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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. Electronegativities _______ as you go down a group.






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






3. 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






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






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






6. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






7. The vapor pressure increases with increasing _____.






8. 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.






9. 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.






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






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






12. 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.






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






14. 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






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






16. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






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






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






19. 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.






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






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






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






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






24. 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.






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






26. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






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






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






29. 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.






30. 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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31. 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).






32. 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.






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






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






36. 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.






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






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






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






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






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






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






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






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






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






46. 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.






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






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






49. Cells that convert electrical energy into chemical energy.






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