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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.
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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 ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






3. Chalcogens - - Oxide O






4. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






6. 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






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






8. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






10. A solution in which water is the solvent






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






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






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






14. 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






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






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






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






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






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






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






21. 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.






22. 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.






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






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






26. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






27. 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






28. Named after their cation and anion






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






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






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






32. 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.






33. 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






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






35. 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.






36. 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.






37. Two or more atoms held together by covalent bonds






38. Small discrete increments of energy.






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






40. 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-






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

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42. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






43. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






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






46. 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






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






48. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






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