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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. 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.






2. 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.






3. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






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






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






14. Electronegativities _______ as you go down a group.






15. 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.






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






17. 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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18. *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.






19. 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).






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






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






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






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






24. 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.






25. The freezing point is always lowered by addition of solute.






26. 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.






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






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






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






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






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






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






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






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






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






36. 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






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






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






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






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






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






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






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






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

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46. A hypothetical gas would follow Boyles law under all conditions and is called?






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






48. 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






49. Metals have electronegativities less than ____






50. When the rate of evaporation equals the rate of condensation - the system is in __________.