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






2. 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.






3. Two or more atoms held together by covalent bonds






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






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






6. 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






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






8. 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






9. 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






10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






11. PH of a molecule at which it contains no net electric charge - isoelectric point.






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






13. 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.






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






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






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

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


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






18. The percent by mass of each element in a compound






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






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






21. A horizontal row of elements in the periodic table






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






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






24. 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

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


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






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






27. 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






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






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






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






31. Simplest whole # ration of atoms in a compound






32. An ionic compound that resists changes in its pH






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






34. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






37. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






38. Small discrete increments of energy.






39. 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






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






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






42. 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






43. Gram equivalent weight of solute per liter of solution - often denoted by N.






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. 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.






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






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






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






49. Named after their cation and anion






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