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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.
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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. 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






2. 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.






3. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






5. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






6. E=hc/?






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






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






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






10. Tells you how much solute is present compared to the amount of solvent






11. 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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12. A substance that - when dissolved in water - results in a solution that can conduct electricity






13. 5 different orbitals shaped like clover leaves and max electrons is 10






14. The lowest allowable energy state of an atom






15. 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.






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






17. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






18. 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.






19. 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.






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






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






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






23. 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






24. 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






25. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






26. A solid made up of particles that are not arranged in a regular pattern.






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






28. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






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






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






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






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






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






35. 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






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. Having characteristics of both an acid and a base and capable of reacting as either






38. 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.






39. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






40. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






41. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






43. Redox reaction - in which the same species is both oxidized and reduced.






44. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






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






46. Small discrete increments of energy.






47. 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






48. 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.






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






50. Simplest whole # ration of atoms in a compound