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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. 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






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






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






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






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






6. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






8. Named after their cation and anion






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






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






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






12. 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.






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. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






15. 5 valence electrons -3 ions - Nitride N






16. 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.






17. Simplest whole # ration of atoms in a compound






18. 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






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






20. The average distance between the nuclei of two bonded atoms






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






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






23. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






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






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






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






27. 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






28. 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






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






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






31. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






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






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






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






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






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






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






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






39. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






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






42. 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.






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


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






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


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






47. 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






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






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






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