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CLEP Chemistry 1

Subjects : clep, science, chemistry
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. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






2. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






3. Electronegativities ________ from left to right in a period.






4. The most active metals are found in what corner of the periodic table?






5. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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6. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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7. Rays made up of electrons in basic electron charges.






8. Rays made up of positive electrodes in basic electron charges.






9. In an endothermic process - energy is absorbed and ^E is _______.






10. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






11. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






12. When an electron moves from an excited state to the ground state - it _______ energy.






13. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






14. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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15. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






16. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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17. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






18. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






19. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






20. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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21. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






22. This process occurs when the system is maintained at the same temperature throughout an experiment.






23. A chemical reaction formed from the union of its elements.






24. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






25. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






26. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.






27. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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28. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






29. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






30. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.






31. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






32. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






33. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






34. A process that occurs whent eh system is maintained at constant pressure.






35. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






36. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






37. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






38. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






39. Electronegativities _______ as you go down a group.






40. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






41. Liquids with strong attractive forces have ______ boiling points.






42. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






43. The change in enthalpy of an exothermic reaction is ________.






44. Heat added to a system and work done by a system are considered _________ quantities.






45. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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46. A state function in which it is the heat content of a substance.






47. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






48. The action of salts of weak acids or bases with water to form acidic or basic solutions.






49. In titration - this is the point at which a particular indicator changes color.






50. The molecules in a gas are in constant - continueous - random - and straight-line motion.