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






2. 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






3. 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.






4. 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






5. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






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






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






9. 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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10. 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.






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






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






13. Chalcogens - - Oxide O






14. Property of the elements that can be predicted from the arrangement of the periodic table






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






16. 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






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






18. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






19. Elements in the middle of the periodic table - in groups 3-12.






20. Small discrete increments of energy.






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






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






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






25. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






27. 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






28. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






29. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






30. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






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






34. Simplest whole # ration of atoms in a compound






35. The maximum amount of product that can be produced from a given amount of reactant






36. 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.






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






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






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






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






41. 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.






42. 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

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






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






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






46. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






47. E=hc/?






48. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






50. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.