Test your basic knowledge |

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. 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






2. 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.






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






4. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






5. An elementary particle with 0 charge and mass about equal to a proton






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






7. 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.






8. The lowest allowable energy state of an atom






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






10. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






11. Simplest whole # ration of atoms in a compound






12. 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.






13. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






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






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






18. 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.






19. 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.






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






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






22. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






23. 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.






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






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






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






27. 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






28. E=hc/?






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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






31. Small discrete increments of energy.






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






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






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






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






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






38. 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






39. Chalcogens - - Oxide O






40. 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






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






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






43. 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






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






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






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






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






48. 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






49. 2.18 x 10^-18 J/electron






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