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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • 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. The slowest elementary step which is the limit for the rate of the other steps






2. 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






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






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






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






6. 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.






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






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






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






10. 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






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






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






13. 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






14. Small discrete increments of energy.






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






16. Named after their cation and anion






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. E=hc/?






20. 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






21. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






22. 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.






23. 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


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






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






26. 5 different orbitals shaped like clover leaves and max electrons is 10






27. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






28. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






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


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






31. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






32. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






33. 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






34. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






35. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






36. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






38. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






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






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






42. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






44. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






46. 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.






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






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






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






50. 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