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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. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






2. 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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3. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






6. 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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7. The change in enthalpy of an endothermic reaction is ________.






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






9. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






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






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






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






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






17. Electronegativities _______ as you go down a group.






18. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






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






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






21. 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.






22. *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






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






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






25. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






26. Deviations from Boyles law that occur with real gases represent _______ behavior.






27. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






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






29. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






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






31. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






32. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






33. 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






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






35. 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.






36. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






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






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

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






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






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






42. The energy required to remove an electron from an isolated atom in its ground state.






43. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






46. **Proceeding across a period from left to right - the ionization energy _______.






47. The temperature at which a substance's solid and liquid phases are in equilibrium.






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






49. *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.






50. 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.