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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. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






3. 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.






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






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


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






7. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






9. 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






10. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






11. E=hc/?






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






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






14. A dynamic condition in which two opposing changes occur at equal rates in a closed system






15. 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.






16. 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






17. Chalcogens - - Oxide O






18. The slowest elementary step which is the limit for the rate of the other steps






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






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






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






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






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






24. The lowest allowable energy state of an atom






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






26. (chemistry) p(otential of) H(ydrogen)






27. Named after their cation and anion






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






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






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


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. 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-






33. 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.






34. 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.






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






36. 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






37. 2.18 x 10^-18 J/electron






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






39. 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.






40. A reaction in which atoms of one element take the place of atoms of another element in a compound






41. Small discrete increments of energy.






42. 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






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






44. 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.






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






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






49. The energy required to break a chemical bond and form neutral isolated atoms






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