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






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






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






4. 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.


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






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






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






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






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






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






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






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






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






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






15. 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






16. 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.






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






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






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






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






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






22. 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.






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






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


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






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






27. 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).






28. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






29. 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.


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






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






32. 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.






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






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






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






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






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






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






39. *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.






40. 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.






41. *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






42. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






44. 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.






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






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






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






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






49. 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.






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