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






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






3. 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






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






5. 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






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






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






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






9. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






10. 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.






11. 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






12. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






13. 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






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






15. In a solution - the substance that dissolves in the solvent






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






17. 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






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






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






21. 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.






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






23. E=hc/?






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






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






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






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






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






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






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






31. 5 different orbitals shaped like clover leaves and max electrons is 10






32. 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






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






34. 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.






35. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






36. (chemistry) p(otential of) H(ydrogen)






37. 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.






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






39. 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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40. 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






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






42. 2.18 x 10^-18 J/electron






43. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






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






46. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






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






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






49. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






50. Substance in which a solute is dissolved to form a solution