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






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






3. 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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4. 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.






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






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






7. *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.






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






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






10. 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.






11. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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






14. *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.






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






16. *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.






17. 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.






18. *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






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






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






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






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






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






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






25. 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.






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






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






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






29. 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).






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






31. 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






32. Cells that convert electrical energy into chemical energy.






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






34. 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.






35. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






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






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






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






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






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






42. 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






43. 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.






44. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






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






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






47. 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.






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






49. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






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