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






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






3. The vapor pressure increases with increasing _____.






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






5. 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






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






7. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






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






9. 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).






10. 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).






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






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






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






14. 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.






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






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






17. *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.






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






19. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






20. 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






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






22. 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.






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






24. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






25. 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.






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






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






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






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






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






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






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






33. 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.






34. Metals have electronegativities less than ____






35. 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.






36. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.






37. 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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38. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






39. *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.






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






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






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






43. 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.






44. 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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45. The change in enthalpy of an exothermic reaction is ________.






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






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






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






49. 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.






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