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






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






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






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






5. Tells you how much solute is present compared to the amount of solvent






6. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






7. 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.






8. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






9. Named after their cation and anion






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






11. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






12. 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-






13. 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






14. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






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






17. 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






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






19. 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






20. 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






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






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






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






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


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






26. Temperature is constant; effusion and temperature are proportional to the square root of their masses


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






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






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






31. A horizontal row of elements in the periodic table






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






33. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






35. 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






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






37. 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






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






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






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






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






42. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






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






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






46. 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






47. 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






48. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






50. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.