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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. A definite stable energy that a physical system can have






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






3. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






4. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






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






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






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






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






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






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






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






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






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






15. 2.18 x 10^-18 J/electron






16. 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






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






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






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






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






22. The process of decomposing a chemical compound by the passage of an electric current.






23. (chemistry) a substance that changes color to indicate the presence of some ion or substance






24. 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






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






26. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






27. 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






28. 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






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

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30. 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.






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






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






33. An ionic compound that resists changes in its pH






34. 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






35. 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






36. 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






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






38. Chalcogens - - Oxide O






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






40. 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.






41. A horizontal row of elements in the periodic table






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






43. 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.






44. 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






45. 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.






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






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






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






49. 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.






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