named after their cation and anion






8. 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






9. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






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






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






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






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






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






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






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






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






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






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






22. 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.






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






24. 2.18 x 10^-18 J/electron






25. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






27. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






28. Sum of the protons and neutrons in an element often denoted by the letter A






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






30. 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






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






32. 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


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






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






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






36. 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.






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






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






39. 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.






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






41. 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






42. Small discrete increments of energy.






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






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






45. 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






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






47. An ionic compound that resists changes in its pH






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






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






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