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






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






3. 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






4. 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






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






6. 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.






7. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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

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9. An ionic compound that resists changes in its pH






10. 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.






11. 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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12. 2.18 x 10^-18 J/electron






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






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






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






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






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






18. Two or more atoms held together by covalent bonds






19. 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






20. A horizontal row of elements in the periodic table






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






22. 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.






23. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






24. The lowest allowable energy state of an atom






25. A reaction where a compound does Not change its molecular structure.






26. 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.






27. Chalcogens - - Oxide O






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 representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






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






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






33. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






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






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






36. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






37. 5 different orbitals shaped like clover leaves and max electrons is 10






38. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






39. 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






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






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






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






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






44. 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






45. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






46. 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






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






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






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






50. A base that can accept two moles of H+ per mole of itself (ex: SO4