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






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






3. 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-






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






5. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






6. 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






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






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






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






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






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






12. Chalcogens - - Oxide O






13. 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






14. Named after their cation and anion






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






16. 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.






17. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






18. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






19. 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






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






21. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






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






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






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






26. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






27. 5 different orbitals shaped like clover leaves and max electrons is 10






28. 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.






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






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






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






32. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






33. 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.






34. The process by which one or more substances change to produce one or more different substances






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






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






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






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






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






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






41. 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






42. 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.






43. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






44. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






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






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






48. 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






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






50. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.