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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. 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






2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






4. 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






5. 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






6. 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






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






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






9. Small discrete increments of energy.






10. Chalcogens - - Oxide O






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. The lowest allowable energy state of an atom






13. Simplest whole # ration of atoms in a compound






14. The percent by mass of each element in a compound






15. A solution in which water is the solvent






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






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






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






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






20. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






21. Gram equivalent weight of solute per liter of solution - often denoted by N.






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






23. 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






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






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






26. 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.






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






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






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






30. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






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






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






33. 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.






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






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






36. 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






37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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






41. 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

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






43. 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






44. The average distance between the nuclei of two bonded atoms






45. 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.






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






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






48. Named after their cation and anion






49. An ionic compound that resists changes in its pH






50. 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