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






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






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






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






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






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






7. The vapor pressure increases with increasing _____.






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






9. 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.






10. Electronegativities _______ as you go down a group.






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






12. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






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






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

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15. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






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






17. 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.






18. 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






19. 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






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






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






23. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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






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






26. 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.






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






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






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






30. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






31. 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.






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






33. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






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






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






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






37. The pressure exerted by each gas in a mixture is called its _____ pressure.






38. 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.






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






40. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






41. *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.






42. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






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






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






45. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






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






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






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