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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. Having characteristics of both an acid and a base and capable of reacting as either






2. 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






3. E=hc/?






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






5. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






6. A horizontal row of elements in the periodic table






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






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






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






10. Slightly less reactive than alkali metals - comprise group II






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






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






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






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






15. 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






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






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






18. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






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






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






21. Chalcogens - - Oxide O






22. 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.






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






24. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin


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






26. Small discrete increments of energy.






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






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


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






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






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






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






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






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






35. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






37. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






38. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






40. 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


41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






43. Simplest whole # ration of atoms in a compound






44. 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






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






46. 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.






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






48. 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






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






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