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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. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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2. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






3. When the electron moves from the ground state to an excited state - it ______ energy.






4. The heat required to change 1mole of solid completely to vapor.






5. 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.






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






7. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






8. 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.






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






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






11. 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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12. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






13. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






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






16. 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.






17. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






18. Cells that convert electrical energy into chemical energy.






19. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






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






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






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






23. The most active nonmetals are found in what corner of the periodic table?






24. The change in enthalpy of an endothermic reaction is ________.






25. A solution in which solid solute is in equilibrium with dissolved solute.






26. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






27. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






28. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






29. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






30. The heat change during a process carried out at a constant pressure.






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






32. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






33. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






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






36. _____ bonds are present in molecules containing double or triple bonds.






37. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






38. In an exothermic process - energy is released and ^E of reaction is ________.






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






40. Electronegativities _______ as you go down a group.






41. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






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






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






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






45. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






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






47. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






48. 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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49. This process occurs when the system is thermally isolated so that no heat enters or leaves.






50. *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