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






2. Small discrete increments of energy.






3. A horizontal row of elements in the periodic table






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






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






6. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






8. 2.18 x 10^-18 J/electron






9. 5 different orbitals shaped like clover leaves and max electrons is 10






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






11. 5 valence electrons -3 ions - Nitride N






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






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






14. Two or more atoms held together by covalent bonds






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






16. 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-






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






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






20. 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.






21. 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.






22. 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


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






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






25. 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






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






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






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






29. The lowest allowable energy state of an atom






30. An ionic compound that resists changes in its pH






31. 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






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






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






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






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






36. 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






37. 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.






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






39. An atom or group of atoms that has a positive or negative charge






40. 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






41. 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.






42. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






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






44. 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.






45. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






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






47. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






49. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






50. 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.